m/c QUIZ of chemical calculations for harder-higher
tier GCSE level (includes moles)
Given the following relative atomic masses: Cu = 64, S = 32 and O = 16; calculate the relative formula mass of copper
sulfate, CuSO4 [rfm-1]
160
112
96
336
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of ethane, C2H6 [rfm-2]
13
30
18
25
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of octane, C8H18 [rfm-3]
13
96
114
112
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of nitric acid, HNO3 [rfm-4]
31
93
62
63
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH4NO3 [rfm-5]
80
31
90
180
Given the following relative atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the relative formula mass of ammonium
sulfate, (NH4)2SO4 [rfm-6]
63
132
216
100
Given the following relative atomic masses: H = 1, O = 16 and S = 32; calculate the relative formula mass of
sulfuric acid, H2SO4 [rfm-7]
49
194
98
66
Given the following relative atomic masses: O = 16, Al = 27 and S = 32; calculate the relative formula mass of aluminium
sulfate, Al2(SO4)3 [rfm-8]
75
315
171
342
Given the following relative atomic masses: H = 1 and Cl = 35.5, calculate the relative formula mass of hydrochloric acid, HCl [rfm-9]
36.5
18
35.5
37.5
Given the following relative atomic masses: Na = 23 and Cl = 35.5, calculate the relative formula mass of sodium chloride, NaCl [rfm-10]
40
58.5
49.5
35
Given the following relative atomic masses: Ca = 40 and Cl = 35.5, calculate the relative formula mass of calcium chloride, CaCl2 [rfm-11]
75.5
151
111
146.5
Given the following relative atomic masses: H = 1, O = 16 and Mg = 24, calculate the relative formula mass of magnesium hydroxide, Mg(OH)2 [rfm-12]
41
82
42
58
Given the following relative atomic masses: Al = 27 and Cl = 35.5, calculate the relative formula mass of aluminium chloride, AlCl3 [rfm-13]
133.5
62.5
187.5
98
Given the following relative atomic masses: H = 1, O = 16 and Al = 27, calculate the relative formula mass of aluminium hydroxide, Al(OH)3 [rfm-14]
44
78
132
46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of glucose, C6H12O6 [rfm-5]
29
40
180
90
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanol ('alcohol'), C2H5OH [rfm-16]
29
23
41
46
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanoic acid ('acetic acid'), CH3COOH [rfm-17]
60
29
84
58
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(II) oxide, FeO [rfm-18]
40
72
56
16
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(III) oxide, Fe2O3 [rfm-19]
72
200
160
216
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of the iron oxide, Fe3O4 [rfm-20]
72
272
174
232
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of methane, CH4 [rfm-21]
16
13
52
10
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of propane, C3H8 [rfm-22]
13
44
99
40
Given the following relative atomic masses: C = 12 and O = 16; calculate the relative molecular mass of carbon dioxide, CO2 [rfm-23]
28
56
44
14
Given the following relative atomic masses: C = 12, O = 16 and Cu = 64; calculate the relative formula mass of copper carbonate, CuCO3 [rfm-24]
92
276
148
124
Given the following relative atomic masses: C = 12, O = 16 and Ca = 40; calculate the relative formula mass of calcium carbonate, CaCO3 [rfm-25]
100
68
204
124
Given the following symbol equation: 2Mg + O2 ==> 2MgO Calculate how many g of magnesium oxide is formed by burning 24g of magnesium in air. (Relative atomic masses, Ar: Mg = 24 and O = 16) [com-1]
40
16
20
80
Given the following symbol equation: 2Mg + O2 ==> 2MgO Calculate how many tonne of magnesium is needed to make 80 tonne of magnesium oxide. (Relative atomic masses, Ar: Mg = 24 and O = 16) [com-2]
96
48
24
16
Given the following symbol equation: CaCO3(s) ==> CaO(s) + CO2(g) Calculate how many kg of calcium carbonate is needed to make 56 kg of calcium oxide. (Relative atomic masses, Ar: Ca = 40, C = 12 and O = 16) [com-3]
50
44
100
40
Given the following symbol equation: CaCO3(s) ==> CaO(s) + CO2(g) Calculate how many g of carbon dioxide is formed if 25g of calcium carbonate is decomposed on heating to form 14g of calcium oxide. (Relative atomic masses, Ar: Ca = 40, C = 12 and O = 16) [com-4]
22
44
10
11
Given the symbol equation to show the formation of iron
sulfide: Fe + S ==> FeS Calculate the mass in g of iron sulfide formed when 5.6g of iron combines with 3.2g of
sulfur. (Relative atomic masses, Ar: Fe = 56 and S = 32) [com-5]
8.8
2.4
5.6
3.2
Given the symbol equation to show the formation of iron
sulfide: Fe + S ==> FeS Calculate the mass in g of iron sulfide formed when 28g of iron combines with 16g of
sulfur. (Relative atomic masses, Ar: Fe = 56 and S = 32) [com-6]
12
44
28
16
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine: Ca(s) + Cl2(g) ==> CaCl2(s) Calculate the mass in g of calcium chloride formed when 20g of calcium combines with 35.5g of chlorine. (Relative atomic masses, Ar: Ca = 40 and Cl = 35.5) [com-7]
15.5
70.0
55.5
17.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine: Ca(s) + Cl2(g) ==> CaCl2(s) Calculate the mass in g of chlorine needed when 40g of calcium forms 111g of calcium chloride. (Relative atomic masses, Ar: Ca = 40 and Cl = 35.5) [com-8]
80
100
151
71
Given the symbol equation to show the formation of aluminium
sulfide by heating a mixture of aluminium and sulfur: 2Al + 3S ==> Al2S3 How many g of
sulfur is needed if 54g of aluminium is reacted to form 150g of aluminium
sulfide? (Relative atomic masses, Ar: Al = 27 and S = 32) [com-9]
96
204
64
27
Given the symbol equation to show the formation of aluminium
sulfide by heating a mixture of aluminium and sulfur: 2Al + 3S ==> Al2S3 How many kg of
sulfur is needed if 108kg of aluminium is reacted to form 300kg of aluminium
sulfide? (Relative atomic masses, Ar: Al = 27 and S = 32) [com-10]
408
192
96
32
Given the symbol equation to show the formation of iron
sulfide by heating a mixture of iron and sulfur: Fe + S ==> FeS Calculate the mass in g of iron unreacted when 60g of iron reacts with 32g of
sulfur to form 88g of iron sulfide. (Relative atomic masses, Ar: Fe = 56 and S = 32) [com-11]
8
32
4
56
Given the symbol equation to show the formation of iron
sulfide by heating a mixture of iron and sulfur: Fe + S ==> FeS Calculate the mass in g of
sulfur unreacted when 28g of iron reacts with 22g of sulfur to form 44g of iron
sulfide. (Relative atomic masses, Ar: Fe = 56 and S = 32) [com-12]
22
16
12
6
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine: Ca(s) + Cl2(g) ==> CaCl2(s) Calculate the mass in g of calcium left unreacted when 25g of calcium reacts with 35.5g of chlorine. (Relative atomic masses, Ar: Ca = 40 and Cl = 35.5) [com-13]
10.5
5.0
7.1
12.5
Given the symbol equation to show the formation of calcium chloride by burning calcium in chlorine: Ca(s) + Cl2(g) ==> CaCl2(s) Calculate the mass in g of chlorine left unreacted when 80g of calcium reacts with 150g of chlorine to form 222g of calcium chloride. (Relative atomic masses, Ar: Ca = 40 and Cl = 35.5) [com-14]
70
8
16
72
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of copper in copper(II)
sulfate, CuSO4 [pbm-1]
40.0
16.7
64.0
16.0
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in ethane, C2H6 [pbm-2]
25
80
24
20
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in octane, C8H18 [pbm-3]
30.8
96.0
84.2
80.0
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of hydrogen in nitric acid, HNO3 [pbm-4]
20.0
1.0
3.0
1.6
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of hydrogen in ammonium nitrate, NH4NO3 [pbm-5]
5.0
44.4
4.0
50.0
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of nitrogen in ammonium
sulfate, (NH4)2SO4 [pbm-6]
53.3
21.2
14.0
28.0
Given the atomic masses: H = 1, O = 16 and S = 32; calculate the % by mass of hydrogen in
sulfuric acid, H2SO4 [pbm-7]
28.6
2.1
2.0
20.0
Given the atomic masses: O = 16, Al = 27 and S = 32; calculate the % by mass of aluminium in aluminium
sulfate, Al2(SO4)3 [pbm-8]
7.9
27
54
15.8
