Calculate the mass of CO2 that can be obtained by the interaction of calcium carbonate weighing 3.5 g

Calculate the mass of CO2 that can be obtained by the interaction of calcium carbonate weighing 3.5 g with a solution of hydrochloric acid weighing 15 g with a mass fraction of 20%

The reaction of dissolving limestone in hydrochloric acid is described by the following chemical reaction equation:

CaCO3 + 2HCl = CaCl2 + CO2 + H2O;

When 1 mol of limestone is dissolved in acid, 1 mol of gaseous carbon dioxide is synthesized. This consumes 2 mol of hydrochloric acid.

Let’s calculate the available chemical amount of hydrochloric acid substance.

M HCl = 1 + 35.5 = 36.5 grams / mol;

N HCl = 15 x 0.2 / 36.5 = 0.082 mol;

Let’s calculate the available chemical amount of calcium carbonate substance.

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

N CaCO3 = 3.5 / 100 = 0.035 mol;

Thus, when 0.035 mol of limestone is dissolved, 0.035 mol of carbon dioxide is synthesized. This will require 0.07 mol of acid.

Let’s calculate the weight of carbon dioxide.

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

m CO2 = 0.035 x 44 = 1.54 grams;