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

Δ H < 0 a n d Δ S = 0

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Δ H = 0 a n d Δ S < 0

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Δ H < 0 a n d Δ S > 0

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Δ H < 0 a n d Δ S < 0

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Solution

The correct option is C $Δ H < 0 a n d Δ S > 0$
The correct thermodynamic conditions for the spontaneous reaction at all temperature is

$Δ H < 0 a n d Δ S > 0$

Under conditions, $Δ G = Δ H - T Δ S < 0$

The correct thermodynamic conditions for the spontaneous reaction at all temperatures is
$Δ H < 0 a n d Δ S > 0$

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 process to be spontaneous at all conditions of temperature, which of the following is correct?

T

P

△ H = + 29 k J m o l^{- 1}; △ S = - 35 J K^{- 1} m o l^{- 1}

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