Can I please get help with questions D, E, and F please Week 4 Lab: Rationalizing Reactive Pathways1. Answer the following questions on the reaction coordinate diagram pictured below.Reaction Progressa. Label AG on the diagram above.b. Label the reactants, products, transition state(s), and intermediate(s).c. How many steps would the mechanism of this reaction have?d. Label the activation energy for each step on the diagram above.e. Would you expect the equilibrium constant for the reaction above to be greater than 1, less than 1, orequal to 1?f. Would you expect the rate-determining step to have an early or a late transition state?

Given reaction coordinate diagram is,(D) To label the activation energy for each step on the diagram above Activation energy is defined as the extra amount of energy that must be given to molecule to activate the molecule, so that it can reach at the transition state and make then transform into the product. In the given diagram there are two steps, activation energy for first step is labeled by A1 and for second step is labeled by A2.(E) Equilibrium constant of the reaction and change in free energy are proportional to each other as shown by below equation. ΔG˚ = -RT ln Keq Since energy or product is greater than reactant therefore ΔG˚rxn for the reaction is positive and therefore Keq is less than 1. Answer: Less than 1(F) Rate of a reaction is related to the activation energy. Greater the activation energy, the slower will be the reaction. In the given reaction, early transition state has higher activation energy as compare to the late transition state therefore the first step of reaction is slower and hence it is rate-determining step of the reaction. Answer: Early transition state