314879 Which of the following statement (s) is/are correct?
(I) \(\Delta \mathrm{G}\) is negative, then the reaction is spontaneous and proceeds in the forward direction
(II) \(\Delta \mathrm{G}\) is positive, then reaction is non spontaneous
(III) \(\Delta \mathrm{G}\) is 0, then reaction is at equilibrium

314880 For the reaction,
\({\text{A(g) + B(g) }} \rightleftharpoons {\text{ C(g) + D(g)}}\), \(\Delta {\text{H}}^\circ \) and \(\Delta {\text{S}}^\circ \) and \(\Delta {\text{S}}^\circ \) are, respectively, \( - 29.8{\text{kJ}}{\text{mo}}{{\text{l}}^{ - 1}}\) and \(-0.100 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) at \(298 \mathrm{~K}\). The equilibrium constant for the reaction at \(298 \mathrm{~K}\) is:

314881 The equilibrium concentrations of the species in the reaction \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\) are \(2,3,10\) and \(6 \mathrm{~mol} \mathrm{~L}^{-1}\), respectively at \(300 \mathrm{~K}\). \(\Delta \mathrm{G}^{\circ}\) for the reaction is \((\mathrm{R}=2 \mathrm{cal} / \mathrm{mol} \mathrm{K})\)

314882 If \(\Delta G^{0}\) for the reaction given below is \(1.7 \mathrm{~kJ}\), the equilibrium constant for a reaction, \(2 \mathrm{HI}_{(\mathrm{g})} \rightleftharpoons \mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})}\) at \(25^{\circ} \mathrm{C}\) is

314879 Which of the following statement (s) is/are correct?
(I) \(\Delta \mathrm{G}\) is negative, then the reaction is spontaneous and proceeds in the forward direction
(II) \(\Delta \mathrm{G}\) is positive, then reaction is non spontaneous
(III) \(\Delta \mathrm{G}\) is 0, then reaction is at equilibrium

314880 For the reaction,
\({\text{A(g) + B(g) }} \rightleftharpoons {\text{ C(g) + D(g)}}\), \(\Delta {\text{H}}^\circ \) and \(\Delta {\text{S}}^\circ \) and \(\Delta {\text{S}}^\circ \) are, respectively, \( - 29.8{\text{kJ}}{\text{mo}}{{\text{l}}^{ - 1}}\) and \(-0.100 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) at \(298 \mathrm{~K}\). The equilibrium constant for the reaction at \(298 \mathrm{~K}\) is:

314881 The equilibrium concentrations of the species in the reaction \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\) are \(2,3,10\) and \(6 \mathrm{~mol} \mathrm{~L}^{-1}\), respectively at \(300 \mathrm{~K}\). \(\Delta \mathrm{G}^{\circ}\) for the reaction is \((\mathrm{R}=2 \mathrm{cal} / \mathrm{mol} \mathrm{K})\)

314882 If \(\Delta G^{0}\) for the reaction given below is \(1.7 \mathrm{~kJ}\), the equilibrium constant for a reaction, \(2 \mathrm{HI}_{(\mathrm{g})} \rightleftharpoons \mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})}\) at \(25^{\circ} \mathrm{C}\) is

314879 Which of the following statement (s) is/are correct?
(I) \(\Delta \mathrm{G}\) is negative, then the reaction is spontaneous and proceeds in the forward direction
(II) \(\Delta \mathrm{G}\) is positive, then reaction is non spontaneous
(III) \(\Delta \mathrm{G}\) is 0, then reaction is at equilibrium

314880 For the reaction,
\({\text{A(g) + B(g) }} \rightleftharpoons {\text{ C(g) + D(g)}}\), \(\Delta {\text{H}}^\circ \) and \(\Delta {\text{S}}^\circ \) and \(\Delta {\text{S}}^\circ \) are, respectively, \( - 29.8{\text{kJ}}{\text{mo}}{{\text{l}}^{ - 1}}\) and \(-0.100 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) at \(298 \mathrm{~K}\). The equilibrium constant for the reaction at \(298 \mathrm{~K}\) is:

314881 The equilibrium concentrations of the species in the reaction \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\) are \(2,3,10\) and \(6 \mathrm{~mol} \mathrm{~L}^{-1}\), respectively at \(300 \mathrm{~K}\). \(\Delta \mathrm{G}^{\circ}\) for the reaction is \((\mathrm{R}=2 \mathrm{cal} / \mathrm{mol} \mathrm{K})\)

314882 If \(\Delta G^{0}\) for the reaction given below is \(1.7 \mathrm{~kJ}\), the equilibrium constant for a reaction, \(2 \mathrm{HI}_{(\mathrm{g})} \rightleftharpoons \mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})}\) at \(25^{\circ} \mathrm{C}\) is

314879 Which of the following statement (s) is/are correct?
(I) \(\Delta \mathrm{G}\) is negative, then the reaction is spontaneous and proceeds in the forward direction
(II) \(\Delta \mathrm{G}\) is positive, then reaction is non spontaneous
(III) \(\Delta \mathrm{G}\) is 0, then reaction is at equilibrium

314880 For the reaction,
\({\text{A(g) + B(g) }} \rightleftharpoons {\text{ C(g) + D(g)}}\), \(\Delta {\text{H}}^\circ \) and \(\Delta {\text{S}}^\circ \) and \(\Delta {\text{S}}^\circ \) are, respectively, \( - 29.8{\text{kJ}}{\text{mo}}{{\text{l}}^{ - 1}}\) and \(-0.100 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\) at \(298 \mathrm{~K}\). The equilibrium constant for the reaction at \(298 \mathrm{~K}\) is:

314881 The equilibrium concentrations of the species in the reaction \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+\mathrm{D}\) are \(2,3,10\) and \(6 \mathrm{~mol} \mathrm{~L}^{-1}\), respectively at \(300 \mathrm{~K}\). \(\Delta \mathrm{G}^{\circ}\) for the reaction is \((\mathrm{R}=2 \mathrm{cal} / \mathrm{mol} \mathrm{K})\)

314882 If \(\Delta G^{0}\) for the reaction given below is \(1.7 \mathrm{~kJ}\), the equilibrium constant for a reaction, \(2 \mathrm{HI}_{(\mathrm{g})} \rightleftharpoons \mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})}\) at \(25^{\circ} \mathrm{C}\) is