At the boiling point of water,$900 \ J/g$ of heat is exchanged. What is the increase in entropy in $J \ K^{-1} \ mol^{-1}$?

For the reaction $2 H_{2(g)} + O_{2(g)} \longrightarrow 2 H_2O_{(g)}$,at $300 \ K$,$\Delta G$ and $\Delta H$ of water are $-228.4 \ kJ \ mol^{-1}$ and $-241.60 \ kJ \ mol^{-1}$,respectively. Calculate the value of change in entropy for the given reaction.

Standard entropies of $X_2, Y_2$ and $XY_5$ are $70, 50$ and $110 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature in Kelvin at which the reaction $\frac{1}{2} X_2 + \frac{5}{2} Y_2 \rightarrow XY_5$ with $\Delta H = -35 \ kJ \ mol^{-1}$ will be at equilibrium is . . . . . . (Nearest integer).

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

An irreversible process occurring isothermally in an isolated system leads to

For the reaction $H_2O_{(l)} \longrightarrow H_2O_{(g)}$ at $T=100^{\circ} C$ and $P=1 \ atm$,choose the correct option: