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 $, K$)

One mole of an ideal gas at $300 \ K$ is expanded isothermally from an initial volume of $1 \ L$ to $10 \ L$. The value of $\Delta E$ for this process is $(R = 2 \ cal \ mol^{-1} \ K^{-1})$.

In the equation $C_P - C_V = R$,what does $R$ represent?

Which of the following statements is not correct?

Work done when $2 \ mol$ of an ideal gas is compressed from a volume of $5 \ m^{3}$ to $2.5 \ m^{3}$ at $300 \ K$, under a constant external pressure of $100 \ kPa$ is: (in $kJ$)

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 $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)