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Using Moles To Balance Equations (ht Only) (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Using Moles To Balance Equations (ht Only)' from the broader topic Quantitative Chemistry. The test is geared towards the AQA exam board style syllabus.
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CaCO3 ? CaO + CO2. If 10.0 g CaCO3 decomposes fully, how many moles CO2 are formed? (Mr CaCO3 = 100.0)
A theoretical yield of a product is 10.0 g but the actual mass obtained is 7.50 g. What is the percentage yield?
2H2 + O2 ? 2H2O. If you start with 3.00 mol H2 and 1.00 mol O2, which statement is correct about the limiting reagent and moles of H2O formed?
Propane combusts: C3H8 + 5O2 ? 3CO2 + 4H2O. If 5.00 g propane burns completely, how many moles of CO2 are produced? (Mr propane = 44.0)
Which set of smallest whole-number coefficients balances Fe + O2 ? Fe2O3 ?
CH4 + 2O2 ? CO2 + 2H2O. If 10.0 dm3 O2 are consumed at RTP, what volume of CO2 is produced (RTP same conditions)?
A balanced equation is 2Al + 3Cl2 ? 2AlCl3. If 0.100 mol Cl2 reacts completely, how many moles of Al are required?
When 0.500 mol of gas at RTP occupies 12.0 dm3, what is the molar volume assumed in the calculation?
2Al + 3CuSO4 ? Al2(SO4)3 + 3Cu. If you have 0.500 mol CuSO4, how many moles Al are required?
For N2 + 3H2 ? 2NH3, if 10.0 dm3 H2 reacts with excess N2 at RTP, what volume NH3 (dm3) is formed?
In Fe3O4 what is the percentage by mass of iron? (Ar Fe 56, O 16)