Limestone with a mass of 100 g, containing 84% calcium carbonate CaCO3, interacts with the required
Limestone with a mass of 100 g, containing 84% calcium carbonate CaCO3, interacts with the required amount of hydrochloric acid HCl. Calculate the mass of the resulting carbon monoxide (IV).
1. Let’s compose the equation of the proceeding reaction:
CaCO3 + 2HCl = CaCl2 + H2O + CO2 ↑;
2. Determine the mass of calcium carbonate contained in limestone:
m (CaCO3) = w (CaCO3) * m (limestone) = 0.84 * 100 = 84 g;
3. Find the chemical amount of calcium carbonate:
n (CaCO3) = m (CaCO3): M (CaCO3);
M (CaCO3) = 40 + 12 + 3 * 16 = 100 g / mol;
n (CaCO3) = 84: 100 = 0.84 mol;
4. Set the amount of carbon dioxide released:
n (CO2) = n (CaCO3) = 0.84 mol;
5. Calculate the mass of carbon monoxide:
m (CO2) = n (CO2) * M (CO2);
M (CO2) = 12 + 2 * 16 = 44 g / mol;
m (CO2) = 0.84 * 44 = 36.96 g.
Answer: 36.96 g.