Salt bridge Cr(s) electrode Cu(s) electrode 1.0 M...

salt bridge Cr(s) electrode Cu(s) electrode 1.0 M Cr3+(aq) 1.0 M Cu2+(aq) A electrolytic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a power supply. One electrode compartment consists of a chromium strip placed in a 1.0 M CrCl3 solution, and the other has a copper strip placed in a 1.0 M CuSO4 solution. The overall cell reaction is: 2 Cr3+(aq) + 3 Cu(s) ? 2 Cr(s) + 3 Cu2+(aq) (a) Fill in the information necessary to complete the half reactions that occur in the two electrode compartments. Use the lowest-possible whole-number coefficients. To input an ion surround the ion's element symbol with square brackets and put the ion's charge to the right like this: Al3+ = [Al]3+ (not [Al]+3), and Li+ = [Li]+ (not [Li]1+ or [Li]+1). Do not use brackets for neutral species. Anode half reaction: Cr (s) ? [Cr]3+ (aq) + 3 e- Cathode half reaction: [Cu]2+ (aq) + 2 e- ? Cu (s)

Thanks for your feedback!

(b) Figure out which electrode is the anode, which is the cathode, the signs on these electrodes, the direction in which the electrons flow through the power supply, and the direction in which cations and anions migrate through the salt bridge and solutions. Use this work to pick all of the statements from below which are true. Electrons flow from the chromium electrode to the copper electrode through the power supply. The chromium electrode is the anode and the copper electrode is the cathode. The copper electrode is positive and the chromium electrode is negative. Anions migrate from the 1.0 M CrCl3 solution through the salt bridge to the 1.0 M CuSO4 solution. The copper electrode is the anode and the chromium electrode is the cathode. Anions migrate from the 1.0 M CuSO4 solution through the salt bridge to the 1.0 M CrCl3 solution. Cations migrate from the 1.0 M CuSO4 solution through the salt bridge to the 1.0 M CrCl3 solution. Electrons flow from the copper electrode to the chromium electrode through the power supply. The chromium electrode is positive and the copper electrode is negative. Cations migrate from the 1.0 M CrCl3 solution through the salt bridge to the 1.0 M CuSO4 solution. Cr(s) electrode Cu(s) electrode 1.0 M Cr3+(aq) 1.0 M Cu2+(aq) An electrolytic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a power supply. One electrode compartment consists of a chromium strip placed in a 1.0 M CrCl3 solution, and the other has a copper strip placed in a 1.0 M CuSO4 solution. The overall cell reaction is: 2 Cr3+(aq) + 3 Cu(s) = 2 Cr(s) + 3 Cu2+(aq) Write the half reactions that occur in the two electrode compartments. Use the square brackets to complete the symbol and put the possible whole number coefficients. To input an ion, surround the ion's element with brackets. For example, [Al]3+ (not [Al]+3) or [Li]+ (not [Li]1+ or [Li]+1). Do not use brackets for neutral species. Anode half reaction: Cr(s) -> [Cr]3+(aq) Cathode half reaction: [Cu]2+(aq) -> Cu(s)

Play audio

Feedback

Question

Please give Ace some feedback