a What is the rate law for the uncatalyzed reaction? a

a What is the rate law for the uncatalyzed reaction? a. \rm rate={\it k}[Ce^{4+}]^2[Tl^+] b. \rm rate={\it k}[Ce^{4+}][Tl^+] c. \rm rate={\it k}[Ce^{4+}] d. \rm rate={\it k}[Ce^{4+}][Tl^+]^2 e. \rm rate={\it k}[Ce^{4+}]^2[Tl^+]^2 f. \rm rate={\it k}[Tl^+] Part B If the uncatalyzed reaction occurs in a single elementary step, why is it a slow reaction? Check all that apply. Check all that apply. a. The reaction requires the collision of three particles with the correct energy and orientation. b. The probability of an effective three-particle collision is low. c. All reactions that occur in one step are slow. d. The transition state is low in energy. Part C The catalyzed reaction is first order in \rm [Ce^{4+}] and first order in \rm [Mn^{2+}]. Which of the steps in the catalyzed mechanism is rate determining? a. \rm Ce^{4+}(aq)+Mn^{2+}(aq)\rightarrow Ce^{3+}(aq) + Mn^{3+}(aq) b. \rm Ce^{4+}(aq)+Mn^{3+}(aq)\rightarrow Ce^{3+}(aq)+Mn^{4+}(aq) c. \rm Mn^{4+}(aq)+Tl^+(aq)\rightarrow Mn^{2+}(aq)+Tl^{3+}(aq) Based on their available oxidation states, rank the following metals on their ability to catalyze this and other oxidation-reduction reactions. Rank from best to worst catalyst. To rank items as equivalent, overlap them. Manganese , titanium and vanadium