Which of the following reactions is expected | vedclass

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(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be non-spontan

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$2Ag + 3N_2 \rightarrow 2AgN_3$; $\Delta H = +ve, \Delta S = -ve$

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(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be non-spontaneous at all temperatures,$\Delta G$ must always be positive. This occurs when $\Delta H$ is positive (endothermic) and $\Delta S$ is negative (decrease in entropy). In option $D$,$\Delta H = +ve$ and $\Delta S = -ve$,so $\Delta G = (+ve) - T(-ve) = (+ve) + (T 	imes +ve)$,which is always positive. Therefore,the reaction in option $D$ is never spontaneous.

	$\Delta_r H^{\circ}$	$\Delta_r S^{\circ}$	$\Delta_r G^{\circ}$	Spontaneity of the reaction
$A$	$+$	$+$	$+$	Spontaneous at low $T$
$B$	$+$	$+$	$-$	Spontaneous at high $T$
$C$	$-$	$-$	$-$	Spontaneous at low $T$
$D$	$+$	$-$	$+$	Spontaneous at high $T$

Which of the following reactions is expected to never be spontaneous?

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