A rigid diatomic ideal gas undergoes an adiabatic process at room temperature. The rational between temperature and volume for the process is $TV^x =$ constant, then $x$ is

One mole of an ideal gas expands adiabatically from an initial state $\left(T_A, V_0\right)$ to final state $\left(T_f, 5 V_0\right)$. Another mole of the same gas expands isothermally from a different initial state ( $T_{\mathrm{B}}, \mathrm{V}_0$ ) to the same final state $\left(T_{\mathrm{f}}, 5 V_0\right)$. The ratio of the specific heats at constant pressure and constant volume of this ideal gas is $\gamma$. What is the ratio $T_{\mathrm{A}} / T_{\mathrm{B}}$ ?

During the adiabatic expansion of $2 \,moles$ of a gas, the internal energy was found to have decreased by $100 J$. The work done by the gas in this process is ….. $J$

For two different gases $X$ and $Y$, having degrees of freedom $f_1$ and $f_2$ and molar heat capacities at constant volume $C_{V1}$ and $C_{V2}$ respectively, the ln $P$ versus ln $V$ graph is plotted for adiabatic process, as shown

A tyre filled with air $({27^o}C,$ and $2$ atm) bursts, then what is temperature of air ……. $^oC$ $(\gamma = 1.5)$