For a reaction- 2Kg - Lg- 2Mg - - U0 - -10-5 kJ and - S0 - -44-1 J K-1- Calculate - G0 for the reaction and predict whether the reaction will be spontaneous or non-spontaneous-

Which of the following is not correct?
(a) $Δ$ G is zero for a reversible reaction.
(b) $Δ$ G is positive for a spontaneous reaction.
(c) $Δ$ G is negative for a spontaneous reaction.
(d) $Δ$ G is positive for a non-spontaneous reaction.

Q. For a certain reaction,

Δ H^{0}

and

Δ S^{0}

respectively are 400 kJ and 200 J/Mole/K. The process is non-spontaneous at:

Q. Assertion :All exothermic reactions are spontaneous at room temperature. Reason:

Δ G

=-ve for above reactions and for spontaneous reactions

Δ G = - v e

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For a reaction, 2K(g)+L(g)→2M(g);ΔU0 = -10.5 kJ and ΔS0 = -44.1 J K−1. Calculate ΔG0 for the reaction and predict whether the reaction will be spontaneous or non-spontaneous.

The correct option is A ΔG = + 0.16 kJ, non-spontaneous2K+L→2MΔng = 2-3 = -1ΔH=ΔU+ΔngRT=−10.5×103+(−1×8.314×298)=−12.98kJΔG0=ΔH0−TΔS0=−12.98−298(−44.1×10−3)=0.16kJSince ΔG0 is +ve, hence it is non-spontaneous.

For a reaction, $2 K_{(g)} + L_{(g)} \to 2 M_{(g)}; Δ U^{0}$ = -10.5 kJ and $Δ S^{0}$ = -44.1 J $K^{- 1}$ . Calculate $Δ G^{0}$ for the reaction and predict whether the reaction will be spontaneous or non-spontaneous.