question_answer 1)

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.

Answer:

Calculation of mass of \[C{{O}_{2}}\] produced: Mass of the compound = 0.20 g We know that, \[%\,of\,C=\frac{12}{44}\times \frac{Mass\,of\,C{{O}_{2}}\,formed}{Mass\,of\,the\,compound}\times 100\] \[69=\frac{12}{44}\times \frac{Mass\,of\,C{{O}_{2}}\,formed}{0.2}\times 100\] or mass of \[C{{O}_{2}}\] formed = \[\frac{69\times 44\times 0.2}{12\times 100}=0.56g\] Similarly, \[%\,of\,H=\frac{2}{18}\times \frac{Mass\,of\,{{H}_{2}}O\,formed}{Mass\,of\,the\,compound}\times 100\] \[4.8=\frac{2}{18}\times \frac{Mass\,of\,{{H}_{2}}O\,formed}{0.2}\times 100\] or mass of \[{{H}_{2}}O\] formed = \[=\frac{4.8\times 18\times 0.2}{2\times 100}=0.0864g\]