A laboratory technician heats a sample of basic copper carbonate, Cu2CO3(OH)2\text{Cu}_2\text{CO}_3(\text{OH})_2Cu2CO3(OH)2, to decompose it into solid copper(II) oxide, water vapour, and carbon dioxide gas:
Cu2CO3(OH)2(s)→2CuO(s)+H2O(g)+CO2(g) \text{Cu}_2\text{CO}_3(\text{OH})_2(\text{s}) \rightarrow 2\text{CuO}(\text{s}) + \text{H}_2\text{O}(\text{g}) + \text{CO}_2(\text{g}) Cu2CO3(OH)2(s)→2CuO(s)+H2O(g)+CO2(g)The technician starts with 15.540 g of basic copper carbonate in a crucible. After heating strongly until the reaction is complete, the mass of the solid copper(II) oxide residue remaining in the crucible is 11.170 g.
Calculate the total mass of the gaseous products that escaped during the reaction.
258 exam-style questions on Edexcel GCSE Chemistry Calculations involving masses. Each one has a worked solution and a mark scheme showing where the marks go.