Given the atomic masses: H = 1 and Cl = 35.5, calculate the % by mass of hydrogen in hydrogen chloride, HCl [pbm-9]
2.7
50.0
96.3
1.0
Given the atomic masses: Na = 23 and Cl = 35.5, calculate the % by mass of sodium in sodium chloride, NaCl [pbm-10]
50.0
39.3
23.0
46.0
Given the atomic masses: Ca = 40 and Cl = 35.5, calculate the % by mass of calcium in calcium chloride, CaCl2 [pbm-11]
33.3
40.0
36.0
20.0
Given the atomic masses: H = 1, O = 16 and Mg = 24, calculate the % by mass of magnesium in magnesium hydroxide, Mg(OH)2 [pbm-12]
20.0
24.0
48.0
41.4
Given the atomic masses: Al = 27 and Cl = 35.5, calculate the % by mass of aluminium in aluminium chloride, AlCl3 [pbm-13]
20.2
25.0
27.0
43.2
Given the atomic masses: H = 1, O = 16 and Al = 27, calculate the % by mass of aluminium in aluminium hydroxide, Al(OH)3 [pbm-14]
14.3
34.6
27.0
9.0
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of carbon in glucose, C6H12O6 [pbm-15]
25
7
40
60
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of carbon in ethanol ('alcohol'), C2H5OH [pbm-16]
22.2
24.0
48.0
52.2
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in iron(II) oxide, FeO [pbm-17]
77.8
50.0
56.0
22.2
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in iron(II) oxide, FeO [pbm-18]
50.0
22.2
16.0
77.8
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in iron(III) oxide, Fe2O3 [pbm-19]
40
56
70
48
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in the iron oxide, Fe3O4 [pbm-20]
42.9
56.0
27.6
72.4
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in methane, CH4 [pbm-21]
75
20
12
48
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in propane, C3H8 [pbm-22]
27.3
81.8
36.0
90.3
Given the atomic masses: C = 12 and O = 16; calculate the % by mass of oxygen in carbon dioxide, CO2 [pbm-23]
33.3
32.0
72.7
66.6
Given the atomic masses: C = 12, O = 16 and Cu = 64; calculate % by mass of copper in copper carbonate, CuCO3 [pbm-24]
20.0
64.0
36.0
51.6
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of calcium in calcium carbonate, CaCO3 [pbm-25]
40
20
60
80
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of oxygen in copper(II)
sulfate, CuSO4 [pbm-26]
66.6
40.0
64.0
39.0
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of
sulfur in copper(II) sulfate, CuSO4 [pbm-27]
16.7
16.0
20.0
32.0
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in ethane, C2H6 [pbm-28]
75.0
6.0
7.5
20.0
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in octane, C8H18 [pbm-29]
15.8
69.2
18.0
82.0
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of oxygen in nitric acid, HNO3 [pbm-30]
60.0
76.2
48.0
76.0
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of nitrogen in nitric acid, HNO3 [pbm-31]
14.0
20.0
22.2
42.2
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of nitrogen in ammonium nitrate, NH4NO3 [pbm-32]
22
14
28
35
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of oxygen in ammonium nitrate, NH4NO3 [pbm-33]
60
48
16
40
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of hydrogen in ammonium
sulfate, (NH4)2SO4 [pbm-34]
4.0
6.1
8.0
7.1
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of
sulfur in ammonium sulfate, (NH4)2SO4 [pbm-35]
32.0
24.1
24.2
32.1
Given the atomic masses: H = 1, N = 14, O = 16 and S = 32; calculate the % by mass of oxygen in ammonium
sulfate, (NH4)2SO4 [pbm-36]
16.0
48.0
32.0
48.5
Given the atomic masses: H = 1, O = 16 and S = 32; calculate the % by mass of oxygen in
sulfuric acid, H2SO4 [pbm-37]
65.3
14.3
64.0
32.0
Given the atomic masses: O = 16, Al = 27 and S = 32; calculate the % by mass of
sulfur in aluminium sulfate, Al2(SO4)3 [pbm-38]
27.0
28.1
54.0
54.1
Given the atomic masses: O = 16, Al = 27 and S = 32; calculate the % by mass of oxygen in aluminium
sulfate, Al2(SO4)3 [pbm-39]
16.0
64.0
56.1
57.2
Given the atomic masses: H = 1 and Cl = 35.5, calculate the % by mass of chlorine in hydrogen chloride, HCl [pbm-40]
50.0
35.5
36.5
97.3
Given the atomic masses: Na = 23 and Cl = 35.5, calculate the % by mass of chlorine in sodium chloride, NaCl [pbm-41]
60.7
50.0
35.5
70.0
Given the atomic masses: Ca = 40 and Cl = 35.5, calculate the % by mass of chlorine in calcium chloride, CaCl2 [pbm-42]
66.7
64.0
71.0
35.5
Given the atomic masses: H = 1, O = 16 and Mg = 24, calculate the % by mass of oxygen in magnesium hydroxide, Mg(OH)2 [pbm-43]
40.0
32.0
55.2
60.2
Given the atomic masses: Al = 27 and Cl = 35.5, calculate the % by mass of chlorine in aluminium chloride, AlCl3 [pbm-44]
25.0
75.0
66.7
79.8
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of hydrogen in glucose, C6H12O6 [pbm-45]
6.7
50.0
6.0
12.3
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of oxygen in glucose, C6H12O6 [pbm-46]
25.0
53.3
96.0
16.0
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of hydrogen in ethanol ('alcohol'), C2H5OH [pbm-47]
75
5
13
6
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of oxygen in ethanol ('alcohol'), C2H5OH [pbm-48]
16.0
11.1
40.0
34.8
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in iron(III) oxide, Fe2O3 [pbm-49]
30
48
16
60
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in methane, CH4 [pbm-50]
4
25
20
80
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in the iron oxide, Fe3O4 [pbm-51]
64.0
44.0
27.6
33.6
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of carbon in calcium carbonate, CaCO3 [pbm-52]
20
40
48
12
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of oxygen in calcium carbonate, CaCO3 [pbm-53]
48
16
60
56
If 54g of aluminium combines with oxygen to form 102g of aluminium oxide, work out the formula of aluminium oxide. (Relative atomic masses: Al = 27 and O = 16) [emp-1]
Al2O3
Al2O
AlO2
AlO3
In an experiment, 56g of iron combined with exactly 64g of
sulfur. Work out the formula of the iron sulfide formed. (Relative atomic masses: Fe = 56 and S = 32) [emp-2]
FeS
FeS2
Fe2S
FeS3
In an experiment, 21g of lithium combined with exactly 14g of nitrogen. Work out the formula of lithium nitride. (Relative atomic masses: Li = 7 and N = 14) [emp-3]
LiN2
Li2N
Li3N
LiN3
If 168g of iron combined with oxygen to form 232g of an iron oxide, work out the formula of the iron oxide. (Relative atomic masses: Fe = 56 and O = 16) [emp-4]
FeO
FeO2
Fe2O3
Fe3O4
If 28g of silicon combined with oxygen to form 60g of silicon oxide, work out the formula of silicon oxide. (Relative atomic masses: Si = 28 and O = 16) [emp-5]
SiO2
SiO
Si2O
SiO3
In an experiment, heating 128g of copper combined with exactly 32g of
sulfur. Work out the formula of the copper sulfide formed. (Relative atomic masses: Cu = 64 and S = 32) [emp-6]
CuS
Cu2S
CuS2
CuS4
In an experiment, excess chlorine was passed over 24g of heated magnesium metal until all the metal had reacted. If 95g of white magnesium chloride solid was formed, work out the formula of magnesium chloride. (Relative atomic masses: Mg = 24 and Cl = 35.5) [emp-7]
MgCl
Mg2Cl
MgCl2
MgCl3
In an experiment, excess chlorine was passed over 27g of heated aluminium metal until all the metal had reacted. If 133.5g of white
aluminium chloride was formed work out the formula of aluminium chloride. (Relative atomic masses: Al = 27 and Cl = 35.5) [emp-8]
Al3Cl
AlCl2
AlCl4
AlCl3
In an experiment, excess chlorine was passed over 28g of heated silicon until all of it had reacted. If 170g of liquid silicon chloride was formed work out the formula of silicon chloride. (Relative atomic masses: Si = 28 and Cl = 35.5) [emp-9]
SiCl4
SiCl2
Si2Cl
Si4Cl
In an experiment, excess chlorine was passed over 31g of hot phosphorus until all of it had reacted. If 208.5g of white phosphorus chloride was formed work out the formula of phosphorus chloride. (Relative atomic masses: P = 31 and Cl = 35.5) [emp-10]
PCl3
PCl5
PCl6
PCl7
If 8g of
sulfur combines with 12g of oxygen, what is the formula of the sulfur oxide formed? (Relative atomic masses: S = 32 and O = 16) [emp-11]
SO
SO2
SO3
SO4
If 16g of
sulfur combines with 103.5g of lead, what is the formula of the lead sulfide formed? (Relative atomic masses: S = 32 and Pb = 207) [emp-12]
