Determine the mass of barium carbonate, which reacted with an excess of hydrochloric acid
Determine the mass of barium carbonate, which reacted with an excess of hydrochloric acid, if 20 liters of carbon dioxide were released, and the product yield was 90%.
To solve the problem, we write down the equation of the process:
BaCO3 + 2HCl = BaCl2 + CO2 + H2O – ion exchange, carbon dioxide is released;
We make calculations:
M (BaCO3) = 197.3 g / mol;
M (CO2) = 44 g / mol.
Proportion:
1 mole of gas at normal level – 22.4 liters;
X mol (CO2) -20 L from here, X mol (CO2) = 1 * 20 / 22.4 = 0.89 mol.
Y (BaCO3) = 0.89 mol since the amount of substances is 1 mol.
We find the mass of the starting material, taking into account the product yield:
m (BaCO3) = Y * M = 0.89 * 197.3 = 175.6 g (theoretical weight);
W = m (practical) / m (theoretical) * 100;
m (BaCO3) = 0.90 * 175.6 = 158.04 g (practical weight).
Answer: you need barium carbonate weighing 158.04 g