As a result of the reaction of aluminum with sulfuric acid, 26.88 liters of hydrogen were released.

As a result of the reaction of aluminum with sulfuric acid, 26.88 liters of hydrogen were released. Determine the mass of reacted aluminum.

Metallic aluminum interacts with sulfuric acid. In this case, aluminum sulfate can be obtained and bubbles of hydrogen gas are released. The reaction is described by the following equation.

2Al + 3H2SO4 = Al2 (SO4) 3 + 3 H2;

Let’s find the chemical amount of synthesized hydrogen gas. To do this, we find the ratio of its volume to the volume of 1 mole of gas (filling a space with a volume of 22.4 liters).

N H2 = 26.88 / 22.4 = 1.2 mol;

To synthesize such an amount of gaseous hydrogen, you need to take 1.2 x 2/3 = 0.8 mol of metallic aluminum.

Let’s calculate its weight.

For this purpose, we multiply the amount of the substance by the weight of 1 mole of this chemical element.

M Al = 27 grams / mol;

m Al = 0.8 x 27 = 21.6 grams;