Question

# An organic compound contains $$69$$% carbon and $$4.8$$% hydrogen, the remainder being oxygen. Calculate the masses of carbon dioxide and water produced when $$0.20$$ g of this substance is subjected to complete combustion.

Solution

## 100 g of organic compound contains 69 g of C, 4.8 g of hydrogen and 26.2 g of oxygen. 0.2 g of organic compound will contain $$\displaystyle \frac {69 \times 0.2}{100} = 0.138$$ g of C.12 g of C is present in 44 g of $$\displaystyle CO_2$$. 0.138 g of carbon will be present in $$\displaystyle \frac {44 \times 0.138}{12} =0.506$$  g of $$\displaystyle CO_2$$. 0.2 g of organic compound will contain $$\displaystyle \frac {4.8 \times 0.2}{100} = 0.0096$$g of hydrogen.18 g of water contains 2 g of hydrogen.Hence, $$0.0096$$ g of hydrogen will be present in $$\displaystyle \frac {18 \times 0.0096}{2} = 0.0864$$ g of waterThus, complete combustion of $$0.20$$ g of organic compound will produce $$0.506$$ g of carbon dioxide and $$0.0864$$ g of water. ChemistryNCERTStandard XI

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