What mass of aluminum shavings containing 97% by mass of metal can be dissolved in 730 g of hydrochloric

What mass of aluminum shavings containing 97% by mass of metal can be dissolved in 730 g of hydrochloric acid with a mass fraction of hydrogen chloride of 15%? calculate the amount of gas evolved.

Aluminum enters into an active reaction with hydrochloric acid. In this case, an aluminum chloride salt can be obtained and hydrogen gas bubbles are released. The reaction is described by the following equation.

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

Let’s calculate the chemical amount of hydrochloric acid. For this purpose, we divide its weight by the molar weight of the acid.

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

N HCl = 730 x 0.15 / 36.5 = 3 mol;

The chemical amount of released hydrogen will be 2 times less: 3/2 = 1.5 mol

Let’s define its volume.

To do this, 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 = 1.5 x 22.4 = 33.6 liters;

With this amount of acid, 3/3 = 1 mol of aluminum will react.

Let’s find its weight:

M Al = 27 grams / mol;

m Al = 27 x 1 = 27 grams;