One mole of an ideal monatomic gas undergoes a reversible process described by $PV^2 = ext{constant}$. The molar heat capacity of the gas during this process is:

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

An ideal gas at a pressure of 1 atom sphere and temperature of ${27^0}C$ is compressed adiabatically until its pressure becomes 8 times the initial pressure, then the final temperature is $\left( {\gamma = \frac{3}{2}} \right)$

If for a gas $\frac{R}{{{C_V}}}$, the gas may be made up of molecules which are

The specific heats of an ideal gas at constant pressure and constant volume are 525 J ${(k{g^ \circ }C)^{( - 1)}}$ and $315{\rm{J}}{\left( {{\rm{kg^\circ C}}} \right)^{ - 1}}$ respectively. Its density at NTP is

Boyle’s law holds for an ideal gas during

The specific heats of an ideal gas at constant pressure and constant volume are 525 J ${(k{g^ \circ }C)^{( - 1)}}$ and $315{\rm{J}}{\left( {{\rm{kg^\circ C}}} \right)^{ - 1}}$ respectively. Its density at NTP is

One mole of an ideal gas expands at a constant temperature of $300K$ from an initial volume of $10\,\,\,litres$to a final volume of $20\,\,\,litres$. The work done in expanding the gas is $(R = 8.31J/mole - K)$

500 J of heat energy is removed from 4 moles of a monoatomic ideal gas at constant volume. The temperature drops by

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

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