Calculate the masses of sulfuric acid and zinc required to obtain 1 m³ of hydrogen

Calculate the masses of sulfuric acid and zinc required to obtain 1 m³ of hydrogen as a result of the substitution reaction.

Zinc metal reacts with sulfuric acid to release hydrogen gas and form zinc sulfate. The reaction is described by the following equation:

Zn + H2SO4 = ZnSO4 + H2;

1 mole of metal reacts with 1 mole of acid. This synthesizes 1 mol of salt and 1 mol of hydrogen.

Let’s calculate the amount of substance in 1000 liters of hydrogen.

To do this, we divide this volume by the volume of 1 mole of gas.

N H2 = 1000 / 22.4 = 44.643 mol;

Let’s calculate the masses of such an amount of sulfuric acid and zinc.

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

m H2SO4 = 44.643 x 98 = 4375 grams;

M Zn = 65 grams / mol;

m Zn = 44.643 x 65 = 2902 grams;