The correct thermodynamic conditions for the spontaneous reaction at all temperatures is:

△ H < 0

and

△ S = 0

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△ H = 0

and

△ S < 0

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△ H < 0

and

△ S > 0

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△ H < 0

and

△ S < 0

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Solution

The correct option is C $△ H < 0$ and $△ S > 0$
The correct thermodynamic conditions for the spontaneous reaction at all temperatures is

$△ H < 0$ and $△ S > 0$
Under these conditions, $Δ G = Δ H - T Δ S < 0$
The correct thermodynamic conditions for the spontaneous reaction at all temperatures is
$△ H < 0$ and $△ S > 0$
Under these conditions, $Δ G = Δ H - T Δ S < 0$
Note: for spontaneous reactions, $Δ G < 0$ , for non spontaneous reactions, $Δ G > 0$ , for reactions at equilibrium, $Δ G = 0$

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Similar questions

For a non-spontaneous reaction, at 30 $^{0}$ C, $Δ$ H>0 & $Δ$ S > 0. The reaction becomes spontaneous,elta by

△ H

△ S

A + B ⟶ 3 C

P C l_{5} (g) △ ⇌ P C l_{3} (g) + C l_{2} (g) :

Δ H^{0}

Δ S^{0}

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