For a reaction $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)$ at equilibrium, the partial pressure of $\mathrm{B}$ is found to be one-fourth of the particle pressure of $\mathrm{A}$. The value of $\mathrm{\Delta G}°$ of the reaction $\mathrm{A}\to \mathrm{B}$ is

The value of ${\log }_{10} \mathrm{K}$ for a reaction $\mathrm{A}\rightleftharpoons \mathrm{B}$ is

(Given ${\mathrm{\Delta }}_{\mathrm{r}}{{\mathrm{H}}^{\mathrm{o}}}_{298 \mathrm{K}}=-54.07 \mathrm{kJ} {\mathrm{mol}}^{-1}, {\mathrm{\Delta }}_{\mathrm{r}}{{\mathrm{S}}^{\mathrm{o}}}_{298 \mathrm{K}}=10 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$ and $\mathrm{R}=8.314 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}; 2.303\times 8.314\times 298=5705$)

Predict which of the following reaction(s) has a positive entropy change?

$\left(\mathrm{I}\right) {\mathrm{Ag}}^{+ }\left(\mathrm{aq}\right)+{\mathrm{Cl}}^{-} \left(\mathrm{aq}\right)\to \mathrm{AgCl} \left(\mathrm{s}\right)$

$\left(\mathrm{II}\right) {\mathrm{NH}}_4\mathrm{Cl} \left(\mathrm{s}\right)\to {\mathrm{NH}}_3 \left(\mathrm{g}\right)+\mathrm{HCl} \left(\mathrm{g}\right)$

$\left(\mathrm{III}\right) 2{\mathrm{NH}}_3\left(\mathrm{g}\right)\to {\mathrm{N}}_2 \left(\mathrm{g}\right)+3{\mathrm{H}}_2 \left(\mathrm{g}\right)$

For the reaction:

$\mathrm{A}(\mathrm{g},1\mathrm{bar})+\frac{1}{2}{\mathrm{B}}_2(\mathrm{g},25\mathrm{bar})\rightleftharpoons \mathrm{AB}\left(\mathrm{g}\right)$

What is the initial free energy change?

For an ideal gas, consider only $\mathrm{P}-\mathrm{V}$ work in going from an initial state $\mathrm{X}$ to the final state $\mathrm{Z}$. The final state $\mathrm{Z}$ can be reached by either of the two paths shown in the figure. Which of the following choice(s) is(are) correct? [Take $\mathrm{\Delta S}$ as change in entropy and $\mathrm{w}$ as work done.]

Select the correct statement for the equilibrium under standard conditions:

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); {\mathrm{\Delta S}}_1^{\circ }$

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right); {\mathrm{\Delta S}}_2^{\mathrm{o}}$

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right); {\mathrm{\Delta S}}_3^{\mathrm{o}}$