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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 g mol-1)  N=14, Ar=40 ]

 

Option: 1

18 bar


Option: 2

9 bar


Option: 3

12 bar

 


Option: 4

15 bar


Answers (1)

best_answer

Moles of N_{2}=\frac{7g}{28g/mol}= 0.25mol

Moles of Ar=\frac{8g}{40g/mol}= 0.2mol

Mole fraction of N_{2} is \frac{0.25}{0.45}=\frac{5}{9}

From Dalton's law of partial pressure,

Therefore, Pressure exerted by  is N_{2} is \frac{5}{9} \times 27bar=15bar

Therefore, Option(4) is correct.

Posted by

shivangi.bhatnagar

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