What volume of gas will be released when 21 g of magnesium carbonate is dissolved in an excess of sulfuric acid?

The reaction of dissolving magnesium carbonate in sulfuric acid is described by the following chemical reaction equation:

MgCO3 + H2SO4 = MgSO4 + CO2 + H2O;

When 1 mol of magnesium carbonate is dissolved in acid, 1 mol of gaseous carbon dioxide is synthesized. This consumes 1 mol of sulfuric acid.

Let’s calculate the available chemical amount of magnesium carbonate.

M MgCO3 = 24 + 12 + 16 x 3 = 84 grams / mol;

N MgCO3 = 21/84 = 0.25 mol;

Thus, upon dissolution of 0.25 mol of salt, 0.25 mol of carbon dioxide is synthesized.

This will consume 0.25 mol of acid.

Let’s calculate its volume. To do this, multiply the amount of the substance and the standard volume of 1 mole of the gaseous substance.

1 mole of ideal gas fills a volume of 22.4 liters under normal conditions.

V CO2 = 0.25 x 22.4 = 5.6 liters;