Which one is being oxidized and which one is being reduced?
In an electrochemical cell, the potential difference between two electrodes under standard conditions is known as the standard cell potential (E degree_cell). The standard cell potential can be used to identify the overall tendency of a redox reaction to occur spontaneously. The spontaneity of a reaction is identified using the Gibbs free energy Delta G degree, Delta G degree is related to E degree_cell. E degree_cell and Delta G degree are also related to equilibrium constant K_eq of the reaction. Select the image to explore the activity that shows how E degree_cell, K_eq, and Delta G degree are related to each other. In the activity, you should see a triangle, whose three vertices represent K_eq, E degree_cell, and Delta G degree. You can select two vertices and determine the relation between them. You can then reset the activity and select the next two quantities. The following values may be useful when solving this tutorial. In the activity, click on the E degree_cell and K_eq quantities to observe how they are related. Use this relation to calculate K_eq for the following redox reaction that occurs In an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the cell are Cu^2+ (aq) + 2e^- + Cu(s) and Ni(s) rightarrow Ni^2+ (aq) + 2e^- The net reaction is Cu^2+ (aq) + Ni(s) rightarrow Cu(s) + Ni^2+ (aq) Use the given standard reduction potentials in your calculation as appropriate. Express your answer numerically to three significant figures.
