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

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?

2H2 + O2 ? 2H2O. If 3.50 dm3 of H2 is reacted completely at room temperature and pressure, how much air (volume in dm3) is needed if air contains 20% oxygen by volume?

Which method ensures the mass of a reacting system remains constant during a reaction that produces gas so students can easily demonstrate conservation of mass?

Which experimental change will make the measured mass decrease during a reaction more accurately reflect the mass of gas evolved rather than being underestimated?

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?

Calcium carbonate decomposes: CaCO3 ? CaO + CO2. If 10.0 g of CaCO3 completely decomposes and all the CO2 escapes, what mass of CaO remains?

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.)

If a reaction produces 0.20 mol of gas at room temperature and pressure (use 24.0 dm3 per mole), what volume of gas is produced in dm3?

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)?

When 1.00 g of carbon is completely oxidised to CO2 (oxygen supplied from air), by how much does the mass of the carbon sample increase? (Ar C = 12, O = 16)

When magnesium ribbon burns in air to form magnesium oxide the measured mass of the sample increases. Why?