Carbon dioxide (Carbon (IV) oxide) obtained by burning 0.6 g of coal was passed through a solution of barium hydroxide Ba

Carbon dioxide (Carbon (IV) oxide) obtained by burning 0.6 g of coal was passed through a solution of barium hydroxide Ba (OH) 2 weighing 200 g. What is the mass of the precipitate formed if the mass fraction of Ba (OH) 2 is 3.42%?

Given:
m (C) = 0.6 g
m solution (Ba (OH) 2) = 200 g
ω (Ba (OH) 2) = 3.42%
To find:
m (draft) -?
Decision:
1) C + O2 => CO2;
CO2 + Ba (OH) 2 => BaCO3 ↓ + H2O;
2) n (C) = m (C) / M (C) = 0.6 / 12 = 0.05 mol;
3) m (Ba (OH) 2) = ω (Ba (OH) 2) * m solution (Ba (OH) 2) / 100% = 3.42% * 200/100% = 6.84 g;
4) n (Ba (OH) 2) = m (Ba (OH) 2) / M (Ba (OH) 2) = 6.84 / 171 = 0.04 mol;
5) n (BaCO3) = n (Ba (OH) 2) = 0.04 mol;
6) m (BaCO3) = n (BaCO3) * M (BaCO3) = 0.04 * 197 = 7.88 g.
Answer: The mass of BaCO3 is 7.88 g.