(D) According to the ideal gas equation,$PV = nRT$.Rearranging this,we get $\frac{PV}{T} = nR$.Here,$R$ is the universal gas constant,and $n$ is the n

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(D) According to the ideal gas equation,$PV = nRT$.Rearranging this,we get $\frac{PV}{T} = nR$.Here,$R$ is the universal gas constant,and $n$ is the number of moles.If the mass of the gas is constant,the number of moles $n$ remains constant.Since both $n$ and $R$ are constant,their product $(nR)$ is also a constant.Therefore,the equation $\frac{PV}{T} = \text{constant}$ holds true for a constant mass of an ideal gas undergoing any type of thermodynamic process.Correct choice is option $D$.

Class 11 Physics Kinetic Theory of Gases Gas Laws (Charles, Boyle's, Avagadro's, Gay Lussacs and Dalton's law) and Ideal gas Equation

Medium

The gas equation $\frac{PV}{T} = \text{constant}$ is true for a constant mass of an ideal gas undergoing:

A
Isothermal change
B
Adiabatic change
C
Isobaric change
D
Any type of change

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Kinetic Theory of Gases

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Gas Laws (Charles, Boyle's, Avagadro's, Gay Lussacs and Dalton's law) and Ideal gas Equation

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The volume versus temperature graph for a fixed amount of gas at constant pressures $P_1$ and $P_2$ is shown in the figure. From this,it can be concluded that...........

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The gas equation $\frac{PV}{T} = \text{constant}$ is true for a constant mass of an ideal gas undergoing:

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$A$ gas at $27^oC$ has a volume $V$ and pressure $P$. On heating,its pressure is doubled and volume becomes three times. The resulting temperature of the gas will be ...... $^oC$.

When air is pumped into a cycle tyre, the volume and pressure of the air in the tyre both increase. What about Boyle's law in this case?

One mole of an ideal gas undergoes a process $P = \frac{2V^2}{1+V^2} \, Pa$. The change in temperature of the gas when the volume changes from $V = 1 \, m^3$ to $V = 2 \, m^3$ is:

The volume versus temperature graph for a fixed amount of gas at constant pressures $P_1$ and $P_2$ is shown in the figure. From this,it can be concluded that...........

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