Chromium metal reacts with dilute sulfuric acid according to the following unbalanced equation: Cr (s) + H2SO4 (aq) Cr2(SO4)3 (aq) + H2 (g)

Suppose you react 3.51 g of chromium metal with excess dilute sulfuric acid.

(a) What mass of Cr2(SO4)3, in grams, can be obtained?

(b) What mass of hydrogen gas, in grams, can be obtained?

(c) If only 10.3 g of Cr2(SO4)3 is obtained, what is the percentage yield? Formula weight: Cr2(SO4)3 392.183 g/mol