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.
Calculate the number of moles of iron used and the number of moles of copper
formed.
Answers
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 = ?
moles Fe used = g/atomic mass = 0.9845 g Fe/atomic mass Fe = ?
moles Cu formed = 1.024/atomic mass Cu = ?