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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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For N2 + 3H2 ? 2NH3, if 10.0 dm3 H2 reacts with excess N2 at RTP, what volume NH3 (dm3) is formed?
A theoretical yield is 50.0 g but the actual mass collected is 40.0 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?
A compound has mass composition 40.0% C, 6.7% H and 53.3% O by mass. What is its empirical formula?
CaCO3 ? CaO + CO2. If 10.0 g CaCO3 decomposes fully, how many moles CO2 are formed? (Mr CaCO3 = 100.0)
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?
CH4 + 2O2 ? CO2 + 2H2O. If 10.0 dm3 O2 are consumed at RTP, what volume of CO2 is produced (RTP same conditions)?
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?
In combustion 2Fe2O3 + 3C ? 4Fe + 3CO2. If 40.0 kg Fe2O3 is reduced completely with excess C, what volume of CO2 (dm3) is produced at RTP (1 mol gas = 24.0 dm3, Mr Fe2O3 = 160)?
In Fe3O4 what is the percentage by mass of iron? (Ar Fe 56, O 16)
Which set of smallest whole-number coefficients balances Fe + O2 ? Fe2O3 ?