A reaction at 1 bar is non-spontaneous at lo | vedclass

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(A) 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 spontaneous,

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

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(A) 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 spontaneous,$\Delta G$ must be negative $(\Delta G If $\Delta H > 0$ (endothermic) and $\Delta S > 0$ (increase in entropy),then at high temperatures,the term $T\Delta S$ becomes larger than $\Delta H$.Consequently,$\Delta G = \Delta H - T\Delta S$ becomes negative,making the reaction spontaneous at high temperatures.At low temperatures,$T\Delta S < \Delta H$,so $\Delta G$ is positive,making the reaction non-spontaneous.

Condition	Details
$A$. $\Delta H: +, \Delta S: -$	$T$: any $T$,Spontaneity: Non-spontaneous
$B$. $\Delta H: +, \Delta S: +$	$T$: low $T$,Spontaneity: Non-spontaneous
$C$. $\Delta H: -, \Delta S: -$	$T$: low $T$,Spontaneity: Spontaneous
$D$. $\Delta H: -, \Delta S: +$	$T$: any $T$,Spontaneity: Spontaneous

$A$ reaction at $1 \ bar$ is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following:

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