6.5 g of zinc was treated with a dilute solution containing 12 g of sulfuric acid. Determine the amount of hydrogen evolved.

The reaction of zinc with sulfuric acid is described by the following chemical reaction equation:

Zn + H2SO4 = ZnSO4 + H2;

Let’s determine the amount of a substance contained in 6.5 grams of zinc and 12 grams of sulfuric acid.

N Zn = 6.5 / 65 = 0.1 mol;

M H2SO4 = 1 + 1 + 32 + 16 x 4 = 98 grams / mol;

N H2SO4 = 12/98 = 0.122 mol;

Therefore, in the course of the reaction, no more than 0.1 mol of hydrogen will be formed. Let’s find its volume:

Under normal conditions, one mole of ideal gas takes up a volume of 22.4 liters.

V H2 = 0.1 x 22.4 = 2.24 liters;