Dissolution of ammonium chloride in water is an endothermic reaction- yet it is a spontaneous -160-process- This is due to the fact that - -H is -ve- - -S is -ve- -H is -ve- - -S is -ve- -H is -ve and - -H - T- -S- -H is -ve- - -S is -ve and - -H

The correct option is D Δ H is +ve, Δ S is +ve and Δ H Δ H gt;0 (endothermic reaction)Now, Δ G=Δ H TΔ S For spontaneous process, ...

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Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

Dissolution o...

Question

Dissolution of ammonium chloride in water is an endothermic reaction, yet it is a spontaneous process. This is due to the fact that :

Δ

H is +ve,

Δ

S is -ve.

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Δ

H is -ve,

Δ

S is +ve.

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Δ

H is +ve,

Δ

S is +ve and

Δ

H < T

Δ

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Δ

H is +ve and

Δ

H > T

Δ

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Solution

The correct option is D $Δ$ H is +ve, $Δ$ S is +ve and $Δ$ H < T $Δ$ S
$Δ H > 0$ (endothermic reaction)
Now, $Δ G = Δ H - T Δ S$
For spontaneous process, $Δ G < 0$
Therefore, $Δ G = Δ H - T Δ S < 0$
But $Δ H > 0$
Therefore for $Δ G$ to be negative, $Δ S > 0$ and $Δ H < T Δ S$ .

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(b)

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

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Dissolution of ammonium chloride in water is an endothermic reaction, yet it is a spontaneous process. This is due to the fact that :

The correct option is D ΔH is +ve, ΔS is +ve and ΔH < TΔSΔH>0 (endothermic reaction)Now, ΔG=ΔH−TΔSFor spontaneous process, ΔG<0Therefore, ΔG=ΔH−TΔS<0But ΔH>0Therefore for ΔG to be negative, ΔS>0 and ΔH<TΔS.

The correct option is D $Δ$ H is +ve, $Δ$ S is +ve and $Δ$ H < T $Δ$ S
$Δ H > 0$ (endothermic reaction)
Now, $Δ G = Δ H - T Δ S$
For spontaneous process, $Δ G < 0$
Therefore, $Δ G = Δ H - T Δ S < 0$
But $Δ H > 0$
Therefore for $Δ G$ to be negative, $Δ S > 0$ and $Δ H < T Δ S$ .