Type in answer QUIZ of chemical calculations for harder-higher GCSE level @ doc brown's chemistry (includes moles)
Type in formula without subscripts e.g. Fe3O4 even though it is correctly written as Fe3O4
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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 relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of ethane, C2H6 [rfm-2]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of octane, C8H18 [rfm-3]
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of nitric acid, HNO3 [rfm-4]
Given the following relative atomic masses: H = 1, N = 14 and O = 16; calculate the relative formula mass of ammonium nitrate, NH4NO3 [rfm-5]
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]
Given the following relative atomic masses: H = 1, O = 16 and S = 32; calculate the relative formula mass of sulfuric acid, H2SO4 [rfm-7]
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]
Given the following relative atomic masses: H = 1 and Cl = 35.5, calculate the relative formula mass of hydrochloric acid, HCl [rfm-9]
Given the following relative atomic masses: Na = 23 and Cl = 35.5, calculate the relative formula mass of sodium chloride, NaCl [rfm-10]
Given the following relative atomic masses: Ca = 40 and Cl = 35.5, calculate the relative formula mass of calcium chloride, CaCl2 [rfm-11]
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]
Given the following relative atomic masses: Al = 27 and Cl = 35.5, calculate the relative formula mass of aluminium chloride, AlCl3 [rfm-13]
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]
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of glucose, C6H12O6 [rfm-5]
Given the following relative atomic masses: H = 1, C = 12 and O = 16; calculate the relative molecular mass of ethanol ('alcohol'), C2H5OH [rfm-16]
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]
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(II) oxide, FeO [rfm-18]
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of iron(III) oxide, Fe2O3 [rfm-19]
Given the following relative atomic masses: O = 16 and Fe = 56; calculate the relative formula mass of the iron oxide, Fe3O4 [rfm-20]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of methane, CH4 [rfm-21]
Given the following relative atomic masses: H = 1 and C = 12; calculate the relative molecular mass of propane, C3H8 [rfm-22]
Given the following relative atomic masses: C = 12 and O = 16; calculate the relative molecular mass of carbon dioxide, CO2 [rfm-23]
Given the following relative atomic masses: C = 12, O = 16 and Cu = 64; calculate the relative formula mass of copper carbonate, CuCO3 [rfm-23]
Given the following relative atomic masses: C = 12, O = 16 and Ca = 40; calculate the relative formula mass of calcium carbonate, CaCO3 [rfm-23]
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of copper in copper(II) sulfate, CuSO4 [pbm-1]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in ethane, C2H6 [pbm-2]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in octane, C8H18 [pbm-3]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of hydrogen in nitric acid, HNO3 [pbm-4]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of hydrogen in ammonium nitrate, NH4NO3 [pbm-5]
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]
Given the atomic masses: H = 1, O = 16 and S = 32; calculate the % by mass of hydrogen in sulfuric acid, H2SO4 [pbm-7]
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]
Given the atomic masses: H = 1 and Cl = 35.5, calculate the % by mass of hydrogen in hydrogen chloride, HCl [pbm-9]
Given the atomic masses: Na = 23 and Cl = 35.5, calculate the % by mass of sodium in sodium chloride, NaCl [pbm-10]
Given the atomic masses: Ca = 40 and Cl = 35.5, calculate the % by mass of calcium in calcium chloride, CaCl2 [pbm-11]
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]
Given the atomic masses: Al = 27 and Cl = 35.5, calculate the % by mass of aluminium in aluminium chloride, AlCl3 [pbm-13]
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]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of carbon in glucose, C6H12O6 [pbm-15]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of carbon in ethanol ('alcohol'), C2H5OH [pbm-16]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in iron(II) oxide, FeO [pbm-17]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in iron(II) oxide, FeO [pbm-18]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in iron(III) oxide, Fe2O3 [pbm-19]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of iron in the iron oxide, Fe3O4 [pbm-20]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in methane, CH4 [pbm-21]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of carbon in propane, C3H8 [pbm-22]
