Determine the mass of zinc and sulfate acid solution (p = 1.14 g / ml n = 20%)

Determine the mass of zinc and sulfate acid solution (p = 1.14 g / ml n = 20%), which were used to extract hydrogen required for the reduction of Fe3O4 weighing 104.4 g.

Determine the required amount of hydrogen for reduction.

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

Fe2O3 + 3 H2 = 2Fe + 3H2O;

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

N Fe2O3 = 104.4 / 160 = 0.6525 mol;

To restore this amount of oxide, 0.6525 x 3 = 1.9575 mol of hydrogen is needed.

Metallic zinc rapidly “dissolves” in sulfate acid, the reaction is described by the following chemical equation:

Zn + H2SO4 = ZnSO4 + H2;

You need to take the same amount of sulfuric acid.

Let’s calculate the weight of sulfuric acid.

M H2SO4 = 2 + 32 + 16 x 4 = 98 grams / mol;

m H2SO4 = 1.9575 x 98 = 191.835 grams;

The volume of the acid solution will be:

V of H2SO4 solution = 191.835 / 0.2 / 1.14 = 841 ml;

You need to take the same amount of zinc.

Let’s calculate the weight of zinc.

M Zn = 65 grams / mol;

m Zn = 1.9575 x 65 = 127.24 grams;