Question

1. the strongest oxidizing agent in the equations given above is

a. ce³⁺(aq)
b. ce⁴⁺(aq)
c. cd²⁺(aq)
d. in³⁺(aq)

equations of redox reactions
i. 2ce⁴⁺(aq) + pd(s) → 2ce³⁺(aq) + pd²⁺(aq)
ii. pd²⁺(aq) + 2in³⁺(aq) → pd(s) + 2in³⁺(aq)
iii. cd²⁺(aq) + pd(s) → no reaction
iv. in³⁺(aq) + cd(s) → no reaction
use the following information to answer the next question.

Explanation:

Step1: Recall redox - reaction concept

In a redox reaction, a stronger oxidizing agent will oxidize a reducing agent. An oxidizing agent is reduced (gains electrons) in the reaction.

Step2: Analyze each reaction

In reaction I: \(2Ce^{4 +}(aq)+Pd(s)\to2Ce^{3+}(aq)+Pd^{2+}(aq)\), \(Ce^{4+}\) is reduced to \(Ce^{3+}\), so \(Ce^{4+}\) is an oxidizing agent. In reaction II: \(Pd^{2+}(aq)+2In^{3+}(aq)\to Pd(s)+2In^{2+}(aq)\), \(Pd^{2+}\) is reduced to \(Pd\), so \(Pd^{2+}\) is an oxidizing agent. In reaction III: \(Cd^{2+}(aq)+Pd(s)\to\) no reaction, \(Cd^{2+}\) cannot oxidize \(Pd\). In reaction IV: \(In^{3+}(aq)+Cd(s)\to\) no reaction, \(In^{3+}\) cannot oxidize \(Cd\).

Step3: Compare oxidizing - agent strength

Since \(Ce^{4+}\) can oxidize \(Pd\) (reaction I) and \(Pd^{2+}\) can oxidize \(In^{3+}\) (reaction II), and \(Cd^{2+}\) and \(In^{3+}\) show no - reaction with other species in the given reactions, the strongest oxidizing agent is \(Ce^{4+}(aq)\).

Answer:

B. \(Ce^{4+}(aq)\)