Determine the volume of hydrogen that will be released when 104 g of zinc react with an excess of sulfuric acid.

Determine the volume of hydrogen that will be released when 104 g of zinc react with an excess of sulfuric acid. How much iron (III) oxide can be reduced to iron using the hydrogen produced?

Zinc dissolves in sulfuric acid, the reaction proceeds according to the following chemical equation:

Zn + H2SO4 = ZnSO4 + H2;

Let’s determine the chemical amount of zinc. For this purpose, we divide its weight by the molar weight of elemental zinc.

M Zn = 65 grams / mol;

N Zn = 104/65 = 1.6 mol;

The same amount of hydrogen will be released.

Let’s find its volume.

To do this, we multiply the amount of substance by the volume of 1 mole of gas (filling the space of 22.4 liters).

V H2 = 1.6 x 22.4 = 35.84 liters;

The reduction of iron oxide is described by the following reaction:

Fe2O3 + 3 H2 = 2Fe + 3H2O;

1.6 mol of hydrogen will reduce 0.5333 mol of iron oxide.

Let’s calculate its mass.

M Fe2O3 = 56 x 2 + 16 x 3 = 160 grams / mol;

m Fe2O3 = 0.5333 x 160 = 85.33 grams;