If an endothermic reaction is non-spontaneous at the freezing point of water and becomes feasible at its boiling point,then:

The effect of temperature on the spontaneity of reactions is represented as follows:

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

Which of the above conditions are correctly matched?

The standard entropy change for the reaction $4 Fe ( s ) + 3 O_{2} ( g ) \rightarrow 2 Fe_{2} O_{3} ( s )$ is $-550 \ J K^{-1}$ at $298 \ K$. Given: The standard enthalpy change for the reaction is $-165 \ kJ \ mol^{-1}$. The temperature in $K$ at which the reaction attains equilibrium is ... . (Nearest Integer)

At a temperature of $25^\circ C$,if $\Delta H < T \Delta S$,then $\Delta G$ = ?

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

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

The temperature in $K$ at which $\Delta G = 0$, for a given reaction with $\Delta H = -20.5 \ kJ \ mol^{-1}$ and $\Delta S = -50.0 \ J \ K^{-1} \ mol^{-1}$ is: