Question

One mole of an ideal monoatomic gas expends isothermally against constant external pressure of $1$ atm from initial volume of $1L$ to a state where its final pressure become equal to external pressure. If initial temperature of gas is $300K$ then total entropy change of system in the above process is:$[R=0.082Latmmo{l}^{-1}{K}^{-1}=8.3Jmo{l}^{-1}{K}^{-1}]$

• A. $0$
• B. $R\ell n\left(24.6\right)$
• C. $R\ell n\left(2490\right)$
• D. $\frac{3}{2}R\ell n\left(24.6\right)$

Answer 1

The correct option is A $0$

Solution:- (A) $0$

As we know that,

$\Delta S=2.303nR\log \frac{P_i}{P_f}$

As the initial pressure and final pressure of the gas is equal.

Hence the total entropy change of the system is $0$.