(B) $C_p = C_v + R$$\therefore C_p$ for hydrogen,$C_{p_1} = \frac{5}{2} R + R = \frac{7}{2} R$$C_p$ for helium,$C_{p_2} = \frac{3}{2} R + R = \frac{5}

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(B) $C_p = C_v + R$$\therefore C_p$ for hydrogen,$C_{p_1} = \frac{5}{2} R + R = \frac{7}{2} R$$C_p$ for helium,$C_{p_2} = \frac{3}{2} R + R = \frac{5}{2} R$$C_p$ for water vapour,$C_{p_3} = 3 R + R = 4 R$Given: $n_1 = 4, n_2 = 2, n_3 = 1$$C_p \text{ of mixture} = \frac{n_1 C_{p_1} + n_2 C_{p_2} + n_3 C_{p_3}}{n_1 + n_2 + n_3}$$= \frac{4 \times \frac{7}{2} R + 2 \times \frac{5}{2} R + 1 \times 4 R}{4 + 2 + 1}$$= \frac{14 R + 5 R + 4 R}{7} = \frac{23 R}{7}$

Class 11 Physics Kinetic Theory Mixture of Gases

Medium

Four moles of hydrogen,two moles of helium and one mole of water vapour form an ideal gas mixture. $[C_v$ for hydrogen $= \frac{5}{2} R, C_v$ for helium $= \frac{3}{2} R, C_v$ for water vapour $= 3 R]$. What is the molar specific heat at constant pressure of the mixture?

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A
$\frac{11}{3} R$
B
$\frac{23}{7} R$
C
$\frac{16}{7} R$
D
$\frac{23}{3} R$

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In a cubic container of inner side length $10 \ cm$, nitrogen gas at $100 \ kPa$ pressure is maintained at $300 \ K$. If the pressure inside the container is increased to $300 \ kPa$ by adding oxygen gas, the ratio of the number of $N_2$ molecules to $O_2$ molecules in the container is:

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$1 \, \text{mole}$ of a gas having $\gamma = \frac{7}{5}$ is mixed with $1 \, \text{mole}$ of a gas having $\gamma = \frac{4}{3}$. What will be the $\gamma$ for the mixture?

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$14 \, g$ of $CO$ at $27^{\circ} C$ is mixed with $16 \, g$ of $O_2$ at $47^{\circ} C$. The temperature of the mixture is .......... $^{\circ} C$ (vibration mode neglected).

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$A$ mixture of two non-reactive ideal gases is enclosed in a vessel consisting of one mole of a monatomic gas '$A$' and 'n' moles of a diatomic gas '$B$' at a temperature '$T$'. If the adiabatic constant of the gaseous mixture is $\frac{13}{9}$,then the value of 'n' is:

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One litre of oxygen at a pressure of $1 \,atm$ and two litres of nitrogen at a pressure of $0.5 \,atm$ are introduced into a vessel of volume $1 \,L$. If there is no change in temperature, the final pressure of the mixture of gas (in $atm$) is

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Four moles of hydrogen,two moles of helium and one mole of water vapour form an ideal gas mixture. $[C_v$ for hydrogen $= \frac{5}{2} R, C_v$ for helium $= \frac{3}{2} R, C_v$ for water vapour $= 3 R]$. What is the molar specific heat at constant pressure of the mixture?

Similar Questions

In a cubic container of inner side length $10 \ cm$, nitrogen gas at $100 \ kPa$ pressure is maintained at $300 \ K$. If the pressure inside the container is increased to $300 \ kPa$ by adding oxygen gas, the ratio of the number of $N_2$ molecules to $O_2$ molecules in the container is:

$1 \, \text{mole}$ of a gas having $\gamma = \frac{7}{5}$ is mixed with $1 \, \text{mole}$ of a gas having $\gamma = \frac{4}{3}$. What will be the $\gamma$ for the mixture?

$14 \, g$ of $CO$ at $27^{\circ} C$ is mixed with $16 \, g$ of $O_2$ at $47^{\circ} C$. The temperature of the mixture is .......... $^{\circ} C$ (vibration mode neglected).

$A$ mixture of two non-reactive ideal gases is enclosed in a vessel consisting of one mole of a monatomic gas '$A$' and 'n' moles of a diatomic gas '$B$' at a temperature '$T$'. If the adiabatic constant of the gaseous mixture is $\frac{13}{9}$,then the value of 'n' is:

One litre of oxygen at a pressure of $1 \,atm$ and two litres of nitrogen at a pressure of $0.5 \,atm$ are introduced into a vessel of volume $1 \,L$. If there is no change in temperature, the final pressure of the mixture of gas (in $atm$) is

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