Determine the mass of sulfuric acid reacted with 270 grams of aluminum. How much hydrogen will be released in this case?

The reaction of interaction of aluminum with sulfuric acid is described by the following chemical equation:

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

When 2 metal molecules dissolve, 3 hydrogen molecules are released.

Let’s calculate the chemical amount of a substance in 270 grams of metal.

M Al = 27 grams / mol;

N Al = 270/27 = 10 mol;

When dissolving such an amount, 10/2 x 3 = 15 mol of acid will be needed and 10/2 x 3 = 15 mol of hydrogen will be released.

Let’s calculate the mass of sulfuric acid:

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

m H2SO4 = 98 x 15 = 1 470 grams;

Let’s calculate the volume of hydrogen:

1 mole of ideal gas normally takes on a volume of 22.40 liters.

V H2 = 15 x 22.40 = 336 liters;