What volume of co2 and what mass of ca (oh) 2 can be obtained from 1 ton of limestone containing 10% impurities.

1. Let’s write down the reaction equations:

CaCO3 = CaO + CO2;

CaO + H2O = Ca (OH) 2;

2.Calculate the mass of pure calcium carbonate:

m (CaCO3) = m (limestone) – m (impurities);

m (impurities) = w (impurities) * m (limestone) = 0.1 * 1000 = 100 kg;

m (CaCO3) = 1000 – 100 = 900 kg;

3.Calculate the chemical amount of carbonate:

n (CaCO3) = m (CaCO3): M (CaCO3);

M (CaCO3) = 40 + 12 + 3 * 16 = 100 g / mol;

n (CaCO3) = 900: 100 = 9 kmol;

4.determine the amount of carbon dioxide and calcium hydroxide:

n (CO2) = n (CaCO3) = 9 kmol;

n (Ca (OH) 2) = n (CaO) = n (CaCO3) = 9 kmol;

5.find the volume of CO2:

V (CO2) = n (CO2) * Vm = 9 * 22.4 = 201.6 m ^ 3;

6.Calculate the mass of hydroxide:

m (Ca (OH) 2) = n (Ca (OH) 2) * M (Ca (OH) 2);

M (Ca (OH) 2) = 40 + 2 * 17 = 74 g / mol;

m (Ca (OH) 2) = 9 * 74 = 666 kg.

Answer: 201.6 m ^ 3; 666 kg.