Pb2S
PbS2
PbS6
PbS
If 40g of calcium combines with 160g of bromine, what is the formula of calcium bromide? (Relative atomic masses: Ca = 40 and Br = 80) [emp-13]
CaBr2
CaBr
CaBr3
Ca2Br
78g of potassium combines with 160g of bromine. What is the simplest formula of
potassium bromide? (Relative atomic masses: K = 39 and Br = 80) [emp-14]
KBr2
KBr
K2Br
KBr4
48g of magnesium combines with 320g of bromine, what is the formula of magnesium bromide? (Relative atomic masses: Mg = 24 and Br = 80) [emp-15]
MgBr
Mg2Br
MgBr2
MgBr3
160g of calcium combines with 64g of oxygen, what is the formula of calcium oxide? (Relative atomic masses: Ca = 40 and O = 16) [emp-16]
CaO2
Ca2O
Ca4O4
CaO
What is the formula of the phosphorus oxide formed when 62g of phosphorus combines with 80g of oxygen? (Relative atomic masses: P = 31 and O = 16) [emp-17]
P2O5
PO
P2O
PO5
72g of magnesium combines with 48g of oxygen, what is the formula of magnesium oxide? (Relative atomic masses: Mg = 24 and O = 16) [emp-18]
MgO2
MgO
Mg3O3
Mg2O
46g of sodium combined with 16g of oxygen. What is the formula of the sodium oxide formed? (Relative atomic masses: Na = 23 and O = 6) [emp-19]
NaO
NaO2
Na2O
Na2O2
78g of potassium combined with 32g of
sulfur. What is the formula of potassium sulfide formed? (Relative atomic masses: K = 39 and S = 32) [emp-20]
KS
KS2
K2S2
K2S
56g of iron combined with 240g of bromine. What is the formula of the iron bromide formed? (Relative atomic masses: Fe = 56 and Br = 80) [emp-21]
FeBr3
FeBr2
Fe3Br
FeBr
If 20.9g of bismuth combines with 24.0g of bromine, what is the formula of the bismuth bromide formed? (Relative atomic masses: Bi = 209 and Br = 80) [emp-22]
BiBr
BiBr3
Bi3Br
BiBr2
If 54g of aluminium combines with 96g of
sulfur, what is the formula of aluminium sulfide? (Relative atomic masses: = and = ) [emp-23]
AlS
AlS3
Al2S3
Al2S
When 117g of potassium combines with 31g of phosphorus, what is the formula of the potassium phosphide formed? (Relative atomic masses: K = 39 and P = 31) [emp-24]
KP
KP3
KP2
K3P
Given the equation: 2Mg(s) + O2(g) ==> 2MgO(s) and the atomic masses: Mg = 24, O = 16, how many g of magnesium is needed to make 10g of magnesium oxide? [rmc-1]
6.0
3.0
1.2
2.4
Given the equation: 2Mg(s) + O2(g) ==> 2MgO(s) and the atomic masses: Mg = 24, O = 16, how many tonne of magnesium oxide can be made from 3 tonne of magnesium? [rmc-2]
2.4
5.0
8.0
4.8
Given the equation: 2Mg(s) + O2(g) ==> 2MgO(s) and the atomic masses: Mg = 24, O = 16, what mass of oxygen in g, combines with 240g of magnesium? [rmc-3]
64
80
160
32
Iron
sulfide can be made by heating an iron and sulfur mixture. Fe(s) + S(s) ==> FeS(s) Given the atomic masses: Fe = 56, S = 32, how many g of iron
sulfide can be made from 14g of iron? [rmc-4]
44
28
16
22
Iron
sulfide can be made by heating an iron and sulfur mixture. Fe(s) + S(s) ==> FeS(s) Given the atomic masses: Fe = 56, S = 32, how many g of
sulfur reacts with 224g of iron? [rmc-5]
128
32
64
112
Iron
sulfide can be made by heating an iron and sulfur mixture. Fe(s) + S(s) ==> FeS(s) Given the atomic masses: Fe = 56, S = 32, how many g of iron is needed to make 440g of iron
sulfide? [rmc-6]
56
280
220
168
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ... Fe2O3(s) + 3CO(g) ==> 2Fe(l) + 3CO2(g) Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of iron can be made from 40 tonnes of haematite ore? [rmc-7]
56
14
28
7
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ... Fe2O3(s) + 3CO(g) ==> 2Fe(l) + 3CO2(g) Given the atomic masses: Fe = 56, O =16, C=12, how many tonne of haematite ore are needed to make 224 tonne of iron? [rmc-8]
160
480
640
320
The iron ore Haematite consists mainly of iron(III) oxide. In a blast furnace it is reduced to iron with carbon monoxide ... Fe2O3(s) + 3CO(g) ==> 2Fe(l) + 3CO2(g) Given the atomic masses: Fe = 56, O =16, C=12, how g of carbon monoxide are needed to reduce 32g of iron oxide to iron? [rmc-9]
16.8
33.6
8.4
28.0
The iron ore Haematite consists mainly of iron(III)
oxide. In a blast furnace it is reduced to iron with carbon monoxide ... Fe2O3(s) + 3CO(g) ==> 2Fe(l) + 3CO2(g) Given the atomic masses: Fe = 56, O =16, C=12, how many g of carbon dioxide are formed when 80 g of haematite is reduced to iron? [rmc-10]
44
66
33
40
Lime (calcium oxide) is made by heating limestone (calcium carbonate). CaCO3(s) ==> CaO(s) + CO2(g) Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of limestone is needed to make 112 tonne of lime? [rmc-11]
224
400
200
300
Lime (calcium oxide) is made by heating limestone (calcium carbonate). CaCO3(s) ==> CaO(s) + CO2(g) Given the atomic masses: Ca = 40, C = 12, O = 16, what mass in g of lime is made from 20g of limestone? [rmc-12]
8.8
5.6
4.4
11.2
Lime (calcium oxide) is made by heating limestone (calcium carbonate). CaCO3(s) ==> CaO(s) + CO2(g) Given the atomic masses: Ca = 40, C = 12, O = 16, how many tonne of carbon dioxide is formed by decomposing 400 tonne of calcium carbonate? [rmc-13]
176
44
88
132
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid. ZnCO3(s) + 2HCl(aq) ==> ZnCl2(aq) + H2O(l) + CO2(g) Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of zinc carbonate are needed to make 68g of zinc chloride?? [rmc-14]
125.0
62.5
68.0
136.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid. ZnCO3(s) + 2HCl(aq) ==> ZnCl2(aq) + H2O(l) + CO2(g) Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of HCl are needed to make 408g of zinc chloride? [rmc-15]
109.5
36.5
219.0
71.0
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid. ZnCO3(s) + 2HCl(aq) ==> ZnCl2(aq) + H2O(l) + CO2(g) Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, what mass of zinc chloride in g can be made from 25g of zinc carbonate? [rmc-16]
54.4
12.5
13.6
27.2
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid. ZnCO3(s) + 2HCl(aq) ==> ZnCl2(aq) + H2O(l) + CO2(g) Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of water are formed when 250g of zinc carbonate reacts? [rmc-17]
36
18
9
27
The salt zinc chloride can be made by dissolving zinc carbonate in dilute hydrochloric acid. ZnCO3(s) + 2HCl(aq) ==> ZnCl2(aq) + H2O(l) + CO2(g) Given the atomic masses: Zn = 65, C = 12, O =16, H = 1, Cl =35.5, how many g of carbon dioxide are formed when 3.65g of hydrochloric acid reacts? [rmc-18]
4.4
2.2
1.1
8.8
The salt sodium
sulfate, Na2SO4, can be made by neutralising sodium hydroxide with
sulfuric acid. 2NaOH(aq) + H2SO4(aq) ==> Na2SO4(aq) + 2H2O(l) Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium hydroxide is needed to make 213g of sodium
sulfate? [rmc-19]
40
80
120
160
The salt sodium
sulfate, Na2SO4, can be made by neutralising sodium hydroxide with
sulfuric acid. 2NaOH(aq) + H2SO4(aq) ==> Na2SO4(aq) + 2H2O(l) Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, what mass in g of
sulfuric acid is needed to make 7.1g of sodium sulfate? [rmc-20]
9.8
14.7
19.6
4.9
The salt sodium
sulfate, Na2SO4, can be made by neutralising sodium hydroxide with
sulfuric acid. 2NaOH(aq) + H2SO4(aq) ==> Na2SO4(aq) + 2H2O(l) Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of sodium
sulfate is formed when 8g of sodium hydroxide reacts? [rmc-21]
14.2
28.4
7.1
21.3
The salt sodium
sulfate, Na2SO4, can be made by neutralising sodium hydroxide with
sulfuric acid. 2NaOH(aq) + H2SO4(aq) ==> Na2SO4(aq) + 2H2O(l) Given the atomic masses: Na = 23, O = 16, H = 1, S = 32, how many g of water are formed when 46g of
sulfuric acid reacts? [rmc-22]
9
18
36
23
Copper(I)
sulfide ore can be converted to copper by roasting in air: Cu2S(s) + O2(g) ==> 2Cu(s) + SO2(g) How many g of copper can be made from 320g of the copper ore? (Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-23]
128
64
256
192
Copper(I)
sulfide ore can be converted to copper by roasting in air: Cu2S(s) + O2(g) ==> 2Cu(s) + SO2(g) How many tonnes of oxygen are needed to convert 40 tonnes of ore to copper? (Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-24]
16
32
12
8
Copper(I)
sulfide ore can be converted to copper by roasting in air: Cu2S(s) + O2(g) ==> 2Cu(s) + SO2(g) How many tonnes of
sulfur dioxide are produced for every 1280 tonnes of ore processed? (Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-25]
512
128
256
64
Copper(I)
sulfide ore can be converted to copper by roasting in air: Cu2S(s) + O2(g) ==> 2Cu(s) + SO2(g) How many tonnes of ore are needed to make 25.6 tonnes of copper? (Relative atomic masses: Cu = 64, S = 32, O = 16) [rmc-26]
64
32
48
56
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is: 2Al(s) + 6HCl(g) ==> 2AlCl3(s) + 3H2(g) How many kg of aluminium chloride can be made from 27 kg of aluminium? (Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-27]
267.0
400.5
133.5
66.75
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the hydrogen chloride reaction is: 2Al(s) + 6HCl(g) ==> 2AlCl3(s) + 3H2(g) How many tonnes of hydrogen would be produced by reacting 108 tonnes of aluminium? (Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1.0) [rmc-28]
2
3
6
12
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is: 2Al(s) + 3Cl2(g) ==> 2AlCl3(s) How much aluminium is needed to make 89 g of aluminium chloride? (Relative atomic masses: Al = 27.0, Cl = 35.5, H =1) [rmc-29]
18
27
54
9
Aluminium chloride can be prepared by passing dry chlorine or hydrogen chloride gas over heated aluminium metal. The equation for the chlorine reaction is: 2Al(s) + 3Cl2(g) ==> 2AlCl3(s) How many tonne of chlorine is needed to make 1068 tonne of aluminium chloride? (Relative atomic masses: Al = 27.0, Cl = 35.5, H = 1) [rmc-30]
71
852
426
213
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal: lead(II) oxide + carbon ==> lead + carbon dioxide 2PbO(s) + C(s) ==> 2Pb(l) + CO2(g) How many tonne of lead can be made from 223 tonne of ore? (Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-31]
414.0
103.5
207.0
310.5
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal: lead(II) oxide + carbon ==> lead + carbon dioxide 2PbO(s) + C(s) ==> 2Pb(l) + CO2(g) How many tonne of ore is needed to make 828 tonne of lead? (Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-32]
223
446
1784
892
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal: lead(II) oxide + carbon ==> lead + carbon dioxide 2PbO(s) + C(s) ==> 2Pb(l) + CO2(g) How many kg of carbon is needed to make 828 kg of lead? (Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-33]
24
12
6
48
Yellow lead(II) oxide ore can be reduced by heating with charcoal (carbon) in a furnace to give silvery liquid lead metal: lead(II) oxide + carbon ==> lead + carbon dioxide 2PbO(s) + C(s) ==> 2Pb(l) + CO2(g) How many g of carbon dioxide are formed when 207 g of lead are produced? (Relative atomic masses: Pb = 207, O = 16, C = 12) [rmc-34]
44
22
11
33
Chlorine consists of 75% chlorine-35 and 25% chlorine-37. Calculate the Ar of chlorine to 3sf/1dp. [ram-1]
35.5
35.0
36.0
35.6
Bromine consists of the isotopes: 50.5% Br-79 and 49.5% Br-81. Calculate the relative atomic mass, Ar, of bromine to 3sf/1dp. [ram-2]
80.1
80.0
79.9
79.8
Lithium consists of 7.4% lithium-6 and 92.6% lithium-7. Calculate the relative atomic mass, Ar, of lithium to 2sf/1dp. [ram-3]
6.5
6.7
6.9
6.6
Boron is 19.7% B-10 and 80.3% B-11. Calculate the relative atomic mass, Ar, of boron to 3sf/1dp. [ram-4]
10.5
10.9
10.3
10.8
Antimony (Sb) is 57.2% Sb-121 and 42.8% Sb-123. Calculate the Ar of Sb to 4sf/1dp. [ram-5]
121.9
122.0
122.1
121.2
Chromium has four stable isotopes. 4.31% Cr-50, 83.76% Cr-52, 9.55% Cr-53 and 2.38% Cr-54. Calculate the relative atomic mass, Ar, of chromium to 3sf/1dp. [ram-6]
52.3
52.1
52.2
52.5
Copper consists of 69.1% Cu-63 and 30.9% Cu-65. Calculate the relative atomic mass, Ar, of copper to 3sf/1dp. [ram-7]
64.0
63.3
63.6
64.5
Europium consists of 47.8% Eu-151 and 52.2% Eu-153. Calculate Ar(Eu) to 4sf/1dp. [ram-8]
151.9
152.2
151.5
152.0
Gallium is made up of 60.2% gallium-69 and 39.8% of gallium-71. Calculate the Ar of gallium to 3sf/1dp. [ram-9]
69.8
70.0
69.9
69.5
Iron has four stable isotopes. 5.8% Fe-54, 91.7% Fe-56, 2.2% Fe-57 and 0.3% Fe-58. Calculate the Ar of iron to 3sf/1dp. [ram-10]
56.2
55.9
56.3
56.1
Magnesium consists of 78.6% 24Mg, 10.1% 25Mg and 11.3% of 26Mg. Calculate the relative atomic mass, Ar, of magnesium to 3sf/1dp. [ram-11]
25.0
24.7
24.3
24.1
Neon consists of 90.9% 20Ne, 0.3% 21Ne and 8.8% 22Ne. Calculate the relative atomic mass, Ar, of neon to 3sf/1dp. [ram-12]
20.5
20.1
20.3
20.2
Rhenium (Re) consists of 37.1% 185Re and 62.9% 187Re. Calculate the relative atomic mass, Ar, of rhenium to 4sf/1dp. [ram-13]
186.3
186.0
185.6
185.5
Rubidium consists of the stable isotopes: 85Rb (72.2%) and 87Rb (27.8%). Calculate Ar(Rb) to 3sf/1dp. [ram-14]
86.0
85.6
85.9
85.5
Thallium consists of 29.5% thallium-203 and 70.5% thallium-205. Calculate the relative atomic mass, Ar, of to 4sf/1dp. [ram-15]
204.0
204.2
204.4
204.1
How many moles of iron are there in 2.8g? (atomic mass Fe = 56) [mam-1]
0.05
156.8
20.0
2.0
How many moles of
sulfur are there in 64g? (atomic mass S = 32) [mam-2]
2048
2.0
0.5
0.05
How many moles of sodium are there in 115g? (atomic mass Na = 23) [mam-3]
2645
0.2
5
4
How many moles of carbon are there in 3g? (atomic mass C = 12 ) [mam-4]
36
4
0.5
0.25
How many moles of zinc are there in 1.625g? (atomic mass Zn = 65) [mam-5]
0.025
105.6
40.0
100.0
How many moles of iodine are there in 12.7g of I2? (atomic mass I = 127) [mam-6]
10.0
0.05
0.10
5.0
How many moles of chlorine are there in 213g of Cl2? (atomic mass Cl = 35.5) [mam-7]
0.17
0.33
3.0
6.0
How many moles of bromine are there in 6.4g of Br2? (atomic mass Br = 80) [mam-8]
512
1024
0.08
0.04
How many moles of phosphorus are there in 24.8g of P4? (atomic mass P = 31) [mam-9]
0.2
0.8
7688
1922
How many moles of oxygen are there in 128g of O2? (atomic mass O = 16) [mam-10]
8
4
2048
1032
How many moles of water are there in 4.5g of H2O? (atomic masses: H = 1, O = 16) [mam-11]
81
0.26
0.25
72
How many moles of methane are there in 112g of CH4? (atomic masses: C = 12, H = 1) [mam-12]
8.6
1792
0.14
7.0
How many moles of sodium
sulfate are there in 7.1g of Na2SO4? (atomic masses: Na = 23, S = 32, O = 16) [mam-13]
0.05
10082
20
5
How many moles of
sulfuric acid are there in 2.45g of H2SO4? (atomic masses: H = 1, S = 32, O = 16) [mam-14]
240.1
0.025
40.0
3.0
How many moles of calcium hydroxide are there in 25.9g of Ca(OH)2? (atomic masses: Ca = 40, O = 16, H = 1) [mam-15]
2.86
1916
0.35
45.0
How many g are there in 1.5 moles of aluminium? (atomic mass Al = 27) [mam-16]
0.056
18.0
9.0
40.5
How many g are there in 0.02 moles of uranium? (atomic mass U = 238) [mam-17]
4.76
11900
0.00008
2.58
How many g are there in 0.65 moles of magnesium? (atomic mass Mg = 24) [mam-18]
0.027
15.6
36.9
7.8
How many g are there in 0.23 moles of silicon? (atomic mass Si = 28) [mam-19]
0.0082
121.7
6.44
0.82
How many g are there in 7.3 moles of boron? (atomic mass B = 10.8) [mam-20]
0.68
1.48
70.0
78.84
How many g are there in 0.05 moles of nitrogen, N 2? (atomic mass N = 14) [mam-21]
1.4
2.4
0.0035
280
How many g are there in 0.75 moles of ozone, O3? (atomic mass O = 16) [mam-22]
0.047
36.0
12.0
0.016
How many g are there in 2.5 moles of oxygen, O2? (atomic mass O = 16) [mam-23]
4.0
6.4
80.0
40.0
How many g are there in 0.16 moles of chlorine, Cl2? (atomic mass Cl = 35.5) [mam-24]
5.68
221.8
443.8
11.36
How many g are there in 1.65 moles of iodine, I2? (atomic mass I = 127) [mam-25]
419.1
77.0
154.0
209.6
How many g are there in 3.6 moles of sodium hydroxide, NaOH? (atomic masses: Na = 23, O = 16, H = 1) [mam-26]
0.09
144
11.1
7.2
How many g are there in 1.5 moles of nitric acid, HNO3? (atomic masses: H = 1, N = 14, O = 16) [mam-27]
42.0
0.024
94.5
46.5
How many g are there in 0.15 moles of ammonium
sulfate, (NH4)2SO4? (atomic masses: N = 14, H = 1, S = 32, O = 16) [mam-28]
0.0011
880.0
17.1
19.8
How many g are there in 0.8 moles of aluminium hydroxide, Al(OH)3? (atomic masses: Al = 27, O = 16, H = 1) [mam-29]
62.4
97.5
0.01
10.0
How many g are there in 0.005 moles of sodium thiosulfate, Na2S2O3? (atomic masses: Na = 23, S = 32, O =16) [mam-30]
0.71
0.79
0.63
0.55
It was found that 0.2 moles of atoms of an element had a mass of 3.2g. What is the relative atomic mass of the element? [mam-31]
6.4
8.0
16.0
15.0
It was found that 0.005 moles of atoms of an element had a mass of 0.295g. What is the relative atomic mass of the element? [mam-32]
15
60
16
59
It was found that 0.15 moles of atoms of an element had a mass of 10.95g. What is the relative atomic mass of the element? [mam-33]
73
164
82
146
It was found that 0.4 moles of atoms of an element had a mass of 56.2g. What is the relative atomic mass of the element? [mam-34]
22.5
140.5
224.0
25.0
It was found that 0.015 moles of atoms of an element had a mass of 2.88g. What is the relative atomic mass of the element? [mam-35]
432
450
192
200
It was found that 0.25 moles of atoms of an element had a mass of 40.65g. What is the relative atomic mass of the element? [mam-36]
10.2
102.0
16.0
162.6
It was found that 0.002 moles of a compound had a mass of 0.24g. What is the relative formula mass of the compound? [mam-37]
120
12
48
480
It was found that 0.005 moles of a compound had a mass of 0.2025g. What is the relative formula mass of the compound? [mam-38]
101.3
40.5
24.7
247
It was found that 0.25 moles of a compound had a mass of 14.05g. What is the relative formula mass of the compound? [mam-39]
177.8
35.1
56.2
28.1
It was found that 0.025 moles of a compound had a mass of 0.70g. What is the relative formula mass of the compound? [mam-40]
175
280
140
28
0.55g of boron combined with 1.2g of oxygen. Deduce the empirical formula of boron oxide. (relative atomic masses, Ar: B = 11, O = 16) [efm-1]
B2O3
BO
B2O
BO2
1.35g of aluminium was burned in excess fluorine to form 4.2g of aluminium fluoride. Deduce the empirical formula of aluminium fluoride. (relative atomic masses, Ar: Al = 27, F = 19) [efm-2]
AlF
AlF3
Al3F
AlF2
3.4g of an unusual carbon oxide contained 1.8g of carbon. Deduce the empirical formula of the carbon oxide. (relative atomic masses, Ar: C=12, O=16) [efm-3]
CO
CO2
C3O2
C2O3
In an experiment 3.175g of copper combined with 0.400g of oxygen. What is the empirical formula of the copper oxide? (relative atomic masses, Ar: Cu = 63.5, O = 16) [efm-4]
CuO
CuO2
Cu2O2
Cu2O
8.875g of chlorine combined with 14.25g of fluorine. What is the formula of the chlorine fluoride? (relative atomic masses, Ar: Cl = 35.5, F = 19) [efm-5]
ClF3
Cl3F
ClF
ClF2
A gas formed by the combination of hydrogen and
sulfur consisted of 5.88% hydrogen and 94.12% sulfur. What is its empirical formula? (relative atomic masses, Ar: H = 1, S = 32) [efm-6]
HS
H2S
HS2
H2S2
5.08g of iodine combined with 1.6g of oxygen. What is the formula of the iodine oxide? (relative atomic masses, Ar: I = 127, O = 16) [efm-7]
IO5
I2O
I2O5
I2O3
2.8g of lithium was heated in a stream of air forming 6.0g of lithium oxide. What is its formula? (relative atomic masses, Ar: Li = 7, O =16) [efm-8]
LiO
LiO2
LiO3
Li2O
A iron-copper
sulfide ore consisted of 30.5% iron, 34.6% copper, and 34.9% sulfur. What is the empirical formula of the ore? (relative atomic masses, Ar: Fe = 56, Cu = 63.5, S = 32) [efm-9]
FeCuS2
FeCuS
FeCu2S
Fe2CuS2
0.48g of magnesium combined with 3.20g of bromine. What is the formula of magnesium bromide? (relative atomic masses, Ar: Mg = 24, Br = 80) [efm-10]
Mg2Br
MgBr2
MgBr
MgBr3
0.7g of nitrogen combined with 5.325g of chlorine. Deduce the formula of nitrogen chloride. (relative atomic masses, Ar: N = 14, Cl = 35.5) [efm-11]
NCl
NCl2
NCl3
N3Cl
Fluorine oxide consists of 70.4% fluorine and 29.6% oxygen by mass. Deduce the formula of fluorine oxide. (relative atomic masses, Ar: F = 19, O = 16) [efm-12]
FO
FO2
FO3
F2O
47.6g of uranium combined with 22.8g of fluorine. What is the empirical formula of this uranium fluoride? (relative atomic masses, Ar: U = 238, F = 19) [efm-13]
UF6
UF3
UF2
UF4
10.35g of lead was heated in excess oxygen. If 11.95g of a lead oxide was formed, deduce its empirical formula. (relative atomic masses, Ar: Pb = 207, O = 16) [efm-14]
PbO
PbO2
Pb2O
PbO3
10.8g of aluminium combined with 19.2g of
sulfur. What is the empirical formula of aluminium sulfide? (relative atomic masses, Ar: Al = 27, S = 32) [efm-15]
Al3S2
AlS3
Al2S3
AlS2
A hydrocarbon of molecular mass 30 consisted of 80% carbon and 20% hydrogen by mass. Deduce the molecular formula of the hydrocarbon. (relative atomic masses, Ar: C = 12, H = 1) [efm-16]
CH3
C2H3
CH18
C2H6
6g of carbon combines with 71g of chlorine. What is the formula of the carbon chloride? (relative atomic masses, Ar: C = 12, Cl = 35.5) [efm-17]
CCl4
C4Cl
CCl2
C2Cl
An organic compound consisted of 52.18% carbon, 13.04% hydrogen and 34.78% oxygen by mass. Deduce its empirical formula. (relative atomic masses, Ar: C = 12, H = 1, O = 16) [efm-18]
CH6O
C2H6O
C2H6O2
CH3O
A chlorinated
hydrocarbon molecule consisted of 37.21% carbon, 7.75% hydrogen and 55.04% chlorine by mass. Deduce its empirical formula. (relative atomic masses, Ar: C = 12, H = 1, Cl = 35.5) [efm-19]
C2H6Cl
CH3Cl
C2H5Cl
C2H4Cl2
A calcium mineral consisted of 29.4% calcium, 23.5%
sulfur and 47.1% oxygen by mass. Calculate the empirical formula of the mineral. (relative atomic masses, Ar: Ca = 40, S = 32, O = 16) [efm-20]
CaSO2
CaSO3
Ca2SO4
CaSO4
A salt consisted of 27.06% sodium, 16.47% nitrogen and 56.47% oxygen by mass. Deduce the formula of the salt. (relative atomic masses, Ar: Na = 23, N = 14, O = 16) [efm-21]
NaNO3
NaNO2
Na2NO3
NaNO
A brominated hydrocarbon consisted of 12.77% carbon, 2.13% hydrogen and 85.10% bromine by mass. If its molecular mass is 188, deduce the molecular formula of the molecule. (relative atomic masses, Ar: C = 12, H = 1, Br =80) [efm-22]
CH2Br
C2H4Br2
CH16Br2
C2H4Br2
It was found that 24g of carbon was combined with 5g of hydrogen in a hydrocarbon. If its molecular mass was 58, what is its molecular formula? (relative atomic masses, Ar: C = 12, H = 1) [efm-23]
C2H5
C3H8
C4H10
C3H22
A hydrocarbon consisted of 92.3% carbon and 7.7% hydrogen. If its molecular mass is 78, work out its molecular formula. (relative atomic masses, Ar: C = 12, H = 1) [efm-24]
C5H18
CH
CH6
C6H6
A carbohydrate on analysis consisted of 40.00% carbon, 6.67% hydrogen and 53.33% oxygen. If its molecular mass is 180, deduce the molecular formula of the carbohydrate. (relative atomic masses, Ar: C = 12, H = 1, O = 16) [efm-25]
C6H12O6
CH2O
C5H8O7
C3H6O3
7.75g of an alcohol consisted of 3.00g carbon, 0.75g hydrogen and 4.00g oxygen. If its molecular mass is 62, work out the molecular formula. (relative atomic masses, Ar: C = 12, H = 1, O = 16) [efm-26]
C3H10O
C2H6O2
CH3O
C2H6O
An alcohol consisted of 39.13% carbon, 8.70% hydrogen and 52.17% oxygen. If its molecular mass is 92, deduce its molecular formula. (relative atomic masses, Ar: C = 12, H = 1, O = 16) [efm-27]
CH2O
C3H6O3
C3H8O3
C2H4O4
In an experiment 6g of carbon combined with 19g of fluorine. Calculate the molecular formula of the compound formed if the molecular mass of it is 100. (relative atomic masses, Ar: C = 12, F = 19) [efm-28]
CF2
C4F2
CF4
C2F4
A compound of hydrogen and oxygen was made up of 0.5g hydrogen and 8g of oxygen. What is its empirical formula? (relative atomic masses, Ar: H = 1, O = 16) [efm-29]
HO
H2O2
H2O
HO2
A lithium compound consisted of 7g of lithium combined with 16g of
sulfur and 32g of oxygen. What is the empirical formula of the compound? (relative atomic masses, Ar: Li = 7, S = 32, O = 16) [efm-30]
LiSO2
Li2SO4
LiSO4
Li2SO3
58g of a sodium phosphate salt consisted of 34.5g of sodium, 15.5g of phosphorus and 32.0g of oxygen. What is the simplest formula of the compound? (relative atomic masses, Ar: Na = 23, P = 31, O = 16) [efm-31]
Na4PO3
Na2PO4
Na3PO4
Na2PO3
