In hydrochloric acid (HCl) was dissolved 270 grams of aluminum containing 10% impurities.

In hydrochloric acid (HCl) was dissolved 270 grams of aluminum containing 10% impurities. What volume of hydrogen was obtained in this case, if its yield from the theoretically possible was 75%? How many grams of 20% HCl was required for the reaction?

Aluminum enters into an active reaction with hydrochloric acid. In this case, an aluminum chloride salt is formed and elemental hydrogen is released. The reaction is described by the following chemical equation.

Al + 3HCl = AlCl3 + 3/2 H2;

Let’s calculate the chemical amount of aluminum. To do this, we divide its weight by the molar weight of the substance.

M Al = 27 grams / mol;

N Al = 270 x 0.9 / 27 = 9 mol;

Taking into account the reaction yield of 75%, the chemical amount of released hydrogen will be: 9 x 3/2 x 0.75 = 10.125 mol

Let’s define its volume.

For this purpose, we multiply the chemical amount of the substance by the volume of 1 mole of gas (filling a space with a volume of 22.4 liters).

V H2 = 10.125 x 22.4 = 226.8 liters;

9 mol of aluminum reacts with 9 x 3 = 27 mol of hydrochloric acid.

Let’s find its weight.

M HCl = 1 + 35.5 = 36.5 grams / mol;

m HCl = 27 x 36.5 = 985.5 grams;