An impure sample of zinc (Zn) is treated with an excess of sulfuric acid (H2SO4) to form zinc sulfate (ZnSO4) and molecular hydrogen (H2).

(a) Write a balanced equation for the reaction.

Zn(s) + →

(b) How many moles are in 3.70 g of pure zinc?

_ mol

(c) How many moles of hydrogen gas are formed if one mole of zinc is treated with excess sulfuric acid?

_mol

(d) If 3.70 g of pure Zn is treated with excess sulfuric acid, how many grams of hydrogen could be collected?

_ g

(e) If 0.0660 g of H2 is obtained from 3.70 g of impure sample, what is the percent purity of the sample?

_ %