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(A) For a spontaneous reaction,the Gibbs free energy change $ \Delta G $ must be negative,where $ \Delta G = \Delta H - T \Delta S $.If $ \Delta H $ i

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$ \Delta H $ value is positive and $ \Delta S $ value is negative

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(A) For a spontaneous reaction,the Gibbs free energy change $ \Delta G $ must be negative,where $ \Delta G = \Delta H - T \Delta S $.If $ \Delta H $ is positive and $ \Delta S $ is negative,then $ \Delta G = (+ \Delta H) - T(- \Delta S) = + \Delta H + T \Delta S $.Since both terms are positive,$ \Delta G $ will always be positive regardless of the temperature $ T $.Therefore,the reaction cannot occur spontaneously under any conditions.

$A$ chemical reaction cannot occur at all if

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