(C) The total number of moles $n$ in the container is the sum of the moles of each gas: $n = 2 + 5 + 3 = 10 \ moles$.The temperature $T$ in Kelvin is

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(C) The total number of moles $n$ in the container is the sum of the moles of each gas: $n = 2 + 5 + 3 = 10 \ moles$.The temperature $T$ in Kelvin is $T = 0 \ ^{\circ}C + 273.15 = 273.15 \ K$. For simplicity,we use $T = 273 \ K$.The volume $V$ is $16.62 \ m^3$.Using the ideal gas equation $PV = nRT$,we can solve for pressure $P$:$P = \frac{nRT}{V}$$P = \frac{10 \times 8.31 \times 273}{16.62}$$P = \frac{83.1 \times 273}{16.62}$$P = 5 \times 273 = 1365 \ Pa$.Thus,the pressure in the container is $1365 \ Pa$.

Class 11 Physics Kinetic Theory of Gases Mixture of Gases

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In a container of volume $16.62 \ m^3$ at $0 \ ^{\circ}C$ temperature,$2 \ moles$ of oxygen,$5 \ moles$ of nitrogen,and $3 \ moles$ of hydrogen are present. Then,the pressure in the container is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $Pa$)

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$1570$
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$1270$
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$1365$
D
$2270$

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Kinetic Theory of Gases

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Mixture of Gases

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One mole of monatomic gas and three moles of diatomic gas are put together in a container. The molar specific heat (in $J K^{-1} mol^{-1}$) at constant volume is (Let $R=8 \, J K^{-1} mol^{-1}$).

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$A$ gas mixture consists of $2.0$ moles of oxygen and $4.0$ moles of neon at temperature $T$. Neglecting all vibrational modes, calculate the total internal energy of the system. (Oxygen has two rotational modes.) (in $RT$)

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$A$ cylindrical container of volume $4.0 \times 10^{-3} \, m^3$ contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is $400 \, K$. The pressure of the mixture of gases is:
[Take gas constant as $R = 8.3 \, J \, mol^{-1} \, K^{-1}$]

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In a container of volume $16.62 \ m^3$ at $0 \ ^{\circ}C$ temperature,$2 \ moles$ of oxygen,$5 \ moles$ of nitrogen,and $3 \ moles$ of hydrogen are present. Then,the pressure in the container is (Universal gas constant $R = 8.31 \ J \ mol^{-1} \ K^{-1}$) (in $Pa$)

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The ratio $C_P / C_V$ for a gas mixture consisting of $8 \ g$ of helium and $16 \ g$ of oxygen is

$A$ container holds $8 \, g$ of $O_2$ and $7 \, g$ of $N_2$ at a pressure of $10 \, atm$. If $O_2$ is removed,the pressure becomes ... $atm$.

One mole of monatomic gas and three moles of diatomic gas are put together in a container. The molar specific heat (in $J K^{-1} mol^{-1}$) at constant volume is (Let $R=8 \, J K^{-1} mol^{-1}$).

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$A$ cylindrical container of volume $4.0 \times 10^{-3} \, m^3$ contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is $400 \, K$. The pressure of the mixture of gases is:[Take gas constant as $R = 8.3 \, J \, mol^{-1} \, K^{-1}$]

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$A$ cylindrical container of volume $4.0 \times 10^{-3} \, m^3$ contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is $400 \, K$. The pressure of the mixture of gases is:
[Take gas constant as $R = 8.3 \, J \, mol^{-1} \, K^{-1}$]