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A mixture of N2 and Ar gases in a cylind...

A mixture of `N_2` and Ar gases in a cylinder contains 7g of `N_2` & 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27bar, the partial pressure of `N_2` is:

A

12 bar

B

15 bar

C

18 bar

D

9 bar

Text Solution

Verified by Experts

The correct Answer is:
B
The number of moles of `N_2` and Ar are :
`n_(N_2) = ("given mass")/("Molar mass")`
`= (7g)/(28 g)`
`= 0.25 mol`
`M_(Ar)= 8/40`
`= 0.20 mol`
Now, Applying Dalton.s law of partial pressure
Partial pressure of `N_2` = (mole fractin of `N_2`) `xx` Total pressure
`P_(N_2) = ((0.25)/((0.20 + 0.25))) xx 27` bar
`= (0.25)/(0.45) xx 27` bar
`P_(N_2) = 15 ` bar
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Knowledge Check

  • A mixture of N_2 and Ar gases in cylinder contains 7 g of N_2 and 8g 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]

    A
    12 bar
    B
    15 bar
    C
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    D
    9 bar

  • 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]

    A
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    B
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    C
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