If 87 grams of sulfuric acid were used in the following reaction, how many liters of hydrogen would be collected at STP? 2Fe + 3H2SO4 → 3H2 + Fe2(SO4)3

Answer 1

2Fe + 3H2SO4 → 3H2 + Fe2(SO4)3

Find moles of H2SO4 used.

Convert that to mole of H2 gas formed

Convert that to liters of H2 gas (recall that 1 mol of an ideal gas = 22.4 L at STP)

Moles H2SO4 = 87 g H2SO4 x 1 mol / 98 g = 0.888 moles H2SO4

Moles H2 gas formed = 0.888 mols H2SO4 x 3 mols H2 / 3 mols H2SO4 = 0.888 mols H2 gas formed

Liters of H2 gas @STP = 0.888 moles H2 x 22.4 L / mol = 19.9 L H2 gas formed