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Conservation Of Mass And Balanced Chemical Equations (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Conservation Of Mass And Balanced Chemical Equations' from the broader topic Quantitative Chemistry. The test is geared towards the AQA exam board style syllabus.
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Below a typical questions that will be covered in this test. You final score will be logged on your account

An element X forms an oxide X2O3. If 2.00 g of X combine with 0.48 g oxygen, what is the relative atomic mass (Ar) of X (approx)?
If a balanced equation gives a mole ratio 1:2:1 (A:B:C) and you start with 1.00 mol A and 5.00 mol B, which is limiting and how many moles of C form?
Balance the redox equation by inspection: Fe2O3 + C ? Fe + CO. The coefficient for C is:
What is the empirical formula of a compound that is 40.0% C, 6.7% H, 53.3% O by mass (approx)?
At RTP 1 mole of any gas occupies 24.0 dm3. If 48.0 dm3 of oxygen is collected, how many moles is that?
Sodium reacts with chlorine gas to form sodium chloride. Which balanced equation is correct?
When gas volumes are measured and conditions are constant, which quantity is directly proportional to number of moles of gas?
Which calculation gives the concentration (mol/dm3) if you have 0.0150 mol dissolved in 30.0 cm3 of solution?
When 2.00 mol of hydrogen reacts completely with 1.00 mol of oxygen to form water, what mass (g) of water is produced? (Mr H2O = 18.0)
Which calculation gives the number of moles in 36.0 g of water (H2O)? (Ar H = 1, O = 16)
A reaction A + B ? C is found to produce 30.0 g of product C from 50.0 g total starting mass of A + B in a closed system with no mass lost. How much mass of unreacted material remains in the container after reaction?