Chapter 17: Problem 22

Identify which of the following reactions (as written) is an anodic reaction and which is a cathodic reaction. Write the balanced over- all ionic equation for the redox reaction of the cell. $$\begin{array}{l}{\mathrm{Cd}(s) \rightarrow \mathrm{Cd}^{2+}(a q)+2 e^{-}} \\\ {\mathrm{Ag}^{+}(a q)+e^{-} \rightarrow \mathrm{Ag}(s)}\end{array}$$

Short Answer

Expert verified

The anodic reaction is $Cd(s) \rightarrow Cd^{2+}(aq)+2 e^{-}$, and the cathodic reaction is $Ag^{+}(aq)+e^{-} \rightarrow Ag(s)$. The balanced ionic equation for this cell's redox reaction is $Cd(s) + 2Ag^{+}(aq) \rightarrow Cd^{2+}(aq) + 2Ag(s)$.

Step by step solution

Identify Anodic and Cathodic Reactions

In redox reactions, oxidation and reduction occur concurrently. The oxidation reaction, also known as the anodic reaction, is where a compound loses electrons. Conversely, the reduction reaction, also referred to as the cathodic reaction, is where a compound gains electrons. Thus, here Cadmium (Cd) is oxidized from Cd(solid) to Cd2+(aqueous) by losing 2 electrons, making it the anode. Similarly, Silver ion (Ag+) is reduced to Ag(solid) by gaining one electron, making it the cathode.

Balance the Ionic Equation

To form the overall equation, combine the anodic and cathodic reactions. Here, the number of electrons in both reactions must be identical. The reaction with fewer electrons should be multiplied by a factor to balance the electrons. Here, the silver reaction has only 1 electron compared to cadmium's 2 electrons, so multiply the silver reaction by 2. Hence, the balanced over-all ionic equation would be $Cd(s) + 2Ag^{+}(aq) \rightarrow Cd^{2+}(aq) + 2Ag(s)$.

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Short Answer

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Identify Anodic and Cathodic Reactions

Balance the Ionic Equation

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