1.The voltaic cell x(s) | x2+(1.0 M) || Cu2+(1.0 M) | Cu(s) was constructed and its cell potential was measured as 1.97 V.

a. Calculate the half-cell potential for x.

b. Calculate the potential of the cell that will be formed by combining the unknown half-cell with a nickel half-cell, under standard conditions.

2. A voltaic cell was constructed using the half-cell Cr(s) | Cr3+(0.20 M) as the anode and the half-cell Sn2+(x M) | Sn(s) as the cathode; the measured cell voltage was 0.56 V. Calculate x, the molarity of Sn2+ in the cathode.

3. Chemical energy storage is big business and possibly one of the most important technological advances society could make (storing energy is MUCH harder than making it)! Based on the information in table 1 what two materials would you use to create a high potential battery?

a. Write the half-reaction for your anode and your cathode, Explain your choice for each

b. Calculate the E˚cell for your choice

c. Explain why sodium is a perfect example of a material that is theoretically a good choice but does not work in the real world.

4. Compare table 1 (the standard reduction potentials) to the periodic trends from last quarter (radius, Ionization energy, electron affinity, electronegativity). Do the potentials in the table agree with our periodic trends? Why/why not (use at least two examples in your argument)?

Answer rating: 100% (QA)

a Calculate the halfcell potential for x The halfcell potential for x can be calculated using the Nernst equation E E RTnFlnQ E 197 V E 0 V R 8314 JmolK T 298 K n 2 F 96485 Cmol Q Cu2x2 197 0 8314 Jmo... View the full answer