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Mass Changes When A Reactant Or Product Is A Gas (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Mass Changes When A Reactant Or Product Is A Gas' 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

When a reactant gas is used up in an open vessel and the gas is not replaced, which laboratory observation is expected?
Calcium carbonate decomposes: CaCO3 ? CaO + CO2. If 10.0 g of CaCO3 completely decomposes and all the CO2 escapes, what mass of CaO remains?
24.0 cm3 of hydrogen is collected at room temperature and pressure in an open experiment where H2 escapes from the system. How many moles of H2 does this represent? (Use 24 dm3 = 24 000 cm3 per mole.)
A student measures the mass of a beaker + contents before and after a reaction that produces hydrogen gas which is collected. The measured mass decreases by 0.016 g. Which statement best explains the change?
A carbonate reacts with acid producing 0.10 mol CO2 that escapes. What volume (in dm3) does this gas occupy at room temperature and pressure (24 dm3 per mole)?
A student completely reacts 5.00 g of Na2CO3 with acid producing CO2 that escapes. (Mr Na2CO3 = 106, CO2 = 44) What mass of CO2 is produced and lost?
A container initially contains 1.00 g of hydrated copper sulfate. After heating to drive off water the mass is 0.64 g. What mass of water was lost?
When 1.00 g of methane (CH4) is burned in an open system and CO2 escapes, what happens to the mass of the remaining solids/liquids?
A student reacts 2.00 g of zinc with excess hydrochloric acid in an open flask (Zn ? Zn2+ + 2 e-; reaction produces H2 gas). Using Zn Ar = 65.4, how much mass is lost from the system when the reaction produces hydrogen gas? (Give an approximate value.)
A sample of 11.7 g of hydrated copper sulfate changes to 2.99 g anhydrous CuSO4 and 1.47 kJ of energy is absorbed when 4.68 g of hydrate changed to 2.99 g anhydrous. Using these ratios, calculate the maximum mass of water that can be produced from 11.7 g of hydrated copper sulfate. (Use proportional scaling.)
A sealed container is used when a solid reacts with oxygen to form a solid oxide. What happens to the mass of the sealed container during the reaction?