QUESTION THREE (a) (i) Predict the intermediate and products of the following reaction. -CH3 RCN/ PMe3 Rh Me P H (ii) Identify the mechanism/s of this reaction. (iii) Describe fully, the mechanism of this reaction. (b) (i) State the principle of microscopic reversibility. (ii) Explain the use of principle of microscopic reversibility.

The activation energy for the isomerization reaction ofCH3NC in Problem 14 is 161 kJ mol-1, and the reactionrate constant at 600 K is 0.41 s-1.(a) Calculate the Arrhenius factor A for this reaction.(b) Calculate the rate constant for this reaction at 1000 K.

5 Br-(aq) + BrO3-(aq) + 6 H+(aq)--> 3 Br2(aq) + 3 H2O(l);          (a) write the expressions of the reaction rates mathematically in terms of                 (i) the disappearance of Br- (Reactant);                  (ii) the disappearance of BrO3- (Reactant), and                 (iii) the formation of Br2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)

The overall reactions A --> D occurs via the following mechanism with the given reaction energies and barriers for each step  Assume that a single step controls the rate of the reaction and that any steps preceding the rate-determining step can be considered quasi-equilibrium. What are the values for apparent activation barriers you would measure for the following.   i) Step 1 is the rate-determining step.   ii) Step 2 is the rate-determining step.