During an adiabatic process, the pressure and volume of an ideal gas are related by $PV^\gamma = ext{constant}$. If the ratio of specific heats $\gamma$ is $\frac{5}{3}$, the work done by the gas when the volume changes from $V_1$ to $V_2$ is:

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?

The specific heat of a gas

In an isothermal reversible expansion, if the volume of $96g$ of oxygen at ${27^ \circ }C$ is increased from $70litres$ to $140litres$, then the work done by the gas will be

Two moles of an ideal monoatomic gas at ${27^ \circ }C$ occiupies a volume of $V$. If the gas is expanded adiabatially to the volume 2$V$, then the work done by the gas will be $\left( {\gamma = \frac{5}{3},R = 8.31{\rm{J}}/{\rm{mol}} - {\rm{K}}} \right)$

Two interconnected, thermally insulated chambers of equal volume are separated by a valve. One chamber contains an ideal gas at $273 K$ and $1 atm$, while the other is evacuated. If the valve is opened, allowing the gas to freely expand, what is the final temperature of the gas?

For an adiabatic process, the correct relation is:

If 2 moles of an ideal gas are compressed adiabatically to one-fourth of their original volume, which of the following is true about the work done?

During an isothermal expansion of an ideal gas:

Two cylinders ${\rm{A}}$ and ${\rm{B}}$ of equal capacity are connected to each other via a stop cock. ${\rm{A}}$ contains an ideal gas at standard temperature and pressure. ${\rm{B}}$ is completely evacuated. The entire system is thermally insulated. The stop cock is suddenly opened. The process is:

When $1kg$ of ice at ${0^ \circ }C$melts to water at ${0^ \circ }C$, the resulting change in its entropy, taking latent heat of ice to be $80cal{/^ \circ }C$ is