How many ml of 10% sulfuric acid solution (pl. = 1.07 g / ml) and how much zinc is required

How many ml of 10% sulfuric acid solution (pl. = 1.07 g / ml) and how much zinc is required to obtain 112 liters of hydrogen?

Sulfuric acid reacts with zinc in equimolar chemical quantities.

The process is described by the equation:

Zn + H2SO4 → ZnSO4 + H2;

Let’s determine the chemical amount of synthesized hydrogen.

N H2 = 112 / 22.4 = 5 mol;

To obtain such an amount of hydrogen, it is necessary to dissolve 5 mol of zinc in 5 mol of acid.

Let’s find their weights.

The zinc weight will be:

M Zn = 65 grams / mol;

m Zn = 5 x 65 = 325 grams;

The weight of sulfuric acid will be:

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

m H2SO4 = 5 x 98 = 490 grams;