The temperature of a hypothetical gas increases to $\sqrt 2 $ times when compressed adiabatically to half the volume. Its equation can be written as
The $PV$ diagram shows four different possible reversible processes performed on a monatomic ideal gas. Process $A$ is isobaric (constant pressure). Process $B$ is isothermal (constant temperature). Process $C$ is adiabatic. Process $D$ is isochoric (constant volume). For which process$(es)$ does the temperature of the gas decrease?
An ideal gas is compressed to half its initial volume by means of several processes. Which of the process results in the maximum work done on the gas?
An ideal monoatomic gas with pressure $P$, volume $V$ and temperature $T$ is expanded isothermally to a volume $2\, V$ and a final pressure $P_i$. If the same gas is expanded adiabatically to a volume $2\,V$, the final pressure is $P_a$ . The ratio $\frac{{{P_a}}}{{{P_i}}}$ is
A polyatomic gas $\left( {\gamma = \frac{4}{3}} \right)$ is compressed to $\frac{1}{8}$ of its volume adiabatically. If its initial pressure is ${P_o}$, its new pressure will be