Areaction will be spontaneous only at low temperatures if both δh and δs are negative. for a reaction in which δh = −310.1 kj/mol and δs = −89.00 j/k · mol, determine the temperature (in °c) below which the reaction is spontaneous.

3211.12 K

Explanation:

The expression for the standard change in free energy is:

Where,  

is the change in the Gibbs free energy.

T is the absolute temperature. (T in kelvins)

is the enthalpy change of the reaction.

is the change in entropy.

For reaction to be spontaneous,

Given,

So,

Thus, applying values as:-

So, T = 3484.27 K

The conversion of T( °C) to T(K) is shown below:

T( °C)  = T(K) - 273.15  

So,  

T = (3484.27 - 273.15) K = 3211.12 K

The temperature below which the reaction is spontaneous is:- 3211.12 K

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