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Sandmeyer Reaction

For a reactio...

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For a reaction, A +B ➡️C. ∆H = 30kJ/mol and ∆S = 60 J/K/mol. The temperature,above which reaction will be spontaneous is

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Q. The value of

Δ H

Δ S

for a reaction are respectively

30 k J

{m o l}^{- 1}

100 J K^{- 1}

{m o l}^{- 1}

. Then temperature above which the reaction will become spontaneous is:

Q. For a reaction at 298k A+B gives u C+D : ∆H = -10kJ/mol, ∆S = -33.3kJ/mol. At what temperature will be the reaction become spontaneous in the forward direction ?

Q. For a reaction,

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

at what temperature, the reaction will be spontaneous?

Q. For a given reaction,

Δ H = 35.5 k J m o l^{- 1} a n d Δ S = 83.6 J K^{- 1} m o l^{- 1}

. The reaction is spontaneous at (Assume that

Δ H a n d Δ S

do not vary with temperature.)

Q. For the reaction at 298 K, 2A+B

\to C

△

m o l^{- 1}

△

K^{- 1}

m o l^{- 1}

At what temperature will the reaction become spontaneous considering

△

△

S to be constant over the temperature range?

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Sandmeyer Reaction

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