Calculate the sign of $\Delta S$ for the melting of ice at $275 \ K$.

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 $-286 \text{ kJ mol}^{-1}$?

The enthalpy of vaporization of benzene is $+35.3 \ kJ/mol$ at its boiling point,$80^{\circ} C$. The entropy change in the transition of vapour to liquid at its boiling point is

In which of the following processes does entropy increase?

If the standard molar entropies $(S^o)$ for $H_2$,$Cl_2$,and $HCl$ are $0.13$,$0.22$,and $0.19 \, kJ \, K^{-1} \, mol^{-1}$ respectively,what is the total change in standard entropy $(\Delta S^o)$ for the reaction $H_2 + Cl_2 \rightarrow 2HCl$ in $J \, K^{-1} \, mol^{-1}$?

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).