If the enthalpy of vaporization for water is $186.5 \ kJ \ mol^{-1}$,the entropy of its vaporization will be ...... $J \ K^{-1} \ mol^{-1}$ (Assume the boiling point of water is $373 \ K$).

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

$STATEMENT-1:$ There is a natural asymmetry between converting work to heat and converting heat to work.
$STATEMENT-2:$ No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.

Which of the following processes is associated with a decrease in entropy?

What is the change in entropy of the surroundings for the reaction, $H_2(g) + 1/2 O_2(g) \rightarrow H_2O(l)$ at $298 \text{ K}$, if the standard enthalpy of formation of water is $-286 \text{ kJ mol}^{-1}$?

Which of the following reactions will have the value of $\Delta S$ with a negative sign?