A sodium compound consisted of 46g of sodium combined with 254g of iodine and 128g of oxygen. What is the compounds empirical formula? (relative atomic masses, Ar: Na = 23, I = 127, O = 16) [efm-32]
NaIO3
NaIO2
Na2IO4
NaIO4
16g of copper, after heating in oxygen, formed 20g of a copper oxide. What is the formula of the oxide? (relative atomic masses, Ar: Cu = 64, O = 16) [efm-33]
CuO
CuO2
Cu2O
CuO3
An oxide of carbon consisted of 3g of carbon combined with 4g of oxygen. What is the formula of the oxide? (relative atomic masses, Ar: C = 12, O = 16) [efm-34]
CO2
CO
C2O4
C2O
1.95g of potassium combined with 4.00g of bromine. What is the empirical formula of the compound? (relative atomic masses, Ar: K = 39, Br = 80) [efm-35]
K2Br
KBr2
KBr
KBr3
5g of calcium on heating in oxygen formed 7g of calcium oxide. What is the simplest formula of calcium oxide? (relative atomic masses, Ar: Ca = 40, O = 16) [efm-36]
CaO2
Ca2O
CaO3
CaO
13g of zinc combined with 6.4g of
sulfur. What is the empirical formula of zinc sulfide? (relative atomic masses, Ar: Zn = 65, S = 32) [efm-37]
ZnS
ZnS2
Zn2S
ZnS3
An oxide of copper contained 80% copper and 20% oxygen by mass. What is the formula of the copper oxide? (relative atomic masses, Ar: Cu = 64, O = 16) [efm-38]
Cu2O
CuO
CuO2
CuO3
If magnesium oxide consists of 60% magnesium and 40% oxygen, what is its simplest formula? (relative atomic masses, Ar: Mg = 24, O = 16) [efm-39]
Mg2O
MgO2
MgO
MgO3
2.3g of sodium combined with 1.6g of
sulfur. What is the formula of sodium sulfide? (relative atomic masses, Ar: Na = 23, S = 32) [efm-40]
NaS
NaS2
NaS3
Na2S
In an experiment 1.28g of copper combined with 0.16g of oxygen. What is the formula of the copper oxide? (relative atomic masses, Ar: Cu = 64, O = 16) [efm-41]
Cu2O
CuO
CuO2
CuO3
13.8g of sodium combined with 6.2g of phosphorus. What is the formula of sodium phosphide? (relative atomic masses, Ar: Na = 23, P = 31) [efm-42]
NaP
Na3P
NaP2
Na2P
10g of calcium combined with 40g of bromine. What is the formula of calcium bromide? (relative atomic masses, Ar: Ca = 40, Br = 80) [efm-43]
CaBr
Ca2Br
CaBr2
CaBr3
22g of boron combined with 114g of fluorine. What is the empirical formula of boron fluoride? (relative atomic masses, Ar: B = 11, F = 19) [efm-44]
BF
BF2
B3F
BF3
1.2g of titanium, after heating in oxygen, formed 2.0g of a titanium oxide. What is the empirical formula for the titanium oxide? (relative atomic masses, Ar: Ti = 48, O = 16) [efm-45]
TiO2
TiO
Ti2O
TiO3
0.800g of magnesium reacted with 8.47g of iodine. Calculate the empirical formula for magnesium iodide. (relative atomic masses, Ar: Mg = 24, I = 127) [efm-46]
MgI
MgI2
Mg2I
MgI3
Given the equation: 2Na(s) + 2H2O(l) ==> 2NaOH(aq) + H2(g) Calculate the volume of hydrogen formed in dm3 when 2.3g of sodium reacts with water. (Ar's Na=23, H=1, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-1]
1.2
2.4
4.8
0.6
Given the equation: 2Na(s) + 2H2O(l) ==> 2NaOH(aq) + H2(g) Calculate the volume of hydrogen formed in dm3 when 9.2g of sodium reacts with water. (Ar's Na=23, H=1, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-2]
2.4
4.8
9.6
1.2
Given the equation: 2Na(s) + 2H2O(l) ==> 2NaOH(aq) + H2(g) What mass of sodium in g will form 600 cm3 of hydrogen gas? (Ar's Na=23, H=1, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-3]
2.30
2.40
1.15
4.60
Given the equation: 2Na(s) + 2H2O(l) ==> 2NaOH(aq) + H2(g) What mass of sodium in g will form 18 dm3 of hydrogen gas? (Ar's Na=23, H=1, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-4]
23.0
46.0
16.5
34.5
Given the equation for the thermal decomposition of calcium carbonate (limestone): CaCO3(s) ==> CaO(s) + CO2(g) What volume of carbon dioxide in dm3 is formed when 10g of limestone is heated strongly? (Ar's Ca=40, C=12, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-5]
2.4
4.8
1.2
4.4
Given the equation for the thermal decomposition of calcium carbonate (limestone) ... CaCO3(s) ==> CaO(s) + CO2(g) What volume of carbon dioxide in dm3 is formed when 200g of limestone is heated strongly? (Ar's Ca=40, C=12, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-6]
24
48
12
96
Given the equation for the thermal decomposition of calcium carbonate (limestone) ... CaCO3(s) ==> CaO(s) + CO2(g) What mass of limestone in g, on strong heating, will form 6 dm3 carbon dioxide? (Ar's Ca=40, C=12, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-7]
50
56
25
12
Given the equation for the thermal decomposition of calcium carbonate (limestone) ... CaCO3(s) ==> CaO(s) + CO2(g) What mass of limestone in g, on strong heating, will form 120 cm3 carbon dioxide? (Ar's Ca=40, C=12, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-8]
0.3
1.0
2.0
0.5
5 g of a gas had a volume of 60 dm3. What is its molecular mass? (1 mol gas = 24 dm3 at room temp./press.) [mvg-9]
2
6
4
12
What is the volume in dm3 of 8 g of a gas of molecular mass 16? (1 mol gas = 24 dm3 at room temp./press.) [mvg-10]
6
12
0.5
2
What mass of gas, of molecular mass 36.5, is present in 4.8 dm3 of the gas? (1 mol gas = 24 dm3 at room temp./press.) [mvg-11]
14.6
3.65
7.30
0.76
0.145 g of a gas had a volume of 60 cm3. What is its molecular mass? (1 mol gas = 24 dm3 at room temp./press.) [mvg-12]
29
30
116
58
What is the volume in dm3 of 0.85 g of a gas of molecular mass 17? (1 mol gas = 24 dm3 at room temp./press.) [mvg-13]
1.2
0.6
2.4
3.4
What mass of gas, of molecular mass 71, is present in 1.2 dm3 of the gas? (1 mol gas = 24 dm3 at room temp./press.) [mvg-14]
14.2
3.55
7.10
8.52
2.55g of a gas had a volume of 0.6 dm3. What is its molecular mass? (1 mol gas = 24 dm3 at room temp./press.) [mvg-15]
17
51
102
34
What is the volume in dm3 of 1 g of a gas of molecular mass 96? (1 mol gas = 24 dm3 at room temp./press.) [mvg-16]
4.00
0.50
1.92
0.25
What mass of gas, of molecular mass 44, is present in 0.15 dm3 of the gas? (1 mol gas = 24 dm3 at room temp./press.) [mvg-17]
0.275
6.600
3.600
0.003
What is the volume in dm3 of 0.8 g of a gas of molecular mass 32? (1 mol gas = 24 dm3 at room temp./press.) [mvg-18]
0.025
0.6
19.2
1.33
Given the equation for magnesium dissolving in hydrochloric acid: Mg(s) + 2HCl(aq) ==> MgCl2(aq) + H2(g) What mass of magnesium in g, will form 1.2 dm3 of hydrogen gas? (Ar's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-19]
28.8
0.6
1.2
2.4
Given the equation for magnesium dissolving in hydrochloric acid: Mg(s) + 2HCl(aq) ==> MgCl2(aq) + H2(g) What mass of magnesium in g, will form 36 dm3 of hydrogen gas? (Ar's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-20]
24
12
72
36
Given the equation for magnesium dissolving in hydrochloric acid: Mg(s) + 2HCl(aq) ==> MgCl2(aq) + H2(g) What volume of hydrogen gas, in dm3, is formed when 4g of magnesium dissolves in the acid? (Ar's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-21]
4
2
6
3
Given the equation for magnesium dissolving in hydrochloric acid: Mg(s) + 2HCl(aq) ==> MgCl2(aq) + H2(g) What volume of hydrogen gas, in dm3, is formed when 72g of magnesium dissolves in the acid? (Ar's Mg=24, H=1, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-22]
36
72
48
24
Given the equation for aluminium dissolving in dilute
sulfuric acid: 2Al(s) + 3H2SO4(aq) ==> Al2(SO4)3(aq) + 3H2(g) What mass of aluminium (g) dissolves when 7.2 dm3 of hydrogen is formed? (Ar's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-23]
2.7
0.3
5.4
16.2
Given the equation for aluminium dissolving in dilute
sulfuric acid: 2Al(s) + 3H2SO4(aq) ==> Al2(SO4)3(aq) + 3H2(g) What mass of aluminium in g, dissolves when 48 dm3 of hydrogen is formed? (Ar's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-24]
18
6
18
36
Given the equation for aluminium dissolving in dilute
sulfuric acid: 2Al(s) + 3H2SO4(aq) ==> Al2(SO4)3(aq) + 3H2(g) What volume of hydrogen, in dm3, is formed, when 54g of aluminium dissolves? (Ar's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-25]
72
24
48
36
Given the equation for aluminium dissolving in dilute