Given the atomic masses: C = 12 and O = 16; calculate the % by mass of oxygen in carbon dioxide, CO2 [pbm-23]
Given the atomic masses: C = 12, O = 16 and Cu = 64; calculate % by mass of copper in copper carbonate, CuCO3 [pbm-24]
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of calcium in calcium carbonate, CaCO3 [pbm-25]
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of oxygen in copper(II) sulfate, CuSO4 [pbm-26]
Given the atomic masses: Cu = 64, S = 32 and O = 16; calculate the % by mass of sulfur in copper(II) sulfate, CuSO4 [pbm-27]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in ethane, C2H6 [pbm-28]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in octane, C8H18 [pbm-29]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of oxygen in nitric acid, HNO3 [pbm-30]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of nitrogen in nitric acid, HNO3 [pbm-31]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of nitrogen in ammonium nitrate, NH4NO3 [pbm-32]
Given the atomic masses: H = 1, N = 14 and O = 16; calculate the % by mass of oxygen in ammonium nitrate, NH4NO3 [pbm-33]
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]
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]
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]
Given the atomic masses: H = 1, O = 16 and S = 32; calculate the % by mass of oxygen in sulfuric acid, H2SO4 [pbm-37]
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]
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]
Given the atomic masses: H = 1 and Cl = 35.5, calculate the % by mass of chlorine in hydrogen chloride, HCl [pbm-40]
Given the atomic masses: Na = 23 and Cl = 35.5, calculate the % by mass of chlorine in sodium chloride, NaCl [pbm-41]
Given the atomic masses: Ca = 40 and Cl = 35.5, calculate the % by mass of chlorine in calcium chloride, CaCl2 [pbm-42]
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]
Given the atomic masses: Al = 27 and Cl = 35.5, calculate the % by mass of chlorine in aluminium chloride, AlCl3 [pbm-44]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of hydrogen in glucose, C6H12O6 [pbm-45]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of oxygen in glucose, C6H12O6 [pbm-46]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of hydrogen in ethanol ('alcohol'), C2H5OH [pbm-47]
Given the atomic masses: H = 1, C = 12 and O = 16; calculate the % by mass of oxygen in ethanol ('alcohol'), C2H5OH [pbm-48]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in iron(III) oxide, Fe2O3 [pbm-49]
Given the atomic masses: H = 1 and C = 12; calculate the % by mass of hydrogen in methane, CH4 [pbm-50]
Given the atomic masses: O = 16 and Fe = 56; calculate the % by mass of oxygen in the iron oxide, Fe3O4 [pbm-51]
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of carbon in calcium carbonate, CaCO3 [pbm-52]
Given the atomic masses: C = 12, O = 16 and Ca = 40; calculate the % by mass of oxygen in calcium carbonate, CaCO3 [pbm-53]
If 54g of aluminium combines with oxygen to form 102g of aluminium oxide, what is the formula of aluminium oxide? (Relative atomic masses: Al = 27 and O = 16) [emp-1]
In an experiment, 56g of iron combined with exactly 64g of sulfur. What is the formula of the iron sulfide formed? (Relative atomic masses: Fe = 56 and S = 32) [emp-2]
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]
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]
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]
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]
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]
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]
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]
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]
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]
If 16g of sulfur combines with 103.5g of lead, what is the formula of the lead sulfide formed? (Relative atomic masses: Pb = 207 and S = 32) [emp-12]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
If 54g of aluminium combines with 96g of sulfur, what is the formula of aluminium sulfide? (Relative atomic masses: = and = ) [emp-23]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
Chlorine consists of 75% chlorine-35 and 25% chlorine-37. Calculate the Ar of chlorine to 3sf/1dp. [ram-1]
