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The molar heat capacity at constant pres...

The molar heat capacity at constant pressure of nitrogen gas at `STP` is nearly `3.5 R`. Now when the temperature is increased, it gradually increases and approaches `4.5 R`. The most approprite reason for this behaviour is that at high temperatures

A

nitrogen does not behave as an ideal gas

B

nitrogen molecules dissociate in atoms

C

the molecules collides more frequently

D

molecules vibration gradually beome effective

Text Solution

Verified by Experts

The correct Answer is:
D
`C_(P) = 3.5 R (At STP)`
As temperature increases, vibrational degree of freedom becomes `2` at high temperature.
`C_(P) = (9)/(2) R = 4.5 R`
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Knowledge Check

  • Molar heat capacity for a gas at constant temperature and pressure is

    A
    `3//2` R
    B
    `5//2` R
    C
    depends on atomicity of gas
    D
    infinity `(infty)`

  • The molar heat capacity of a gas at constant pressure is equal to [R equiv the universal molar gas constant, gamma equiv the adiabatic constant]

    A
    `gammaR`
    B
    `(gamma-1)R`
    C
    `(gamma)/(gamma-1)R`
    D
    `(gamma-1)/(gamma)R`

  • The molar heat capacity, C_(v) of helium gas is 3//2 R and is independent of temperature. For hydrogen gas, C_(v) approaches 3//2 R at a very low temperature, equals 5//2 R at moderate temperature and is higher than 5//2 R at high temperature. Choose the correct reason for the temperature dependence of C_(v) in case of hydrogen :

    A
    Hydrogen is diatomic so at high temperature rotational and vibrational motion also counts
    B
    Hydrogen is monoatomic so at high temperature rotational and vibrational motion also counts
    C
    Hydrogen is diatomic so at high temperature rotational and vibrational motion are not counted
    D
    can’t be defined

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