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

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 reaction produces gas that is dissolved in the liquid rather than escaping. If later the liquid is heated and gas evolves, what will an open-balance measurement show while gas is dissolved and then after heating?

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.)

When a reactant gas is used up in an open vessel and the gas is not replaced, which laboratory observation is expected?

If 0.50 mol of gas is produced at room temperature and pressure, how many cm3 of gas is this (use 24 dm3 per mole)?

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?

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?

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.)

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

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