a. Draw a diagram of an electrochemical cell consisting of a Cr³⁺/Cr half-cell and a Cl₂/Cl^– half-cell.

b. Use the data in Appendix 2 to calculate the cell voltage.

c. Which half-cell is the positive pole?

Transcribed Image Text:

Selected standard electrode potentials Electrode reaction Electrode reactlon Ag* +e- Ag Mn2+ + 2e- Mn +0.80 -1.18 Br, + 2e= 2Br +1.07 Mno, + 8H* + 5e- Mn2+ + 4H,0 +1.52 Ca2+ + 2e Ca -2.87 Ni2+ + 2e Ni - 0.25 Cl, + 2e 2CI- NO,-+ 2H+ +e - NO, + H,0 +0.81 +1.36 CIO- + H,0 + 2e Cl+ 20H NO, + 10H* + 8e- NH,+3H,0 +0.89 +0.87 Cr2+ + 2e Cr -0.91 0, + 4H* + 4e= 2H,0 +1.23 Cr3+ + 3e Cr 0, + 2H,0 + 4e 40H- -0.74 +0.40 Cr,0,2-+14H* + 6e- 2Cr+ + 7H,0 Pb2* + 2e Pb +1.33 -0.13 Cut + e- Cu Pbo, +4H* + 2e= Pb2+ + 2H,o +0.52 +1.47 Cu* + e= Cut +0.15 Sn2+ + 2e Sn -0.14 Cu2+ + 2e Cu +0.34 Sn+ + 2e Sn2+ +0.15 F, + 2e 2F so, + 4H* + 2e so, + 2H,0 +2.87 +0.17 Fe2+ + 2e Fe -0.44 S,0,-+ 2e= 250,2 +2.01 Fe3+ + e Fe2+ s,0, +2e= 25,0, +0.77 +0.09 Fe+ + 3e= Fe -0.04 V2+ + 2e- V -1.20 2H* + 2e H, V3+ + e- V2+ 0.00 -0.26 2H,0 + 2e= H, +20H- VO2+ + 2H* +e = V3+ + H,0 +0.34 -0.83 H,0, + 2H* + 2e 2H,0 vo,* + 2H* +e vo2* + H,0 +1.00 +1.77 I, + 2e 21- Vo,-+ 4H* + e e VO2+ + 2H,0 +0.54 +1.00 K* +e=K -2.92 Zn2+ + 2e Zn -0.76 Mg+ + 2e- Mg -2.38