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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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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?
A compound has mass composition 40.0% C, 6.7% H and 53.3% O by mass. What is its empirical formula?
2Al + 3CuSO4 ? Al2(SO4)3 + 3Cu. If you have 0.500 mol CuSO4, how many moles Al are required?
2H2 + O2 ? 2H2O. If 3.50 dm3 H2 is reacted completely with excess O2 at RTP, how much air (dm3) is needed if air is 20% oxygen by volume?
In Fe3O4 what is the percentage by mass of iron? (Ar Fe 56, O 16)
A theoretical yield is 50.0 g but the actual mass collected is 40.0 g. What is the percentage yield?
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)
Fe + 2HCl ? FeCl2 + H2. If 5.00 g Fe reacts with excess HCl, what volume of H2 (dm3) is produced at RTP (1 mol gas = 24.0 dm3)? (Ar Fe 56.0)
2Na + Cl2 ? 2NaCl. If 46.0 g sodium reacts with excess chlorine, what mass of NaCl is formed? (Ar: Na 23.0, Cl 35.5)
A balanced equation is 2Al + 3Cl2 ? 2AlCl3. If 0.100 mol Cl2 reacts completely, how many moles of Al are required?
If 12.0 g carbon reacts with 64.0 g O2 (C + O2 ? CO2), what mass of CO2 is produced? (Ar C 12, O 16)