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(B) process is spontaneous if $\Delta G  0$. The Gibbs free energy change is given by $\Delta G = \Delta H - T

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$2$

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(B) process is spontaneous if $\Delta G  0$. The Gibbs free energy change is given by $\Delta G = \Delta H - T \Delta S$.For process $A$: $\Delta G = -25000 - (300 	imes -80) = -25000 + 24000 = -1000 \ J \ mol^{-1}$ (Spontaneous).For process $B$: $\Delta G = -22000 - (300 	imes 40) = -22000 - 12000 = -34000 \ J \ mol^{-1}$ (Spontaneous).For process $C$: $\Delta G = 25000 - (300 	imes -50) = 25000 + 15000 = +40000 \ J \ mol^{-1}$ (Non-spontaneous).For process $D$: $\Delta G = 22000 - (300 	imes 20) = 22000 - 6000 = +16000 \ J \ mol^{-1}$ (Non-spontaneous).Thus,processes $C$ and $D$ are non-spontaneous. The total number of non-spontaneous processes is $2$.

Process	$\Delta H \ (kJ \ mol^{-1})$	$\Delta S \ (J \ K^{-1} \ mol^{-1})$
$A$	$-25$	$-80$
$B$	$-22$	$40$
$C$	$25$	$-50$
$D$	$22$	$20$

Reaction	$\Delta H \ (kJ \ mol^{-1}) / \Delta S \ (J \ K^{-1} \ mol^{-1})$
$I$	$+98.0, +14.8$
$II$	$-55.5, -84.6$
$III$	$+28.3, -17.0$
$IV$	$-40.5, +24.6$
$V$	$+34.7, 0.0$

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

For independent processes at $300 \ K$,determine the number of non-spontaneous processes from the following table:

Process $\Delta H \ (kJ \ mol^{-1})$ $\Delta S \ (J \ K^{-1} \ mol^{-1})$

$A$ $-25$ $-80$

$B$ $-22$ $40$

$C$ $25$ $-50$

$D$ $22$ $20$

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For independent processes at $300 \ K$,determine the number of non-spontaneous processes from the following table: Process $\Delta H \ (kJ \ mol^{-1})$ $\Delta S \ (J \ K^{-1} \ mol^{-1})$ $A$ $-25$ $-80$ $B$ $-22$ $40$ $C$ $25$ $-50$ $D$ $22$ $20$