(C) Given:Volume $V = 4.0 \times 10^{-3} \, m^3$Total number of moles $n = 1 \, mol \, (H_2) + 2 \, mol \, (CO_2) = 3 \, mol$Temperature $T = 400 \, K

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(C) Given:Volume $V = 4.0 \times 10^{-3} \, m^3$Total number of moles $n = 1 \, mol \, (H_2) + 2 \, mol \, (CO_2) = 3 \, mol$Temperature $T = 400 \, K$Gas constant $R = 8.3 \, J \, mol^{-1} \, K^{-1}$Using the ideal gas equation $PV = nRT$,we can find the pressure $P$:$P = \frac{nRT}{V}$Substituting the values:$P = \frac{3 \times 8.3 \times 400}{4.0 \times 10^{-3}}$$P = \frac{9960}{4.0 \times 10^{-3}}$$P = 2490 \times 10^3 \, Pa = 24.9 \times 10^5 \, Pa$Therefore,the correct option is $C$.

Class 11 Physics Kinetic Theory Mixture of Gases

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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
$249 \times 10^1 \, Pa$
B
$24.9 \times 10^3 \, Pa$
C
$24.9 \times 10^5 \, Pa$
D
$24.9 \, Pa$

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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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Five moles of helium are mixed with two moles of hydrogen to form a mixture. Take molar mass of helium $M_1 = 4 \ g/mol$ and that of hydrogen $M_2 = 2 \ g/mol$. The equivalent molar mass of the mixture is:

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One gram mole of an ideal gas $A$ with the ratio of constant pressure and constant volume specific heats $\gamma_{A} = 5/3$ is mixed with $n$ gram moles of another ideal gas $B$ with $\gamma_{B} = 7/5$. If the $\gamma$ for the mixture is $19/13$,then what will be the value of $n$?

The capacity of a vessel is $3 \, L$. It contains a mixture of $6 \, g$ oxygen,$8 \, g$ nitrogen,and $5 \, g$ $CO_2$ at $27^{\circ}C$. If $R = 8.31 \, J/(mol \cdot K)$,then the pressure in the vessel in $N/m^2$ will be (approx.)

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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 $R = 8.3 \, J \, mol^{-1} \, K^{-1}$]