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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 water
Thus, complete combustion of $$0.20$$ g of organic compound will produce $$0.506$$ g of carbon dioxide and $$0.0864$$ g of water.

Chemistry
NCERT
Standard XI

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