At $300 \ K$,for the reaction $A \rightarrow P$,the $\Delta S_{sys}$ is $5 \ J \ K^{-1} \ mol^{-1}$. What is the heat absorbed (in $kJ \ mol^{-1}$) by the system?

One mole of an ideal gas at $350 \, K$ is in a $2.0 \, L$ vessel with thermally conducting walls,which are in contact with the surroundings. It undergoes isothermal expansion from $2.0 \, L$ to $3.0 \, L$ against a constant external pressure of $4 \, atm$. The change in entropy of the surroundings $(\Delta S_{surr})$ is $...... \, J \, K^{-1}$ (Nearest integer). Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$.

For the process $H_2O(\ell) \rightarrow H_2O_{(g)}$ at $T = 100^{\circ} C$ and $1 \ atm$ pressure,the correct choice is:

For the reaction $NH_4Cl_{(s)} \rightarrow NH_{3(g)} + HCl_{(g)}$,the entropy change is ...... .

Maximum entropy will be in which of the following?

Which of the following equations indicates an increase in entropy?