In a solution of diluted sulfuric acid weighing 1000 g, zinc with a weight of 13 g was lowered.

In a solution of diluted sulfuric acid weighing 1000 g, zinc with a weight of 13 g was lowered. In this case, all the zinc was dissolved. Determine the mass of the solution by the end of the chemical reaction and the mass fraction of zinc sulfate in the resulting solution.

The reaction between zinc and sulfuric acid is described by the following chemical reaction equation.

Zn + H2SO4 = ZnSO4 + H2;

1 mole of metal reacts with 1 mole of acid. In this case, 1 mol of salt is synthesized and 1 mol of gaseous hydrogen is released.

Let’s calculate the chemical amount of a substance in 13 grams of zinc.

M Zn = 65 grams / mol;

N Zn = 13/65 = 0.2 mol;

The same chemical amount of hydrogen will be obtained.

Let’s calculate its mass.

M H2 = 2 grams / mol;

m H2 = 0.2 x 2 = 0.4 grams;

The weight of the solution after the end of the reaction will increase by the weight of zinc and decrease by the weight of hydrogen and will be 1000 + 13 – 0.4 = 1012.60 grams.

The weight of zinc sulfate will be:

M ZnSO4 = 65 + 32 + 16 x 4 = 161 grams / mol;

m ZnSO4 = 161 x 0.2 = 32.2 grams;