If 4.56 mol of zinc react with excess copper (ii) sulphate, how many moles of precipitate will be formed?

This is done the same way as the HNO3 problem.

To determine the number of moles of precipitate formed, we need to know the balanced chemical equation for the reaction between zinc and copper (II) sulfate.

The balanced equation is as follows:
Zn(s) + CuSO4(aq) -> ZnSO4(aq) + Cu(s)

From the reaction stoichiometry, we can see that one mole of zinc reacts with one mole of copper (II) sulfate to produce one mole of zinc sulfate and one mole of copper precipitate.

Given that we have 4.56 moles of zinc, we can conclude that 4.56 moles of copper (II) sulfate will be required for complete reaction.

Thus, the number of moles of precipitate formed will also be 4.56 moles.