consider the redox reaction below.\nag⁺(aq) + zn(s) → zn²⁺(aq) + ag(s)\nbalance the zinc half - reaction…

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^-).