Question

Joel reacted 0.9845 g of iron fillings with an excess of copper sulphate solution. When the reaction was complete the solution had changed from blue to green and a copper deposit weighing 1.024 g had formed in the solution. In this reaction, metallic iron is converted into ferrous ion (Fe2+) and cupric ion (Cu2+) is converted into metallic copper.

b) Calculate the theoretical mass of copper that was expected to be produced and hence determine the percentage yield of Joel’s experiment.



c) How many molecules of iron are present in 0.9845 g of iron fillings?