sulfuric acid: 2Al(s) + 3H2SO4(aq) ==> Al2(SO4)3(aq) + 3H2(g) What volume of hydrogen, in dm3, when 27g of aluminium dissolves? (Ar's: Al=27, H=1, S=32, O=16, 1 mol gas = 24 dm3 at room temp./press.) [mvg-26]
12
36
18
24
Given the equation for calcium carbonate dissolving in hydrochloric acid: CaCO3(s) + 2HCl(aq) ==> CaCl2(aq) H2O(l) + CO2(g) Calculate the volume of carbon dioxide, in dm3, when 5 g of calcium carbonate dissolves in the acid. (Ar's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-27]
2.4
0.6
1.2
1.8
Given the equation for calcium carbonate dissolving in hydrochloric acid: CaCO3(s) + 2HCl(aq) ==> CaCl2(aq) H2O(l) + CO2(g) Calculate the volume of carbon dioxide, in dm3, when 400 g of calcium carbonate dissolves in the acid. (Ar's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-28]
48
6
24
96
Given the equation for calcium carbonate dissolving in hydrochloric acid: CaCO3(s) + 2HCl(aq) ==> CaCl2(aq) H2O(l) + CO2(g) Calculate the mass of calcium carbonate (in g) that dissolves when 6 dm3 of carbon dioxide is formed. (Ar's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-29]
25.0
12.5
6.0
100.0
Given the equation for calcium carbonate dissolving in hydrochloric acid: CaCO3(s) + 2HCl(aq) ==> CaCl2(aq) H2O(l) + CO2(g) Calculate the mass of calcium carbonate (in g) that dissolves when 36 dm3 of carbon dioxide is formed. (Ar's: Ca=40, C=12, O=16, Cl=35.5, 1 mol gas = 24 dm3 at room temp./press.) [mvg-30]
66
150
100
44
Given the reaction between hydrogen and chlorine to form hydrogen chloride: H2(g) + Cl2(g) ==> 2HCl(g) What volume of hydrogen in cm3 is needed to make 100cm3 of hydrogen chloride? [rgv-1]
50
100
200
150
Given the reaction between hydrogen and chlorine to form hydrogen chloride: H2(g) + Cl2(g) ==> 2HCl(g) What volume of chlorine in dm3 is needed to make 40dm3 of hydrogen chloride? [rgv-2]
40
20
10
30
Given the reaction between hydrogen and chlorine to form hydrogen chloride: H2(g) + Cl2(g) ==> 2HCl(g) What volume of hydrogen chloride in dm3 is made by reacting 20dm3 of hydrogen? [rgv-3]
20
30
40
10
Given the reaction between hydrogen and chlorine to form hydrogen chloride: H2(g) + Cl2(g) ==> 2HCl(g) What volume of hydrogen chloride in cm3 is made by reacting 300cm3 of chlorine? [rgv-4]
300
450
150
600
Given the reaction between nitrogen and hydrogen to form ammonia: N2(g) + 3H2(g) ==> 2NH3(g) What volume of ammonia in cm3 is formed if 180cm3 of hydrogen reacts? [rgv-5]
120
180
90
60
Given the reaction between nitrogen and hydrogen to form ammonia: N2(g) + 3H2(g) ==> 2NH3(g) What volume of ammonia in dm3 is formed if 40dm3 of nitrogen reacts? [rgv-6]
120
80
40
160
Given the reaction between nitrogen and hydrogen to form ammonia: N2(g) + 3H2(g) ==> 2NH3(g) What volume of hydrogen in dm3 is needed to make 60dm3 of ammonia? [rgv-7]
45
60
90
30
Given the reaction between nitrogen and hydrogen to form ammonia: N2(g) + 3H2(g) ==> 2NH3(g) What volume of nitrogen in cm3 is needed to make 640cm3 of ammonia? [rgv-8]
640
960
160
320
The combustion of methane is given by the equation: CH4(g) + 2O2(g) ==> CO2(g) + 2H2O(l) What volume of oxygen in cm3 is needed to burn 200cm3 of methane? [rgv-9]
400
200
300
800
The combustion of methane is given by the equation: CH4(g) + 2O2(g) ==> CO2(g) + 2H2O(l) What volume of carbon dioxide in cm3 is formed on burning 10cm3 of methane? [rgv-10]
20
10
40
30
The combustion of methane is given by the equation: CH4(g) + 2O2(g) ==> CO2(g) + 2H2O(g) What is the total volume of gases produced in cm3 when 30cm3 of methane burns? [rgv-11]
30
60
90
120
The combustion of propane is given by the equation: C3H8(g) + 5O2(g) ==> 3CO2(g) + 4H2O(l) What volume of oxygen in cm3 is needed to burn 20cm3 of propane? [rgv-12]
50
70
200
100
The combustion of propane is given by the equation: C3H8(g) + 5O2(g) ==> 3CO2(g) + 4H2O(l) What volume of propane in cm3 can be completely burned by 200cm3 of oxygen? [rgv-13]
40
50
80
20
The combustion of propane is given by the equation: C3H8(g) + 5O2(g) ==> 3CO2(g) + 4H2O(l) What volume of carbon dioxide in dm3 is formed by burning 30dm3 of propane? [rgv-14]
60
90
150
50
The combustion of propane is given by the equation: C3H8(g) + 5O2(g) ==> 3CO2(g) + 4H2O(g) What total volume of gases in cm3 is formed by burning 40cm3 of propane? [rgv-15]
120
160
280
200
The combustion of propane is given by the equation: C3H8(g) + 5O2(g) ==> 3CO2(g) + 4H2O(g) What volume of steam in cm3 is formed by burning 20cm3 of propane? [rgv-16]
100
160
40
80
The combustion of ethane is given by the equation: 2C2H6(g) + 7O2(g) ==> 4CO2(g) + 6H2O(l) What volume of carbon dioxide in cm3 is formed by burning 20cm3 of ethane? [rgv-17]
40
20
80
70
The combustion of ethane is given by the equation: 2C2H6(g) + 7O2(g) ==> 4CO2(g) + 6H2O(l) What volume of oxygen in cm3 is needed to completely burn 60cm3 of ethane? [rgv-18]
420
210
105
120
The combustion of ethane is given by the equation: 2C2H6(g) + 7O2(g) ==> 4CO2(g) + 6H2O(g) What volume of steam in dm3 is formed when 40dm3 of ethane burns? [rgv-19]
240
60
120
80
The combustion of ethane is given by the equation: 2C2H6(g) + 7O2(g) ==> 4CO2(g) + 6H2O(g) What total volume of gases in dm3 are formed when 15dm3 of ethane burns? [rgv-20]
150
30
45
75
The combustion of ethane is given by the equation: 2C2H6(g) + 7O2(g) ==> 4CO2(g) + 6H2O(g) What volume of ethane in cm3 can be burned completely using 175cm3 of oxygen? [rgv-21]
50
100
25
75
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below. C18H38(g) ==> C6H14(g) + 2C3H6(g) + 3C2H4(g) What total volume in dm3 of hydrocarbon gases are formed when 20dm3 of the large hydrocarbon are broken down? [rgv-22]
60
120
40
80
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below. C18H38(g) ==> C6H14(g) + 2C3H6(g) + 3C2H4(g) What volume in cm3 of propene gas is formed when 120cm3 of the large hydrocarbon are broken down? [rgv-23]
120
360
240
20
A cracking reaction to break down a large hydrocarbon molecule into, in order, hexane, propene and ethene, is shown below. C18H38(g) ==> C6H14(g) + 2C3H6(g) + 3C2H4(g) What volume in cm3 of ethene gas is formed when 40cm3 of the large hydrocarbon are broken down? [rgv-24]
40
80
240
120
What is the molarity of the solution formed by dissolving 20 g of sodium hydroxide (NaOH) in 1000 cm3 of water? (Ar's: Na=23, O=16, H=1) [msc-1]
0.50
0.25
1.00
2.00
What is the molarity of the solution formed by dissolving 10 g of sodium hydroxide (NaOH) in 500 cm3 of water? (Ar's: Na=23, O=16, H=1) [msc-2]
1.00
0.50
0.25
2.00
What is the molarity of the solution formed by dissolving 80 g of sodium hydroxide (NaOH) in 500 cm3 of water? (Ar's: Na=23, O=16, H=1) [msc-3]
2
1
4
8
What is the molarity of the solution formed by dissolving 9.8 g of
sulfuric acid (H2SO4) in 1000 cm3 of water? (Ar's: H=1, S=32, O=16) [msc-4]
10.0
0.01
1.0
0.1
What is the molarity of the solution formed by dissolving 196 g of
sulfuric acid (H2SO4) in 1000 cm3 of water? (Ar's: H=1, S=32, O=16) [msc-5]
2.0
0.5
3.0
1.5
What is the molarity of the solution formed by dissolving 49 g of
sulfuric acid (H2SO4) in 250 cm3 of water? (Ar's: H=1, S=32, O=16) [msc-6]
0.4
2.0
0.5
1.0
What mass (g) of potassium hydroxide (KOH) is needed to make up 1000cm3 of a solution of concentration 1mol/dm3? (Ar's: K=39, O=16, H=1) [msc-7]
0.056
0.56
56
560
What mass (g) of potassium hydroxide (KOH) is needed to make up 500cm3 of a solution of concentration 0.2mol/dm3? (Ar's: K=39, O=16, H=1) [msc-8]
11.2
2.8
0.56
5.6
What mass (g) of potassium hydroxide (KOH) is needed to make up 500cm3 of a solution of concentration 4.0mol/dm3? (Ar's: K=39, O=16, H=1) [msc-9]
112
56
224
28
What mass (g) of hydrogen chloride (HCl) is needed to make up 1000cm3 of a solution of concentration 1mol/dm3? (Ar's: H=1, Cl=35.5) [msc-10]
73
36.5
0.036
0.073
What mass (g) of hydrogen chloride (HCl) is needed to make up 500cm3 of a solution of concentration 4mol/dm3? (Ar's: H=1, Cl=35.5) [msc-11]
36.5
146
73
292
What mass (g) of hydrogen chloride (HCl) is needed to make up 500cm3 of a solution of concentration 0.2mol/dm3? (Ar's: H=1, Cl=35.5) [msc-12]
