d (d) Slow isothermal expansion or compression of an ideal gas is reversible process, while the other given process are irreversible in nature.
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One mole of a monatomic ideal gas undergoes an adiabatic expansion in which its volume becomes eight times its initial value. If the initial temperature of the gas is $100 K$ and the universal gas constant $R =8.0 Jmol ^{-1} K ^{-1}$, the decrease in its internal energy, in Joule, is. . . . .
A fixed amount of a gas undergoes a thermodynamic process as shown such that heat interaction along path $B \to C \to A$ is equal to the work done by the gas along path $A \to B \to C$. Then process $A \to B$ is :-
Starting with the same initial conditions, an ideal gas expands from volume $V_{1}$ to $V_{2}$ in three different ways. The work done by the gas is $W_{1}$ if the process is purely isothermal. $W _{2}$. if the process is purely adiabatic and $W _{3}$ if the process is purely isobaric. Then, choose the coned option