What mass of zinc must be dissolved in sulfuric acid to obtain hydrogen, which can be used to reduce copper (II)

What mass of zinc must be dissolved in sulfuric acid to obtain hydrogen, which can be used to reduce copper (II) oxide weighing 14.4 g? Note that hydrogen is needed for reduction in a twofold excess.

Let’s calculate the required amount of hydrogen. The reduction of copper is described by the reaction:

CuO + H2 = Cu + H2O;

Let’s calculate the molar amount of copper oxide:

M CuO = 64 + 16 = 80 grams / mol;

N CuO = 14.4 / 80 = 0.18 mol;

A twofold excess of hydrogen will be 0.18 x 2 = 0.36 mol;

Let’s calculate the required amount of zinc.

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

Zn + H2SO4 = ZnSO4 + H2;

To obtain 0.36 mol of hydrogen, it is necessary to dissolve 0.36 mol of zinc.

Let’s calculate its weight.

To do this, multiply the amount of the substance by the molar weight of the substance.

M Zn = 65 grams / mol;

m Zn = 65 x 0.36 = 23.4 grams;