7.30
14.6
1.83
3.65
Given the neutralisation equation: NaOH(aq) + HCl(aq) ==> NaCl(aq) + H2O(l) 25 cm3 of hydrochloric acid are neutralised by 20 cm3 of 0.05M sodium hydroxide. What is the molarity of the acid? [vct-1]
0.04
0.02
1.25
0.80
Given the neutralisation equation: NaOH(aq) + HCl(aq) ==> NaCl(aq) + H2O(l) 15 cm3 of hydrochloric acid are neutralised by 25 cm3 of 0.06M sodium hydroxide. What is the molarity of the acid? [vct-2]
0.40
0.10
0.04
0.01
Given the neutralisation equation: NaOH(aq) + HCl(aq) ==> NaCl(aq) + H2O(l) 40 cm3 of 0.05M hydrochloric acid are neutralised by 20 cm3 of a sodium hydroxide solution. What is the molarity of the alkali? [vct-3]
0.20
0.05
0.10
0.50
Given the neutralisation equation: NaOH(aq) + HCl(aq) ==> NaCl(aq) + H2O(l) 25 cm3 of 0.16M hydrochloric acid are neutralised by 10 cm3 of a sodium hydroxide solution. What is the molarity of the alkali? [vct-4]
0.2
0.1
0.8
0.4
Given the neutralisation equation: 2KOH(aq) + H2SO4(aq) ==> K2SO4(aq) + 2H2O(l) What is the molarity of a
sulfuric acid solution, if 15 cm3 of it are neutralised by 20 cm3 of a 0.3 M potassium hydroxide solution? [vct-5]
0.20
0.15
0.40
0.75
Given the neutralisation equation: 2KOH(aq) + H2SO4(aq) ==> K2SO4(aq) + 2H2O(l) What is the molarity of a
sulfuric acid solution, if 30 cm3 of it are neutralised by 10 cm3 of a 0.6 M potassium hydroxide solution? [vct-6]
0.20
0.10
0.05
0.25
Given the neutralisation equation: 2KOH(aq) + H2SO4(aq) ==> K2SO4(aq) +2H2O(l) What is the molarity of a potassium hydroxide solution, if 10 cm3 of it are neutralised by 12 cm3 of a 0.5 M
sulfuric acid solution? [vct-7]
2.4
0.6
1.2
0.6
Given the neutralisation equation: 2KOH(aq) + H2SO4(aq) ==> K2SO4(aq) + 2H2O(l) What is the molarity of a potassium hydroxide solution, if 5 cm3 of it are neutralised by 20 cm3 of a 1 M
sulfuric acid solution? [vct-8]
16
4
5
8
Given the neutralisation equation: 3NaOH(aq) + H3PO4(aq) ==> Na3PO4(aq) + 3H2O(l) What is the molarity of a phosphoric acid solution, if 15 cm3 of it are neutralised by 22.5 cm3 of a 0.2 M sodium hydroxide solution? [vct-9]
0.10
0.30
0.03
0.01
Given the neutralisation equation: 3NaOH(aq) + H3PO4(aq) ==> Na3PO4(aq) + 3H2O(l) What is the molarity of a phosphoric acid solution, if 40 cm3 of it are neutralised by 15 cm3 of a 0.4 M sodium hydroxide solution? [vct-10]
0.150
0.050
0.017
0.115
Given the neutralisation equation: 3NaOH(aq) + H3PO4(aq) ==> Na3PO4(aq) + 3H2O(l) What is the molarity of a sodium hydroxide solution, if 21.6 cm3 of it are neutralised by 18 cm3 of a 0.2 M phosphoric acid solution? [vct-11]
1.50
1.15
0.50
0.17
Given the neutralisation equation: 3NaOH(aq) + H3PO4(aq) ==> Na3PO4(aq) + 3H2O(l) What is the molarity of a sodium hydroxide solution, if 15 cm3 of it are neutralised by 20 cm3 of a 0.6 M phosphoric acid solution? [vct-12]
1.2
7.2
0.8
2.4
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: (-) electrode: 2H+(aq) + 2e- ==> H2(g) (+) electrode: 2Cl-(aq) - 2e- ==> Cl2(g) If 2 g of hydrogen was formed at the (-) electrode, what volume (dm3) of chlorine is formed at the (+) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-1]
24.0
48.0
35.5
71.0
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: (-) electrode: 2H+(aq) + 2e- ==> H2(g) (+) electrode: 2Cl-(aq) - 2e- ==> Cl2(g) If 12 dm3 of hydrogen was formed at the (-) electrode, what mass (g) of chlorine is formed at the (+) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-2]
71.0
35.5
142.0
106.5
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: (-) electrode: 2H+(aq) + 2e- ==> H2(g) (+) electrode: 2Cl-(aq) - 2e- ==> Cl2(g) If 48 dm3 of chlorine was formed at the (+) electrode, what mass (g) of hydrogen is formed at the (-) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-3]
2
1
4
8
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: (-) electrode: 2H+(aq) + 2e- ==> H2(g) (+) electrode: 2Cl-(aq) - 2e- ==> Cl2(g) If 36 dm3 of chlorine was formed at the (+) electrode, what volume (dm3) of hydrogen is formed at the (-) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-4]
48
18
96
36
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: (-) electrode: 2H+(aq) + 2e- ==> H2(g) (+) electrode: 2Cl-(aq) - 2e- ==> Cl2(g) If 213g of chlorine was formed at the (+) electrode, what volume (dm3) of hydrogen is formed at the (-) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-5]
72
36
144
96
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: (-) electrode: 2H+(aq) + 2e- ==> H2(g) (+) electrode: 2Cl-(aq) - 2e- ==> Cl2(g) If 8 g of hydrogen was formed at the (-) electrode, what mass of chlorine (g) is formed at the (+) electrode? [pec-6]
142
284
71
213
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al3O3) and the Ar's: Al=27 and O=16: (-) electrode: 4Al3+(aq) + 12e- ==> 4Al(l) (+) electrode: 6O2-(aq) - 12e- ==> 3O2(g) If 108 g of aluminium is formed at the (-) electrode, what volume (dm3) of oxygen would be formed at the (+) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-7]
144
96
72
36
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al3O3) and the Ar's: Al=27 and O=16: (-) electrode: 4Al3+(aq) + 12e- ==> 4Al(l) (+) electrode: 6O2-(aq) - 12e- ==> 3O2(g) If 54 tonne of aluminium is formed at the (-) electrode, what mass (tonne) of oxygen would be formed at the (+) electrode? [pec-8]
60
24
72
48
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al3O3) and the Ar's: Al=27 and O=16: (-) electrode: 4Al3+(aq) + 12e- ==> 4Al(l) (+) electrode: 6O2-(aq) - 12e- ==> 3O2(g) If 24 g of oxygen is formed at the (+) electrode, what mass (g) of aluminium would be formed at the (-) electrode? [pec-9]
27
54
81
108
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al3O3) and the Ar's: Al=27 and O=16: (-) electrode: 4Al3+(aq) + 12e- ==> 4Al(l) (+) electrode: 6O2-(aq) - 12e- ==> 3O2(g) If 2.7 g of aluminium is formed at the (-) electrode, what volume (dm3) of oxygen would be formed at the (+) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-10]
3.6
1.8
7.2
5.4
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al3O3) and the Ar's: Al=27 and O=16: (-) electrode: 4Al3+(aq) + 12e- ==> 4Al(l) (+) electrode: 6O2-(aq) - 12e- ==> 3O2(g) What mass (g) of aluminium is formed at the (-) electrode, if 72 dm3 of oxygen was formed at the (+) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-11]
54
27
108
81
Given below are the electrode equations for the electrolysis of molten aluminium oxide ore (Al3O3) and the Ar's: Al=27 and O=16: (-) electrode: 4Al3+(aq) + 12e- ==> 4Al(l) (+) electrode: 6O2-(aq) - 12e- ==> 3O2(g) If 54 g of aluminium is formed at the (-) electrode, what volume (dm3) of oxygen was formed at the (+) electrode? (1 mole of any gas = 24dm3 at room temp./press.) [pec-12]
18
72
54
36
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Given the following relative atomic masses: Cu = 64, S = 32 and O = 16; calculate the relative formula mass of copper
sulfate, CuSO4 [rfm-1]
Given the following symbol equation:
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of copper in copper(II)
sulfate, CuSO4 [pbm-1]
If 54g of aluminium combines with oxygen to form 102g of aluminium oxide, work out the formula of aluminium oxide. (Relative atomic masses: Al = 27 and O = 16) [emp-1]
Given the equation: 2Mg(s) + O2(g) ==> 2MgO(s)
Chlorine consists of 75% chlorine-35 and 25% chlorine-37. Calculate the Ar of chlorine to 3sf/1dp. [ram-1]
How many moles of iron are there in 2.8g? (atomic mass Fe = 56) [mam-1]
0.55g of boron combined with 1.2g of oxygen. Deduce the empirical formula of boron oxide.
Given the equation: 2Na(s) + 2H2O(l) ==> 2NaOH(aq) + H2(g)
What is the molarity of the solution formed by dissolving 20 g of sodium hydroxide (NaOH) in 1000 cm3 of water? (Ar's: Na=23, O=16, H=1) [msc-1]
Given the neutralisation equation:
Given below are the electrode equations for the electrolysis of aqueous sodium chloride (brine) and the Ar's: H=1 and Cl=35.5: