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CGB IGCSE Chemistry
Mole Worksheet 2
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Mole Worksheet 2

 

  1. Calcium carbonate decomposes when heated to form calcium oxide and carbon dioxide.

CaCO3(s) CaO(s) + CO2(g)

    1. Calculate the mass of one mole of calcium carbonate.
    2. Calculate the mass of one mole of calcium oxide.
    3. Calculate the mass of one mole of carbon dioxide.
    4. If 12.2 moles of calcium carbonate are heated, how many moles of calcium oxide and carbon dioxide are produced?
    5. Find out how much calcium oxide is produced if 10 g of calcium carbonate is heated.
    6. Find out how much carbon dioxide is produced if 200 g of calcium carbonate is heated.

 

  1. When Iron(III)oxide is heated with carbon monoxide, iron(III)oxide is reduced to iron and carbon monoxide is oxidised to carbon dioxide.

Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)

    1. Calculate the mass of 1 mole of Iron(III)oxide.
    2. How many moles are participating in the reaction?

                                                               i.      Fe2O3

                                                             ii.      CO

                                                            iii.      Fe

                                                           iv.      CO2

    1. Calculate the mass of 1 mole of CO
    2. Calculate the mass of 1 mole of Fe
    3. Calculate the mass of 1 mole of CO2
    4. If one mole of Fe2O3 is heated with excess CO, how many moles of Fe are produced?
    5. If two moles of CO are heated with excess Fe2O3, how many moles of CO2 are produced?
    6. If you have 0.5 moles of Fe2O3, how many moles of CO do you need to make 1   mole of Fe?
    7. If 1.6g of Fe2O3 is heated with excess CO, how much Fe is produced?

 

  1. When magnesium is heated in the presence of oxygen, magnesium oxide is formed.

2 Mg (s) + O2 (g) 2 MgO (s)

    1. How many grams of oxygen will react with 48 g of magnesium?
    2. How many grams of oxygen will react with 2.4 g of magnesium?
    3. How many grams of magnesium will react with 64 g of oxygen?
    4. If 10 g of magnesium and 11 g of oxygen are used, which substance is in excess?
    5. If 10 g of magnesium and 11 g of oxygen are used, name the substances present when the reaction is complete, and find the mass of each.

 

  1. H2 (g) + Br2 (g) 2 HBr (g)
    1. 1 mole of H2 reacts with 1 mole of Br2 to form how many moles of HBr?
    2. If you have 0.6 moles of Br2 and excess H2 how many moles of HBr will you make?
    3. How many grams of Bromine will react with 5 g of hydrogen?
    4. How many grams of hydrogen will react with 80 grams of bromine?
    5. If 40 grams of bromine and 1 gram of hydrogen are used, which gas is in excess?
    6. If 40 grams of bromine and 1 gram of hydrogen are used, name the substances present when the reaction is complete and find the mass of each.

 

  1. Sulfuric acid is neutralized by copper oxide to form  16 grams copper sulfate and water.

CuO(s) + H2SO4(aq) CuSO4(aq) + H2O(l)

    1. What is the relative formula mass of copper sulfate?
    2. How many moles of copper sulfate were produced?
    3. How many moles of CuO and H2SO4 had to react to form 16 g of copper sulfate?
    4. How could the copper sulfate be separated from the water?

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