Question

Metals often form several cations with different charges. Cerium, for example, forms Ce3+ and Ce4+ ions, and thallium forms Tl+ and Tl3+ ions. Cerium and thallium ions react as follows:

2Ce4+(aq)+Tl+(aq)→2Ce3+(aq)+Tl3+(aq)

This reaction is very slow and is thought to occur in a single elementary step. The reaction is catalyzed by the addition of Mn2+(aq) according to the following mechanism:

Ce4+(aq)+Mn2+(aq)Ce4+(aq)+Mn3+(aq)Mn4+(aq)+Tl+(aq)→→ →Ce3+(aq)+Mn3+(aq)Ce3+(aq)+Mn4+(aq)Mn2+(aq)+Tl3+(aq)

Part A

What is the rate law for the uncatalyzed reaction?

What is the rate law for the uncatalyzed reaction?

	rate=k[Ce4+]2[Tl+]2
	rate=k[Ce4+][Tl+]
	rate=k[Ce4+]
	rate=k[Tl+]
	rate=k[Ce4+]2[Tl+]
	rate=k[Ce4+][Tl+]2 If the uncatalyzed reaction occurs in a single elementary step, why is it a slow reaction? Check all that apply. Check all that apply. All reactions that occur in one step are slow. The reaction requires the collision of three particles with the correct energy and orientation. The probability of an effective three-particle collision is low. The transition state is low in energy. The catalyzed reaction is first order in [Ce4+] and first order in [Mn2+]. Which of the steps in the catalyzed mechanism is rate determining? The catalyzed reaction is first order in  and first order in . Which of the steps in the catalyzed mechanism is rate determining? Ce4+(aq)+Mn2+(aq)→Ce3+(aq)+Mn3+(aq) Ce4+(aq)+Mn3+(aq)→Ce3+(aq)+Mn4+(aq) Mn4+(aq)+Tl+(aq)→Mn2+(aq)+Tl3+(aq)

Answer 1