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?

Question

Chemistry

Beckett Delacruz

3 February, 04:13

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?

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Answers (2)

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Kaeden Norton · Answer 1

Rate law for the uncatalyzed reaction:

Rate = k[Ce^4+]^2[Tl]

Explanation: rate law shows the mathematical relationship by comparing the rate of reaction with the reactants concentration.

Rate law = k[reactantA][reactantB].

Rate law can be used to derive an equation that shows a reactant as a function of time. Also, it can be use to calculate the rate of reaction from known concentration.

Natalia Meyers · Answer 2

Rate of reaction = k [Ce^3+]^2 [Tl^3+]

Explanation:

Since the reaction is thought to occur in a single reaction step for the uncatalysed reaction, and the reaction equation is: 2Ce4 + (aq) + Tl + (aq) →2Ce3 + (aq) + Tl3 + (aq)

Rate of reaction = k [Ce^3+]^2 [Tl^3+]

Note that the rate of reaction = rate of appearance of products or rate of disappearance of reactants as shown above.