JEE MAIN - Chemistry (2021 - 25th February Morning Shift - No. 10)
Complete combustion of 1.80 g of an oxygen containing compound (CxHyOz) gave 2.64 g of CO2 and 1.08 g of H2O. The percentage of oxygen in the organic compound is :
51.63
50.33
63.53
53.33
Explanation
CxHyOz + O2 $$ \to $$ xCO2 + $${y \over 2}{H_2}O$$
2.64 g of CO2 contains 0.72 g C.
1.08 g of H2O contains 0.12 g H.
$$ \therefore $$ Mass of oxygen present = 1.80 – (0.72 +0.12) = 0.96 g
% of O = $${{0.96} \over {1.80}} \times 100$$ = 53.33 %
2.64 g of CO2 contains 0.72 g C.
1.08 g of H2O contains 0.12 g H.
$$ \therefore $$ Mass of oxygen present = 1.80 – (0.72 +0.12) = 0.96 g
% of O = $${{0.96} \over {1.80}} \times 100$$ = 53.33 %
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