Citrate synthase catalyzes the reaction: + − → + − the standard free energy change for the reaction is −31.5 ∙ −1. calculate the equilibrium constant for this reaction at 37℃.

The given question is incomplete. The complete question is as follows.

Citrate synthase catalyzes the reaction

Oxaloacetate + acetyl-CoA citrate + HS-CoA

The standard free energy change for the reaction is -31.5 kJ*mol^-1

( a) Calculate the equilibrium constant for this reaction a 37degrees C

Explanation:

(a).  It is known that , relation between change in free energy () of a reaction and equilibrium constant (K) is as follows.

where,  T = temperature in Kelvin

The given data is as follows.

         T = 310 K,        (as 1 kJ = 1000 J)

Now, putting the given values into the above formula as follows.

     ln K =

            =

      ln K = 12.22

         K = antilog (12.22)

           =

Therefore, we can conclude that value of equilibrium constant for the given reaction is .

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.