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(C) For a reaction to be spontaneous, the Gibbs free energy change must be negative, i.e.,$\Delta_r G^{\circ} < 0$.The relationship is given by: $\Del

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$B$ and $C$

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(C) For a reaction to be spontaneous, the Gibbs free energy change must be negative, i.e.,$\Delta_r G^{\circ} The relationship is given by: $\Delta_r G^{\circ} = \Delta_r H^{\circ} - T \Delta_r S^{\circ}$.Analyzing the table:$1$. For row $B$: $\Delta_r H^{\circ} = (+)$, $\Delta_r S^{\circ} = (+)$. $\Delta_r G^{\circ}$ is negative when $T \Delta_r S^{\circ} > \Delta_r H^{\circ}$, which occurs at high temperatures. Thus, $B$ is correct.$2$. For row $C$: $\Delta_r H^{\circ} = (-)$, $\Delta_r S^{\circ} = (-)$. $\Delta_r G^{\circ}$ is negative when $|\Delta_r H^{\circ}| > |T \Delta_r S^{\circ}|$, which occurs at low temperatures. Thus, $C$ is correct.Rows $A$ and $D$ show positive $\Delta_r G^{\circ}$ values, which correspond to non-spontaneous processes under the conditions listed.Therefore, options $B$ and $C$ are correct.

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

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