Can anyone show me how to do this - this question was on the specimen paper:
After reaction of some zinc metal with excess sulfuric acid, a student collected 40.8 g of ZnSO4.7H2O crystals. The yield of crystals was 70.0%. What was the original mass of zinc used?
Work out what a 100% yield would be - 58. 3 With this number divide by the Mr of ZnSO4. 7H2O then multiply by the Mr of Zn metal . I think this is right
Work out what a 100% yield would be - 58. 3 With this number divide by the Mr of ZnSO4. 7H2O then multiply by the Mr of Zn metal . I think this is right
1 mole of zinc reacts to give you 1 mole of hydrated zinc sulfate, so the number of moles of zinc in the product will be the same as the number of moles of zinc in the reactant.
1 mole of zinc reacts to give you 1 mole of hydrated zinc sulfate, so the number of moles of zinc in the product will be the same as the number of moles of zinc in the reactant.
But there are more H and O's on the right of equation?
But there are more H and O's on the right of equation?
This is because the solution is aqueous so you will have H and O in it. However, the number of mol of zinc cannot change from left to right. If you look at your product, you only have 1 mol of zinc.