How much carbon dioxide is released during the interaction of 1260 kg. 30% nitric acid solution with 250 kg of limestone?

When calcium carbonate interacts with nitric acid, calcium nitrate, water is synthesized and gaseous carbon dioxide is released. The reaction proceeds according to the following chemical equation:

CaCO3 + 2HNO3 = Ca (NO3) 2 + CO2 ↑ + H2O;

Let’s calculate the chemical amount of calcium carbonate. For this purpose, we divide its weight by its molar mass.

M CaCO3 = 40 + 12 + 16 x 3 = 100 grams / mol; N CaCO3 = 250,000 / 100 = 2,500 mol;

Let’s calculate the molar amount of nitric acid. To do this, divide its weight by its molar weight.

M HNO3 = 1 + 14 + 16 x 3 = 63 grams / mol; N HNO3 = 1,260,000 x 0.3 / 63 = 6,000 mol;

2,500 moles of calcium carbonate react with 5,000 moles of nitric acid. This will release 2,500 moles of carbon dioxide.

Let’s find its volume.

For this purpose, we multiply the amount of the substance by the volume of 1 mole of gas (which is 22.4 liters).

V CO2 = 2,500 x 22.4 = 56,000 liters = 56 m3;