Partial pressures of components of a gaseous mixture are as given below. | ||||||||||||
|
A) 2.5%
B) 0.025%
C) 2.3%
D) 0.23%
Correct Answer: A
Solution :
From gas laws. we have \[m=M\cdot \left( \frac{pV}{RT} \right)\] |
Mass of hydrogen gas present is \[{{m}_{H}}={{M}_{H\,}}{{p}_{H}}\left( \frac{V}{RT} \right)\] |
Percentage of mass of hydrogen is |
\[{{m}_{H}}=\frac{{{M}_{H}}{{p}_{H}}\left( \frac{V}{RT} \right)\times 100}{({{M}_{H}}{{p}_{H}}+{{M}_{C{{O}_{2}}}}{{p}_{C{{O}_{2}}}}+{{M}_{C{{H}_{4}}}}{{p}_{C{{H}_{4}}}})}\]\[+{{M}_{{{C}_{2}}{{H}_{6}}}}{{p}_{{{C}_{2}}{{H}_{6}}}})\left( \frac{V}{RT} \right)\] |
\[=\frac{2\times 200\times 100}{2\times 200+44+150+16\times 320+30\times 105}\] |
\[=0.026\times 100=2.6%\] |
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