(A) According to the ideal gas law,$PV = nRT$. Since $T$ and $V$ are constant for both gases,the number of moles $n$ is proportional to $P$. Initially

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(A) According to the ideal gas law,$PV = nRT$. Since $T$ and $V$ are constant for both gases,the number of moles $n$ is proportional to $P$. Initially,each gas has $n$ moles. After mixing,the total number of moles becomes $n + n = 2n$. Using the ideal gas equation for the mixture: $P_{new}V = (2n)RT$. Since $PV = nRT$,we have $P_{new}V = 2(PV)$,which gives $P_{new} = 2P$. Since each gas has mass $M$,the total mass of the mixture is $M + M = 2M$. Therefore,the new pressure is $2P$ and the total mass is $2M$.

Class 11 Physics Kinetic Theory of Gases Mixture of Gases

Easy

Two gases have temperature $T$,pressure $P$,and volume $V$ each. If they are mixed in a container of volume $V$ at the same temperature $T$,what will be the new pressure and mass of the mixture?

A
$2P$ and $2M$
B
$P$ and $M$
C
$P$ and $2M$
D
$2P$ and $M$

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Class 11

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Kinetic Theory of Gases

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Mixture of Gases

If three moles of monoatomic gas $\left(\gamma=\frac{5}{3}\right)$ is mixed with two moles of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$,the value of adiabatic exponent $\gamma$ for the mixture is:

DifficultJEE MAIN 2024

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When one mole of monatomic gas is mixed with one mole of a diatomic gas,then the equivalent value of $\gamma$ for the mixture will be (vibration mode neglected).

Medium

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$A$ cylinder consists of a gas mixture of helium and oxygen. If the mass of helium is $4 \,g$ and the mass of oxygen is $32 \,g$, then the ratio of specific heat of the mixture $\left(C_p / C_V\right)$ is:

EasyTS EAMCET 2021

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If a mixture of $28 \, g$ of Nitrogen $(N_2)$,$4 \, g$ of Hydrogen $(H_2)$,and $8 \, g$ of Helium $(He)$ is contained in a vessel at temperature $400 \, K$ and pressure $8.3 \times 10^5 \, Pa$,the density of the mixture will be:

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$A$ rigid tank contains $35 \, kg$ of nitrogen at $6 \, atm$. $A$ sufficient quantity of oxygen is supplied to increase the pressure to $9 \, atm$,while the temperature remains constant. The amount of oxygen supplied to the tank is .... $kg$.

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Two gases have temperature $T$,pressure $P$,and volume $V$ each. If they are mixed in a container of volume $V$ at the same temperature $T$,what will be the new pressure and mass of the mixture?

Similar Questions

If three moles of monoatomic gas $\left(\gamma=\frac{5}{3}\right)$ is mixed with two moles of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$,the value of adiabatic exponent $\gamma$ for the mixture is:

When one mole of monatomic gas is mixed with one mole of a diatomic gas,then the equivalent value of $\gamma$ for the mixture will be (vibration mode neglected).

$A$ cylinder consists of a gas mixture of helium and oxygen. If the mass of helium is $4 \,g$ and the mass of oxygen is $32 \,g$, then the ratio of specific heat of the mixture $\left(C_p / C_V\right)$ is:

If a mixture of $28 \, g$ of Nitrogen $(N_2)$,$4 \, g$ of Hydrogen $(H_2)$,and $8 \, g$ of Helium $(He)$ is contained in a vessel at temperature $400 \, K$ and pressure $8.3 \times 10^5 \, Pa$,the density of the mixture will be:

$A$ rigid tank contains $35 \, kg$ of nitrogen at $6 \, atm$. $A$ sufficient quantity of oxygen is supplied to increase the pressure to $9 \, atm$,while the temperature remains constant. The amount of oxygen supplied to the tank is .... $kg$.

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