The correct thermodynamic conditions for the spontaneous reaction at all temperatures is : (a) ∆H<0 and ∆S < 0 (b) ∆H < 0 and ∆S <0 (c) ∆H <0 and ∆S = 0 (d) ∆H >0 and ∆S < 0 Reaction is spontaneous when ∆S is positive and ∆H is negative

Open in App

Solution

Suggest Corrections

Similar questions

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g)

- 0.094 k J m o l^{- 1} K^{- 1} .

C O_{2}

C O

- 394.4 a n d - 137.2 k J m o l^{- 1}

Δ H^{0}

Δ S^{0}

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

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

Δ_{s y s} G = Δ_{s y s} H - T Δ_{s y s} S

Δ_{s y s} G < 0 (s p o n t a n e o u s)

Δ_{s y s} G = 0 (e q u i l i b r i u m)

Δ_{s y s} G > 0 (n o n - s p o n t a n e o u s)

Δ H

Δ S

Join BYJU'S Learning Program