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Consider the following reaction: Cd (s) AgCl (aq) --> CdCl2 (aq) Ag (s) In this reaction, a. electrons are transferred from silver in AgCl (aq) to Cd (s) b. electrons are transferred from Cd (s) to silver in AgCl (aq) c. no electrons are transferred since the oxidation number of chlorine atoms does not change d. the oxidizing agent is Cd (s) e. the reducing agent is AgCl (aq)

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Answer:

a. electrons are transferred from silver in AgCl (aq) to Cd (s)

Explanation:

In this reaction Ag is reduced:

  • Ag⁺ + 1e⁻ → Ag⁰

While Cd is oxidized:

  • Cd⁰ → Cd⁺² + 2e⁻

With those two semi-reactions we can see that there's a transfer of electrons from silver in AgCl(aq) to the solid cadmium.

For the record, given that Ag was reduced, Cd was the reducing agent. And because Cd was reduced, Ag was the oxidizing agent.

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