BackDraw a reaction coordinate diagram for a two-step reaction in which the first step is endergonic, the second step is exergonic, and the overall reaction is endergonic. Label the reactants, products, intermediates, and transition states.
Draw a reaction coordinate diagram for a one step reaction that has the following values of Ea and ∆H. (c) Ea = 5 kcal/mol; ∆H° = 0 kcal/mol
a. Which step in the reaction coordinate diagram shown here has the greatest free energy of activation in the forward direction?
b. Is the first-formed intermediate more apt to revert to reactants or go on to form products?
c. Which step is the rate-determining step of the reaction?
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When ethyl bromide is added to potassium tert-butoxide, the product is ethyl tert-butyl ether.
CH3CH2–Br + (CH3)3C–O–K+ → (CH3)3C–O–CH2CH3 ethyl bromide potassium tert-butoxide ethyl tert-butyl ether
b. What happens to the rate if the concentration of potassium tert-butoxide is tripled and the concentration of ethyl bromide is doubled?
c. What happens to the rate if the temperature is raised?
Given that A is more stable than B, draw a reaction coordinate diagram that rationalizes the fact that A forms more quickly than B in the following reaction.
Parts (a)–(f) of this assessment refer to the rotation around the single bond of ethane.
(a) Given that the rate of the reaction is independent of concentration, fill in the missing rates in the following table.
Given that step 1 of the following reaction is rate determining, write the rate law for the overall reaction.
Draw a reaction coordinate diagram for the reaction. (Hint: An alkyl halide is more stable than an alkene.)
Draw the reaction-energy diagram for the following reverse reaction:
•CH3 + HCl → CH4 + Cl•
The rate constant for the uncatalyzed reaction of two molecules of glycine ethyl ester to form glycylglycine ethyl ester is 0.6 M-1 s-1. In the presence of Co2+, the rate constant is 1.5 × 106 M-1 s-1. What rate enhancement does the catalyst provide?
Given the following rate data, how many molecules are in the rate-determining step of this reaction?
All things being equal, would you expect a first-order reaction to be faster or slower than a second-order reaction?
Draw a reaction-energy diagram for the propagation steps of the free-radical addition of HBr to isobutylene. Draw curves representing the reactions leading to both the Markovnikov and the anti-Markovnikov products. Compare the values of ∆Gº and Ea and for the rate-limiting steps, and explain why only one of these products is observed.
The rate of the reaction of methyl chloride with hydroxide ion is linearly dependent on both the concentration of methyl chloride and the concentration hydroxide ion. At 30 °C, the constant (k) for the reaction is 1.0 × 10-5 M-1 s-1
b. If the concentration of methyl chloride is decreased to 0.010 M, what will be the effect on
1. the rate of the reaction?
2. the rate constant for the reaction?