| A mixture of \[{{N}_{2}}\] and Ar gases in a cylinder contains 7 g of \[{{N}_{2}}\] and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of \[{{N}_{2}}\] is: |
| [Use atomic masses \[(in\text{ }g\text{ }mo{{l}^{1}}):N=14,\,\,Ar=40]\] [NEET 2020] |
A) 12 bar
B) 15 bar
C) 18 bar
D) 9 bar
Correct Answer: B
Solution :
| [b] \[{{n}_{{{N}_{2}}}}=\frac{7}{28}=\frac{1}{4}=0.25\] |
| \[{{n}_{Ar}}=\frac{8}{40}=\frac{1}{5}=0.20\] |
| Now, Applying Daltons law of partial pressure, |
| \[{{p}_{{{N}_{2}}}}=\left( {{x}_{{{N}_{2}}}} \right){{P}_{Total}}\] |
| \[=\frac{0.25}{0.45}\times 27\,\,bar\] |
| \[=\frac{5}{9}\times 27=15\,\,bar\] |
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