Question

Given the reaction coordinate diagram for the reaction of A to form G, answer the following questions:

a. How many intermediates are formed in the reaction?

b. Which letters represent transition states?

c. What is the fastest step in the reaction?

d. Which is more stable,AorG?

e. DoesAorEform faster fromC?

f. What is the reactant of the rate-determining step?

g. Is the first step of the reaction exergonic or endergonic?

h. Is the overall reaction exergonic or endergonic?

i. Which is the more stable intermediate?

j. Which step in the forward direction has the largest rate constant?

k. Which step in the reverse direction has the smallest rate constant?

Short answer

a) Two intermediates are formed in the reaction.

b) B,D,F represent transition states.

c) E to G the smallest activation energy so fastest will be the reaction.

d) G will be most stable.

e) A will form faster from C.

f) C will be reactant of the rate determining step.

g) First step of the reaction is endergonic.

h) Overall reaction is exergonic.

i) C is the most stable intermediate.

j) E to G has the largest rate constant as here lowest activation energy.

k) G to E has the smallest rate constant as here highest activation energy in reverse direction.

Step-by-step solution

Some definition

Intermediate state= It is the product of one reaction and reactant for other reaction. In graph dip of the graph shows intermediate states. C and E is the intermediates states.

Transition state= The state corresponding to highest potential energy along the reaction coordinate. In graph tip of the graph shows transition states. B,D,F represent transition states.

Activation energy= The difference between molecules having kinetic energy and threshold energy is called activation energy. Which has more activation energy that will be the slow step hence rate determining step.

Exergonic= When heat evolove during the reaction. When product has less free energy than reactant then it is exergonic reaction.

Endergonic= When heat consumed during the reaction. When product has more free energy than reactant then it is endergonic reaction.

Step 3:Final answer

a) Two intermediates are formed in the reaction. In graph dip of the graph shows intermediate states. C and E is the intermediates states.

b) B,D,F represent transition states. In graph tip of the graph shows transition states.

c) E to G the smallest activation energy so fastest will be the reaction. Which has more activation energy that will be the slow step hence rate determining step.

d) G will be most stable as it has less free energy.

e) A will form faster from C due to less activation energy.

f) C will be reactant of the rate determining step because it has more activation energy. Which has more activation energy that will be the slow step hence rate determining step.

g) First step of the reaction is endergonic. When product has more free energy than reactant then it is endergonic reaction.

h) Overall reaction is exergonic. When product has less free energy than reactant then it is exergonic reaction.

i) C is the most stable intermediate because it has less free energy than E.

j) E to G has the largest rate constant as here lowest activation energy.

k) G to E has the smallest rate constant as here highest activation energy in reverse direction.