Question

consider the redox reaction below.
ag⁺(aq) + zn(s) → zn²⁺(aq) + ag(s)
balance the zinc half - reaction. how many electrons are transferred?

Explanation:

Step1: Identify the zinc half - reaction

The zinc half - reaction involves the oxidation of Zn(s) to \(Zn^{2 + }(aq)\). The unbalanced half - reaction is \(Zn(s)\to Zn^{2+}(aq)\).

Step2: Balance charge by adding electrons

In the oxidation process, zinc atoms lose electrons. The charge on the left - hand side (Zn(s)) is 0, and the charge on the right - hand side (\(Zn^{2+}(aq)\)) is + 2. To balance the charge, we need to add 2 electrons to the right - hand side (because oxidation is the loss of electrons). The balanced half - reaction is \(Zn(s)\to Zn^{2+}(aq)+2e^-\). So, the number of electrons transferred in the zinc half - reaction is 2.

Answer:

The number of electrons transferred in the zinc half - reaction is 2. The balanced zinc half - reaction is \(Zn(s)\to Zn^{2+}(aq)+2e^-\).