For the reaction $2\mathrm{A} \left(\mathrm{g}\right) + \mathrm{B}\left(\mathrm{g}\right) \to 2\mathrm{D} \left(\mathrm{g}\right)$; $∆\mathrm{U}° = -10.5 \mathrm{kJ} \mathrm{and} ∆\mathrm{S}° = -44.1 \mathrm{J} {\mathrm{K}}^{-1}$ , the value of $∆\mathrm{G}°$ for the given reaction would be-

1. 1.6 J

2. - 0.16 KJ

3. 0.16 KJ

4. 1.6 KJ

The equilibrium constant for a reaction is 10. The value of $∆\mathrm{G}°$ will be-

($\mathrm{R} = 8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1} ; \mathrm{T} = 300 \mathrm{K}$)

$$\begin{gathered} 1. -5.74 \mathrm{kJ} {\mathrm{mol}}^{-1} \\ 2. - 5.74 \mathrm{J} {\mathrm{mol}}^{-1} \\ 3. + 4.57 \mathrm{kJ} {\mathrm{mol}}^{-1} \\ 4. -57.4 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$