Question

points cach) 7. (ll points Given the reaction coordinate diagram for the reaction of A to form G, answer the follow Cand E B,D,F 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: A or G? e Does A or E form faster from C? f. Which is the more stable intermediate? g. What is the reactant of the rate-determining step h is the first step of the reaction exergonic or endergonic? endergo - Is the overall reaction exergonic or endergonic? exeroon Which step in the forward direction has the largest rate constant? f a Which step in the reverse direction has the smallest rate constant? step a

Answer 1

Progress of reaction » from the giren reaction converted to 'G' through different intermediate profite, we see that different di transition A is state and - The stability of this species can be compaine by the energy associated Coty with them. Higher in energy Unstable lower in energy stable - Transition state & The transition state of a chemical reaction I is a particular configuration along the reaction coordinate It is defined as the state cottuesponding to the highest potential energy along the reaction coordinate. " Here , B, D, f/ are transition state

Intermediate & A reaction intermediale is a species within a multister reaction mechanism that is proncea in the preceding step and consumed in a subsequent p to ultimately generate the final revetim pricdesetan Here species c and E are intermediale I Rate determining step . - In a multistep reaction meachanism, the slowest step is the role determining step. Here cto E is the role determining step I because, formation of c to E requires higher energy then the other step so it is the slowest step.

Answers:

A. 2 intermediates are formed ( C and E)

B. B, D and F represents transition state

C. E to G is the fastest step. ( because lowest energy barrier than the other)

D. Lower in energy more stable is the species. So G is more stable than A

E. Formation of C to E requires higher energy than C to A. So C to A can form easily. Here is a confusion that is if formation C to A is easier than C to E , why reaction proceed forward? Because the reaction is

A  $\rightleftharpoons$ C $\rightleftharpoons$ E $\rightarrow$ G

A to C and C to E is reversible so less amount of C is converted to E but E to G is not reversible and G is the most stable species in the reaction. So all E will converted to G therefore equilibrium shift towards forward direction.

F. Intermediate E is more stable than C

G. Rate determining step is C to E because it is the slowest step. Here C is the reactant of the rate determining step.

H. Formation of A to requires energy because C is in higher energy level than A. So this step is endergonic.

I. G in lower energy level than A. So in this whole reaction energy get realeased. So the reaction is exergonic.

J. Larger the rate constant faster the step. So F to G has largest rate constant.

K. In the reverse direction E to C has the lowest rate constant