(D) Given, $C_V = 12.6 \,J \,mol^{-1} \,K^{-1}$ and $R = 8.314 \,J \,mol^{-1} \,K^{-1}$.According to Mayer's relation for an ideal gas, the relationsh

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(D) Given, $C_V = 12.6 \,J \,mol^{-1} \,K^{-1}$ and $R = 8.314 \,J \,mol^{-1} \,K^{-1}$.According to Mayer's relation for an ideal gas, the relationship between molar specific heat at constant pressure $(C_p)$ and constant volume $(C_V)$ is given by $C_p - C_V = R$.Therefore, $C_p = C_V + R$.Substituting the given values, $C_p = 12.6 + 8.314 = 20.914 \,J \,mol^{-1} \,K^{-1}$.Rounding to one decimal place, we get $C_p \approx 20.9 \,J \,mol^{-1} \,K^{-1}$.

Class 11 Physics Kinetic Theory of Gases Molar Specific Heat of gas and relation between them (Mayer's formula)

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The specific heat of helium at constant volume is $12.6 \,J \,mol^{-1} \,K^{-1}$. The specific heat of helium at constant pressure in $J \,mol^{-1} \,K^{-1}$ is approximately (assume, the universal gas constant, $R=8.314 \,J \,mol^{-1} \,K^{-1}$)

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A
$12.6$
B
$16.8$
C
$18.9$
D
$20.9$

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Kinetic Theory of Gases

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Molar Specific Heat of gas and relation between them (Mayer's formula)

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The molar specific heat at constant volume,${C_V}$,for a monoatomic gas is:

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If $\Delta Q$ is the amount of heat supplied to $n$ moles of a diatomic gas at constant pressure,$\Delta U$ is the change in internal energy,and $\Delta W$ is the work done,then the ratio $\Delta W : \Delta U : \Delta Q$ is

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Can we use the degree of freedom to obtain the specific heat capacity of a gas? Explain.

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When heat $Q$ is supplied to a diatomic gas of rigid molecules at constant volume,its temperature increases by $\Delta T$. The heat required to produce the same change in temperature at constant pressure is:

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The specific heat of helium at constant volume is $12.6 \,J \,mol^{-1} \,K^{-1}$. The specific heat of helium at constant pressure in $J \,mol^{-1} \,K^{-1}$ is approximately (assume, the universal gas constant, $R=8.314 \,J \,mol^{-1} \,K^{-1}$)

Similar Questions

The molar specific heat at constant volume,${C_V}$,for a monoatomic gas is:

The heat energy that must be supplied to $14 \ g$ of nitrogen at room temperature to raise its temperature by $48^{\circ} C$ at constant pressure is (Molecular weight of nitrogen $= 28, R =$ gas constant,$C_p = \frac{7}{2} R$ for diatomic gas). (in $R$)

If $\Delta Q$ is the amount of heat supplied to $n$ moles of a diatomic gas at constant pressure,$\Delta U$ is the change in internal energy,and $\Delta W$ is the work done,then the ratio $\Delta W : \Delta U : \Delta Q$ is

Can we use the degree of freedom to obtain the specific heat capacity of a gas? Explain.

When heat $Q$ is supplied to a diatomic gas of rigid molecules at constant volume,its temperature increases by $\Delta T$. The heat required to produce the same change in temperature at constant pressure is:

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