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

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.