A diatomic ideal gas undergoes a thermodynamic process in which its molar heat capacity is $C = \frac{3R}{2}$. Which of the following processes could this represent?

Which of the following thermodynamic processes involves no heat exchange with the surroundings?

A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is gain reduced to half. Then:

An ideal gas at ${27^0}C$ is compressed adiabatically to 8/7 of its original volume. If $\gamma = \frac{5}{3}$ then the rise in temperature is

In a polytropic process, the relation between pressure and volume is given by $PV^n = ext{constant}$. For an adiabatic process involving an ideal gas, the value of 'n' is equal to:

An ideal gas undergoes isothermal compression to half its volume. If the same gas undergoes adiabatic compression to the same final volume, which process requires more work done by the surroundings?

During an adiabatic process, the pressure of a gas is found to be proportional to the cube of its absolute temperature. The $\gamma$ of the gas is

The gas law $\frac{{PV}}{T}$ = constant is true for

Pressure – Temperature relationship for an ideal gas undergoing adiabatic change is $\left( {\gamma = \frac{{{C_P}}}{{{C_V}}}} \right)$

Two identical cylinders contain the same ideal gas. Cylinder A undergoes isothermal compression to half its initial volume. Cylinder B undergoes adiabatic compression to half its initial volume. Which cylinder experiences a greater change in pressure?

During an adiabatic process, the pressure of a gas is found to be proportional to the cube of its absolute temperature. The $\gamma$ of the gas is