Mole exercise answer 2

What mass of zinc sulfate-7-water could be made from 1.00 g of zinc metal reacting with excess sulfuric acid?

We don't really need a full equation. We know that it takes one mole of zinc to make one mole of the hydrated salt (as the salt contains one mole of zinc):

Zn(s) ⇒ ZnSO₄.7H₂O(s)

Zn = 65.3

\ number of moles of Zn = 1.00/65.3 = 0.0153 mol

Zn º ZnSO₄.7H₂O

\ number of moles of ZnSO₄.7H₂O = 1 × 0.0153 = 0.0153 mol

ZnSO₄.7H₂O = 287.3

\ mass of KHCO₃ = 0.0153 × 287.3 = 4.40 g