Which of the options given below are correct?

Δ H Δ S

Nature of reaction

(-) (+)

Spontaneous at all temperatures

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(+) (-)

Nonspontaneous regardless of temperature

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(+) (+)

Spontaneous only at high temperature

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(-) (-)

Spontaneous only at low temperature

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Solution

The correct options are
A $Δ H Δ S$ Nature of reaction
$(-) (+)$ Spontaneous at all temperatures
B $(+) (-)$ Nonspontaneous regardless of temperature
C $(-) (-)$ Spontaneous only at low temperature
D $(+) (+)$ Spontaneous only at high temperature
Spontaneous and non Spontaneous
Sign of
$△ H$ Sign of
$△ S$ Comment Example $△ H_{298}^{0}$ $△ S_{298}^{0}$
$-$ $+$ Spontaneous
at all temperature $H_{2} (g) + C l_{2} (g) \to 2 H C l (g)$
$C (s) + O_{2} (g) \to C O_{2} (g)$ $- 185 - 394$ $14.1 3$
$-$ $-$ Spontaneous
at low temperature $H_{2} (g) + 1 / 2 O_{2} \to H_{2} O (l)$
$2 S O_{2} (g) + O_{2} (g) \to 2 S O_{3} (g)$ $- 44 - 198$ $- 119 - 187$
$+$ $+$ Spontaneous
at high temperature $N H_{4} C l (s) \to N H_{3} (g) + H C l (g)$
$N_{2} (g) + O_{2} (g) \to 2 N O (g)$ $176180$ $28425$
$+$ $-$ non Spontaneous
at all temperature $3 O_{2} \to 2 O_{3}$
$2 H_{2} O (l) + O_{2} (g) \to 2 H_{2} O_{2} (l)$ $286196$ $- 137 - 126$

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Δ H^{o} = - 33.9 k J a n d Δ S^{o} = - 113 J K^{- 1} m o l^{- 1}

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Sign of $△ H$	Sign of $△ S$	Comment	Example	$△ H_{298}^{0}$	$△ S_{298}^{0}$
$-$	$+$	Spontaneous at all temperature	$H_{2} (g) + C l_{2} (g) \to 2 H C l (g)$ $C (s) + O_{2} (g) \to C O_{2} (g)$	$- 185 - 394$	$14.1 3$
$-$	$-$	Spontaneous at low temperature	$H_{2} (g) + 1 / 2 O_{2} \to H_{2} O (l)$ $2 S O_{2} (g) + O_{2} (g) \to 2 S O_{3} (g)$	$- 44 - 198$	$- 119 - 187$
$+$	$+$	Spontaneous at high temperature	$N H_{4} C l (s) \to N H_{3} (g) + H C l (g)$ $N_{2} (g) + O_{2} (g) \to 2 N O (g)$	$176180$	$28425$
$+$	$-$	non Spontaneous at all temperature	$3 O_{2} \to 2 O_{3}$ $2 H_{2} O (l) + O_{2} (g) \to 2 H_{2} O_{2} (l)$	$286196$	$- 137 - 126$