Exercise 2: Write the schematic representation and reaction of the cell composed of SHE and cadmium electrode. Deduce the half-reaction potential of the cadmium electrode from the E°cell = - 0.403 V. Is the reaction spontaneous or not? Why or why not? If it is not spontaneous, how should the schematic representation be written to make it spontaneous? The magnitude of electrode potentials indicates the relative strength of the ionic species as electron acceptors (oxidizing agents); that is in decreasing strength, Ag* > H* > Cd²* > Zn2*.

What's More Activity 3.3.2. Solve me! Calculate the problem using Nernst equation. Show your solution. Problem: In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn | Zn2+ half-cell and an H2 | H* half-cell under the following conditions: [Zn2+] = 0.010 M [H*] = 2.5 M PH2 = 0.30 atm Calculate Ecell at 298.15 K.

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b. A cell constructed with a Fe|Fe2+ half-cell and a Pb|Pb2+ half cell 1. Determine E°cell (V) NG Info NG 1 2. Write the net ionic equation for the cell. Info Vork Problem 3. Identify the half-cell at the cathode (enter a number 1- 4) 1. Fe2+, (aq) + 2 e → Fe°(s) 2. Fe°(s) → Fe2+ 3. РЬ2+ + 2 e NG (aq) + 2 e → Pb°, Info (s) + 2 e (aq) 4. Pb° > Pb²+, (s) (aq)