What volume of carbon dioxide will be released if 1260 g of a 30% solution

What volume of carbon dioxide will be released if 1260 g of a 30% solution of nitric acid are added to 250 g of limestone containing 20% impurities, if the yield of carbon dioxide is 75% of the theoretically possible

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

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

Let’s determine the chemical amount of calcium carbonate. To do this, divide its weight by its molar weight.

M CaCO3 = 40 + 12 + 16 x 3 = 100 grams / mol; N CaCO3 = 250 x 0.8 / 100 = 2 mol;

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

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

2 moles of calcium carbonate will react with 4 moles of nitric acid. This will release 2 moles of carbon dioxide.

Let’s calculate its volume.

To do this, multiply the amount of substance by the volume of 1 mole of gas (filling 22.4 liters).

V CO2 = 2 x 22.4 = 44.8 liters;