For the pair of species given: Lithium (E° = -3.05 V) and silver (E° = 0.80...

For the pair of species given:
1. Lithium (E° = -3.05 V) and silver (E° = 0.80 V)
2. Aluminum (E° = -1.66 V) and zinc (E° = -0.76 V)
  1. Write balanced half-reactions and the overall spontaneous reaction.
  2. Diagram the cell. Be a specific as possible including labeling electrodes with their charges and names (anode and cathode), showing the direction of electron flow in the circuit and showing the direction of cation and anion flow in the salt bridge.
  3. Calculate the cell potential for the overall reaction.
  4. Calculate the Gibbs free energy for the overall reaction.
  5. Write the standard cell notation for the overall reaction.
  6. Calculate K_eq for the spontaneous reaction.

Expert Solution

Greater is the standard reduction potential of the metal electrode reduction takes place on that electrode. While lower is Standard reduction potential, higher will be its standard oxidation potential, thus oxidation takes place on that electrode.

a. Oxidation of Li takes place on anode . While Reduction of Ag+ takes place on cathode.

Cell potential = E° cathode - E° anode

The Gibbs free energy = - n F E° cell

The equilibrium constant = Keq

Log(keq) = 16.92 n E° cell

Or delta G = - 2.303 n R T log(Keq)

For detailed work, please refer to the images.

queen_honey_blossom answered 3 years ago

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