(C) The total pressure $P$ of a mixture of ideal gases is given by the ideal gas equation $PV = n_{total} RT$,where $n_{total} = n_1 + n_2 + n_3$.Firs

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(C) The total pressure $P$ of a mixture of ideal gases is given by the ideal gas equation $PV = n_{total} RT$,where $n_{total} = n_1 + n_2 + n_3$.First,calculate the number of moles for each gas:$n_{O_2} = \frac{16 \, g}{32 \, g/mol} = 0.5 \, mol$$n_{N_2} = \frac{28 \, g}{28 \, g/mol} = 1.0 \, mol$$n_{CO_2} = \frac{44 \, g}{44 \, g/mol} = 1.0 \, mol$Total moles $n_{total} = 0.5 + 1.0 + 1.0 = 2.5 \, mol = \frac{5}{2} \, mol$.Substituting into the ideal gas equation:$PV = (2.5) RT$$P = \frac{5}{2} \frac{RT}{V}$.

Class 11 Physics Kinetic Theory Mixture of Gases

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The volume $V$ of an enclosure contains a mixture of three gases: $16 \, g$ of oxygen,$28 \, g$ of nitrogen,and $44 \, g$ of carbon dioxide at absolute temperature $T$. Consider $R$ as the universal gas constant. The pressure of the mixture of gases is:

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A
$\frac{88 RT}{V}$
B
$\frac{3 RT}{V}$
C
$\frac{5}{2} \frac{RT}{V}$
D
$\frac{4 RT}{V}$

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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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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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The pressure of a mixture of $64 \ g$ of oxygen, $28 \ g$ of nitrogen, and $132 \ g$ of carbon dioxide gases in a closed vessel is $P$. Under isothermal conditions, if the entire oxygen is removed from the vessel, the pressure of the mixture of the remaining two gases is:

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$A$ mixture of $28 \ g$ of nitrogen,$4 \ g$ of hydrogen,and $8 \ g$ of helium is kept in a vessel at a temperature of $400 \ K$ and a pressure of $8.3 \times 10^5 \ Pa$. What is the density of the mixture?

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The volume $V$ of an enclosure contains a mixture of three gases: $16 \, g$ of oxygen,$28 \, g$ of nitrogen,and $44 \, g$ of carbon dioxide at absolute temperature $T$. Consider $R$ as the universal gas constant. The pressure of the mixture of gases is:

Similar Questions

If $2 \text{ mole}$ of an ideal monoatomic gas at temperature $T$ is mixed with $6 \text{ mole}$ of another ideal monoatomic gas at temperature $2T$, then the temperature of the mixture is:

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

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?

The pressure of a mixture of $64 \ g$ of oxygen, $28 \ g$ of nitrogen, and $132 \ g$ of carbon dioxide gases in a closed vessel is $P$. Under isothermal conditions, if the entire oxygen is removed from the vessel, the pressure of the mixture of the remaining two gases is:

$A$ mixture of $28 \ g$ of nitrogen,$4 \ g$ of hydrogen,and $8 \ g$ of helium is kept in a vessel at a temperature of $400 \ K$ and a pressure of $8.3 \times 10^5 \ Pa$. What is the density of the mixture?

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