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 number of moles of iron used and the number of moles of copper
formed.

Answer 1

Fe(s) + CuSO4(aq) ==> FeSO4(aq) + Cu(s)
moles Fe used = g/atomic mass = 0.9845 g Fe/atomic mass Fe = ?
moles Cu formed = 1.024/atomic mass Cu = ?