In an excess of hydrochloric acid, 2.11 g of ore containing 71% iron (II) carbonate was dissolved. Determine the amount of carbon

In an excess of hydrochloric acid, 2.11 g of ore containing 71% iron (II) carbonate was dissolved. Determine the amount of carbon dioxide released during this.

1) Let’s compose the reaction equation:
FeCO3 + 2HCl = FeCl2 + H2O + CO2 ↑
2) Determine the mass of pure iron carbonate and its amount of substance:
m (FeCO3) = (m (ore) ∙ ω) / 100% = (2.11 ∙ 71) / 100 = 1.50 g.
n (FeCO3) = m (FeCO3) / M (FeCO3) = 1.50 / 116 = 0.013 mol.
3) Let’s calculate the amount of the substance of the released carbon dioxide and its volume:
according to the reaction equation
n (CO2) = n (FeCO3) = 0.013 mol;
V (CO2) = n (CO2) ∙ Vm = 0.013 ∙ 22.4 = 0.29 l.
Answer: 0.29 L