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]
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]
Boron is 19.7% B-10 and 80.3% B-11. Calculate the relative atomic mass, Ar, of boron to 3sf/1dp. [ram-4]
Antimony (Sb) is 57.2% Sb-121 and 42.8% Sb-123. Calculate the Ar of Sb to 4sf/1dp. [ram-5]
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]
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]
Europium consists of 47.8% Eu-151 and 52.2% Eu-153. Calculate Ar(Eu) to 4sf/1dp. [ram-8]
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]
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]
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]
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]
Rhenium (Re) consists of 37.1% 185Re and 62.9% 187Re. Calculate the relative atomic mass, Ar, of rhenium to 4sf/1dp. [ram-13]
Rubidium consists of the stable isotopes: 85Rb (72.2%) and 87Rb (27.8%). Calculate Ar(Rb) to 3sf/1dp. [ram-14]
Thallium consists of 29.5% thallium-203 and 70.5% thallium-205. Calculate the relative atomic mass, Ar, of to 4sf/1dp. [ram-15]
How many moles of iron are there in 2.8g? (atomic mass Fe = 56) [mam-1]
How many moles of sulfur are there in 64g? (atomic mass S = 32) [mam-2]
How many moles of sodium are there in 115g? (atomic mass Na = 23) [mam-3]
How many moles of carbon are there in 3g? (atomic mass C = 12 ) [mam-4]
How many moles of zinc are there in 1.625g? (atomic mass Zn = 65) [mam-5]
How many moles of iodine are there in 12.7g of I2? (atomic mass I = 127) [mam-6]
How many moles of chlorine are there in 213g of Cl2? (atomic mass Cl = 35.5) [mam-7]
How many moles of bromine are there in 6.4g of Br2? (atomic mass Br = 80) [mam-8]
How many moles of phosphorus are there in 24.8g of P4? (atomic mass P = 31) [mam-9]
How many moles of oxygen are there in 128g of O2? (atomic mass O = 16) [mam-10]
How many moles of water are there in 4.5g of H2O? (atomic masses: H = 1, O = 16) [mam-11]
How many moles of methane are there in 112g of CH4? (atomic masses: C = 12, H = 1) [mam-12]
How many moles of sodium sulfate are there in 7.1g of Na2SO4? (atomic masses: Na = 23, S = 32, O = 16) [mam-13]
How many moles of sulfuric acid are there in 2.45g of H2SO4? (atomic masses: H = 1, S = 32, O = 16) [mam-14]
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]
How many g are there in 1.5 moles of aluminium? (atomic mass Al = 27) [mam-16]
How many g are there in 0.02 moles of uranium? (atomic mass U = 238) [mam-17]
How many g are there in 0.65 moles of magnesium? (atomic mass Mg = 24) [mam-18]
How many g are there in 0.23 moles of silicon? (atomic mass Si = 28) [mam-19]
How many g are there in 7.3 moles of boron? (atomic mass B = 10.8) [mam-20]
How many g are there in 0.05 moles of nitrogen, N 2? (atomic mass N = 14) [mam-21]
How many g are there in 0.75 moles of ozone, O3? (atomic mass O = 16) [mam-22]
How many g are there in 2.5 moles of oxygen, O2? (atomic mass O = 16) [mam-23]
How many g are there in 0.16 moles of chlorine, Cl2? (atomic mass Cl = 35.5) [mam-24]
How many g are there in 1.65 moles of iodine, I2? (atomic mass I = 127) [mam-25]
How many g are there in 3.6 moles of sodium hydroxide, NaOH? (atomic masses: Na = 23, O = 16, H = 1) [mam-26]
How many g are there in 1.5 moles of nitric acid, HNO3? (atomic masses: H = 1, N = 14, O = 16) [mam-27]
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]
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]
How many g are there in 0.005 moles of sodium thiosulfate, Na2S2O3? (atomic masses: Na = 23, S = 32, O =16) [mam-30]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
An 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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
0.800g of magnesium reacted with 8.467g of iodine. Calculate the empirical formula for magnesium iodide.? (relative atomic masses, Ar: Mg = 24, I = 127) [efm-46]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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 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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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]
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questions useful for US grade 9-10 chemistry student courses
Given the following symbol equation:
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 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, what is 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. (relative atomic masses, Ar: B = 11, O = 16) [efm-1]
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: