m/c QUIZ of basic chemical calculations for easier-foundation
tier GCSE level (NO 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
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foundation tier GCSE multiple choice calculation questions useful for US grade 9-10 chemistry student courses
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)