Elementary thermodynamics How does change delta G in a catalyzed reaction relati

Question

Elementary thermodynamics How does change delta G in a catalyzed reaction relative to an uncatazlyzed reaction? How does change the equilibrium constant K of a catalyzed reaction relative to an uncatalyzed reaction? If the reaction A rightarrow B has an equilibrium constant K = 1 and the reaction B rightarrow C has K = 10 what will happen to [A] if now we couple the reactions in the sequence A rightarrow B rightarrow C? If delta G for the reaction A rightarrow B is 20 Kcal/mol, what should be the delta G value of the reaction C rightarrow D for the catalyzed reaction A + C + Enzyme rightarrow B + D + Enzyme to happen? How do the standard free energy change delta G degree and the equilibrium constant K relate to each other in the reaction A rightarrow B?

Explanation / Answer

the presen cf catalyst influences the activation energy and nothing to do with the gibbs free energy change. since gibbs free energy is a state function and independent of the path taken. Activation energy changes the path through which the reaction takes place. Hence gibbs free energy change remains constant

since deltaG= -RTlnK, equilibrium constant is also not going to get effected.

3. for A---B, K1= [B]/[A = 1 and for B--->C, K2= [C]/[B] =10

K1*K2= [B]/[A] * [C]/[B] =10, [C]/[A]= 10

there will be less and A and more C. what ever A is reacted to B, B has decomposed to C ( because of high K value).

d) deltaG remains same as gibbs free energy change is independent of presence of catalyst.

e) deltaG=-RTlnK, ln K= -20/(1.987*298) =-0.033, K= 0.97

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