Table of Selected Standard Reduction Potentials at 25 C Cu Cu Reduction half-reaction Stadard Reduction Potential Cu" (aq) + 2 e' → Cu (s) E#2 0.342 V Fe2+ (aq) + 2e. Write the overall redox reaction that would take place in the battery above. Identify the cathode and the anode for this battery, and calculate the value of E°cel ii. Which pair of half reactions would make the battery with the largest E oll ii. Consider the following set of half reactions. Make sure the half-reactions are balanced for electrons, so that the number of electrons in each half reaction is the same before you add the half-reactions together 5. Write the oxidation half-reaction, the reduction half-reaction and the overall redox reaction taking place. What is the calculated value of Ecell for this battery (show your calculation)? ii. Which half-reaction should be used as the cathode, and which should be used as the anode? ii. Use the reduction half-reactions and standard reduction potentials below to answer the following questions 4. To set up this reaction as a battery, you need to separate the half-reactions between a cathode and an anode. Explain your answer Will the reducing agent be at the anode or the cathode? In exercise 6, you put a piece of aluminum foil (Al) in a solution of Cu2 (aq) and watched a redox reaction take place. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is separated from the reducing agent. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair the measured cell potential, and the calculated E°cel 3. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair the measured cell potential, and the calculated E 2.
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