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A vessel of volume , V = 5.0 litre conta...

A vessel of volume , `V = 5.0` litre contains `1.4 g` of nitrogen at a temperature `T = 1800 K`. Find the pressure of the gas if `30%` of its molecules are dissociated into atoms at this temperature.

A

`0.54xx10^(5)N//m^(2)`

B

`1,94xx10^(5) N//m^(2)`

C

`2.62xx10^(5)N//m^(2)`

D

`3.75xx10^(5)N//m^(2)`

Text Solution

Verified by Experts

The correct Answer is:
B
`P=(mu)/(M)(RT)/(V), (P_(1))/(P_(2))-(mu_(2))/(mu_(1))+mu_(2)`
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Knowledge Check

  • A vessel of volume 5 litre contains 1.4 g of nitrogen at a temperature 1800K. The pressure of the gas is 30% of its molecules are dissociated into atoms at this temperature is:

    A
    4.05 atm
    B
    2.025atm
    C
    3.84atm
    D
    1.92atm

  • At constant temperature on increasing the pressure of a gas by 5% will decrease its volume by -

    A
    `5%`
    B
    `5.26%`
    C
    `4.26%`
    D
    `4.76%`

  • A vessel of volume 5000 cm^(3) contains ((1)/(20)) moles of molecular nitrogen at 1800 K. If 30% of the molecules are now dissociated the pressure inside the vessel (in Pa) will be

    A
    `1.49 xx 10^(5)`
    B
    `1.94 xx 10^(5)`
    C
    `2.25 xx 10^(5)`
    D
    `3.78 xx 10^(5)`