What mass of carbon dioxide is formed when 200 g of limestone interacts with the required amount of nitric acid?

What mass of carbon dioxide is formed when 200 g of limestone interacts with the required amount of nitric acid? Calculate the number of carbon dioxide particles formed.

When calcium carbonate reacts with nitric acid, calcium nitrate, water and carbon dioxide gas are produced. The reaction is described by the following 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 mass.

M CaCO3 = 40 + 12 + 16 x 3 = 100 grams / mol; N CaCO3 = 200/100 = 2 mol;

When this amount of limestone is dissolved in nitric acid, an equivalent amount of carbon dioxide will be obtained.

Let’s calculate its weight. For this purpose, we multiply the amount of a substance by its molar weight.

M CO2 = 12 + 16 x 2 = 44 grams / mol; m CO2 = 2 x 44 = 88 grams;

In order to find the number of carbon dioxide molecules, it is necessary to multiply the amount of the substance by the number of molecules in one mole of the substance (6.022 x 10 ^ 23).

N CO2 = 2 x 6.0 ^ 22 x 10 ^ 23 = 1.2044 x 10 ^ 24 molecules;