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Thermodynamic Processes

Which of the ...

Question

Which of the following conditions make the process non spontaneous at all temperatures.

Δ

H = +ve;

Δ

S = -ve

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Δ

H = -ve;

Δ

S = +ve

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Δ

H = +ve;

Δ

S = +ve

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Δ

H = -ve;

Δ

S = -ve

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Solution

The correct option is A $Δ$ H = +ve; $Δ$ S = -ve
$Δ G = Δ H - T Δ S$
for $Δ H$ +ve & $Δ S$ -ve $Δ G$ will be always positve
$∴$ The reaction will be non - spontaneous at all temerpature

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\begin{matrix} Δ H & Δ S & Temperature & Spontanity I. & \oplus v e & ⊖ v e & Any temperature & Non-spontaneous II. & ⊖ v e & ⊖ v e & Low temperature & Non-spontaneous III. & \oplus v e & \oplus v e & Low temperature & Spontaneous IV. & ⊖ v e & \oplus v e & Any temperature & Spontaneous \end{matrix}

\begin{matrix} Δ H & Δ S & Temperature & Spontaneity I. & \oplus v e & ⊖ v e & Any temperature & Non-spontaneous II. & ⊖ v e & ⊖ v e & Low temperature & Non-spontaneous III. & \oplus v e & \oplus v e & Low temperature & Spontaneous IV. & ⊖ v e & \oplus v e & Any temperature & Spontaneous \end{matrix}

2 O_{3} (g) \to 3 O_{2} (g), △ H

△ S

△ G

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