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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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A theoretical yield of a product is 10.0 g but the actual mass obtained is 7.50 g. What is the percentage yield?
In Fe3O4 what is the percentage by mass of iron? (Ar Fe 56, O 16)
When 0.500 mol of gas at RTP occupies 12.0 dm3, what is the molar volume assumed in the calculation?
CH4 + 2O2 ? CO2 + 2H2O. If 10.0 dm3 O2 are consumed at RTP, what volume of CO2 is produced (RTP same conditions)?
2Al + 3CuO ? Al2O3 + 3Cu. If 54.0 g CuO reacts with excess Al, what mass of Cu forms? (Ar Cu 63.5, CuO Mr 79.5)
CaCO3 ? CaO + CO2. If 10.0 g CaCO3 decomposes fully, how many moles CO2 are formed? (Mr CaCO3 = 100.0)
Which set of smallest whole-number coefficients balances Fe + O2 ? Fe2O3 ?
2Al + 3CuSO4 ? Al2(SO4)3 + 3Cu. If you have 0.500 mol CuSO4, how many moles Al are required?
What is the limiting reagent and how many moles of CO2 are made when 1.50 mol NH3 reacts with 0.60 mol O2 in the reaction 4NH3 + 5O2 ? 4NO + 6H2O?
2Al + 3Cl2 ? 2AlCl3. What is the atom economy for producing AlCl3 (mass of desired product ÷ mass of reactants ×100)? (Use Ar Al 27.0, Cl 35.5)
2HCl + Ba(OH)2 ? BaCl2 + 2H2O. If 23.50 cm3 of 0.100 mol/dm3 Ba(OH)2 neutralises 25.00 cm3 HCl, what is the concentration of HCl in mol/dm3?