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Amounts Of Substances In Equations (ht Only) (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Amounts Of Substances In 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 25.0 cm3 sample of 0.100 mol/dm3 NaOH is titrated with HCl. How many moles of HCl are required to neutralise it? (NaOH + HCl ? NaCl + H2O)
What is the mass of 1.00 mol of sodium atoms? (Ar Na = 22.99)
A sample contains 12.0 g of carbon. How many moles of carbon atoms are present?
A reaction has a maximum theoretical salt mass of 12.5 g. If the percentage yield is 92.8%, what mass of salt is actually produced?
How many molecules are in 2.00 mol of CO2? (Avogadro constant = 6.02 × 10^23 mol-1)
Which volume corresponds to 375 moles of gas at RTP (1 mol = 24.0 dm3)?
Calculate the minimum mass of magnesium needed to reduce 1.20 kg of silicon dioxide according to: 2 Mg + SiO2 ? Si + 2 MgO. (Ar: Mg = 24)
Calculate the moles of CO2 produced when 40.0 kg Fe2O3 reacts with excess carbon according to 2 Fe2O3 + 3 C ? 4 Fe + 3 CO2. (Mr Fe2O3 = 160; 1 mol gas = 24.0 dm3 but here moles requested)
What is the formula mass (Mr) of CaCO3? (Ar: Ca = 40.1, C = 12.0, O = 16.0)
The reaction: 2 A + 3 B ? 4 C. If you start with 0.500 mol A and an excess of B, how many moles of C can be formed?
Which relative atomic mass (Ar) corresponds to element with isotopic data: mass-6 (7.6%), mass-7 (92.4%)? Give answer to 1 decimal place.