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.

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.

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

Answer 1

See your other post for Fe moles used and Cu moles formed.

moles Fe used = theoretical moles Cu formed.
Theoretial moles Cu formed x atomic mass Cu = theoretical g Cu formed.
% yield = 100*(actual g Cu formed/theoretical g Cu formed)
Post your work if you get stuck.