JEE MAIN - Chemistry (2022 - 28th June Evening Shift - No. 19)
The complete combustion of 0.492 g of an organic compound containing 'C', 'H' and 'O' gives 0.793 g of CO2 and 0.442 g of H2O. The percentage of oxygen composition in the organic compound is ______________. (nearest integer)
Answer
46
Explanation
Total organic compound = 0.492 gm
Produced CO2 = 0.793 gm
$$\therefore$$ Moles of CO2 = $${{0.793} \over {44}}$$
$$\therefore$$ Moles of C atoms = $${{0.793} \over {44}}$$
$$\therefore$$ Weight of C atoms = $${{0.793} \over {44}}$$ $$\times$$ 12 = 0.216 g
Produced H2O = 0.442 gm
$$\therefore$$ Moles of H2O = $${{0.442} \over {18}}$$
$$\therefore$$ Moles of H atoms = $${{0.442} \over {18}}$$
$$\therefore$$ Weight of H atoms = $${{0.442} \over {18}}$$ $$\times$$ 2 = 0.05 g
$$\therefore$$ Weight of O atoms
= 0.492 $$-$$ (0.216 + 0.05)
= 0.226 gm
% by mass of oxygen in compound
= $${{0.226} \over {0.492}}$$ $$\times$$ 100 = 46%
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