Which of the following processes involves zero work done?

Identify the process from the following such that the volume of the system remains constant.

If $5 \ mol$ of an ideal gas expands from $10 \ L$ to a volume of $100 \ L$ at $300 \ K$ under isothermal and reversible conditions,then the work done,$w$,is $-x \ J$. The value of $x$ is $ . . . . . . $. (Given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)

For the reaction of nitrogen with hydrogen to form ammonia,$\Delta H^o = -92.2 \ kJ/mol$. If the reaction is carried out at a constant pressure of $20.0 \ atm$ and a volume change of $-1.16 \ L$,calculate the change in internal energy $(\Delta U)$ in $kJ$.

Calculate the final temperature of a monoatomic ideal gas that is compressed reversibly and adiabatically from $16 \, L$ to $2 \, L$ at $300 \, K$. (in $, K$)

Which of the following is correct regarding the internal energy of a substance?