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Question

When 0.177 g of a sample containing organic substance is burned with oxygen gas, the carbondioxide realised is held in the solution of barium hydroxide. 0.5613 g of barium carbonate is formed. Calculate the percentage of carbon in the sample.

Ba(OH)2 + CO2 => BaCO3(s) + H2O

Please write the solution with full steps

Answer 1

Ba(OH)₂ + CO₂ => BaCO₃(s) + H₂O ... balanced equation for collecting CO₂ in Ba(OH)₂

The combustion of the organic substance produces CO2 from the carbon atoms of the substance. Find the moles of CO2 and that will tell you the moles of C.

0.5613g BaCO₃ x 1 mol BaCO_3/197.3 g x 1 mol CO₂/mol BaCO₃ = 0.002845 moles CO₂ = 0.002845moles C

Now to find % C, we convert moles C to grams C:

0.002845 mol C x 12 g C/mol = 0.03414 g C

% C in original sample = 0.002845 g C/0.177 g sample (x100%) = 1.61% C