Which of the following processes will never b | vedclass

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(D) For a process to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative $(\Delta G < 0)$.The relationship is given by $\Delta G =

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$2Ag + 3N_2 ightarrow 2AgN_3, \Delta H = 	ext{positive}, \Delta S = 	ext{negative}$

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(D) For a process to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative $(\Delta G The relationship is given by $\Delta G = \Delta H - T\Delta S$.For option $D$,$\Delta H$ is positive and $\Delta S$ is negative.Therefore,$\Delta G = (+\Delta H) - T(-\Delta S) = (+\Delta H) + (T\Delta S)$.Since both terms are positive,$\Delta G$ will always be positive at all temperatures.Thus,the process will never be spontaneous.

Which of the following processes will never be a spontaneous process?

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