The conversion of (CH3)3CI to (CH3)2C=CH2 can occur by either one-step or two-step mechanism, as shown in
Equations (1) and (2]
[1]
있
+ I + H₂O
HK
OH
[2]
07
Slow
+ H₂O
+ I
f) Assume Equation [a] represents an endothermic reaction
and that the product of the rate determining step is
higher in energy than the reactants or products.
Draw an energy dagram for this two-step reaction.
Label the axes, reactants and products for each step,
and the Ea and 4to for each step. Label 44° overall.
Draw the structure for both transition states.

See explanation

Explanation:

a) The rate equation for the mechanism in equation 1 is [(CH3)3CCI] [OH^-]

b) The rate equation for the mechanism in equation 2 is [(CH3)3CCI]

c) The first equation is second order while the first equation is first order.

d) The rate equation shows the species  that are involved in the rate determining step. Hence by manipulating the concentration of the species that appear in each rate equation, we can exactly know which of the rate equations represents the actual mechanism of the reaction.

e) The diagram required is shown in the image attached to this answer.

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.