(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 of Gases 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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Kinetic Theory of Gases

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Mixture of Gases

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For a mixture of non-reactive gases,derive the equation for total pressure.

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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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$3\, \text{moles}$ of an ideal gas at a temperature of $27^{\circ}\, \text{C}$ are mixed with $2\, \text{moles}$ of an ideal gas at a temperature of $227^{\circ}\, \text{C}$. Determine the equilibrium temperature $(^{\circ}\, \text{C})$ of the mixture, assuming no loss of energy.

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$A$ mixture of ideal gases has $2$ moles of $He$,$4$ moles of oxygen $(O_2)$,and $1$ mole of ozone $(O_3)$ at absolute temperature $T$. The internal energy of the mixture is ............. $RT$.

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One mole of an ideal monoatomic gas $(\gamma = 5/3)$ is mixed with one mole of a diatomic gas $(\gamma = 7/5).$ What is $\gamma$ for the mixture? $\gamma$ denotes the ratio of specific heat at constant pressure to that at constant volume.

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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

For a mixture of non-reactive gases,derive the equation for total pressure.

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:

$3\, \text{moles}$ of an ideal gas at a temperature of $27^{\circ}\, \text{C}$ are mixed with $2\, \text{moles}$ of an ideal gas at a temperature of $227^{\circ}\, \text{C}$. Determine the equilibrium temperature $(^{\circ}\, \text{C})$ of the mixture, assuming no loss of energy.

$A$ mixture of ideal gases has $2$ moles of $He$,$4$ moles of oxygen $(O_2)$,and $1$ mole of ozone $(O_3)$ at absolute temperature $T$. The internal energy of the mixture is ............. $RT$.

One mole of an ideal monoatomic gas $(\gamma = 5/3)$ is mixed with one mole of a diatomic gas $(\gamma = 7/5).$ What is $\gamma$ for the mixture? $\gamma$ denotes the ratio of specific heat at constant pressure to that at constant volume.

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