° Half-Reaction E ° (V) Ag + (aq) + e Ag (s) 0.7996 Al 3+ (aq) + 3e Al (s) 1.676

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Half-Reaction E

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(V) Ag+ (aq) + e Ag (s)   0.7996 Al3+ (aq) + 3e Al (s) 1.676 Au+ (aq) + e Au (s)   1.692 Au3+ (aq) + 3e Au (s)   1.498 Ba2+ (aq) + 2e Ba (s) 2.912 Br2 (l) + 2e 2Br (aq)   1.066 Ca2+ (aq) + 2e Ca (s) 2.868 Cl2 (g) + 2e 2Cl (aq)   1.35827 Co2+ (aq) + 2e Co (s) 0.28 Co3+ (aq) + e Co2+ (aq)   1.92 Cr2+ (aq) + 2e Cr (s) 0.913 Cr3+ (aq) + 3e Cr (s) 0.744 Cr3+ (aq) + e Cr2+ (aq) 0.407 CrO42 (aq) + 4H2O (l) + 3e Cr(OH)3 (s) + 5OH (aq) 0.13 Cu2+ (aq) + 2e Cu (s)   0.3419 Cu2+ (aq) + e Cu+ (aq)   0.153 Cu+ (aq) + e Cu (s)   0.521 F2 (g) + 2e 2F (aq)   2.866 Fe2+ (aq) + 2e Fe (s) 0.447 Fe3+ (aq) + e Fe2+ (aq)   0.771 Fe3+ (aq) + 3e Fe (s) 0.037 2H+ (aq) + 2e H2 (g)   0.000 2H2O (l) + 2e H2 (g) + 2OH (aq) 0.8277 H2O2 (aq) + 2H+ (aq) + 2e 2H2O (l)   1.776 I2 (s) + 2e 2I (aq)   0.5355 2IO3 (aq) + 12H+ (aq) + 10e I2 (s) + 6H2O (l)   1.195 Mg2+ (aq) + 2e Mg (s) 2.372 Mn2+ (aq) + 2e Mn (s) 1.185 MnO2 (s) + 4H+ (aq) + 2e Mn2+ (aq) + 2H2O (l)   1.224 MnO4 (aq) + 8H+ (aq) + 5e Mn2+ (aq) + 4H2O (l)   1.507 MnO4 (aq) + 2H2O (l) + 3e MnO2 (s) + 4OH (aq)   0.595 HNO2 (aq) + H+ (aq) + e NO (g) + H2O (l)   0.983 N2 (g) + 4H2O (l) + 4e 4OH (aq) + N2H4 (aq) 1.16 NO3 (aq) + 4H+ (aq) + 3e NO (g) + 2H2O (l)   0.957 Na+ (aq) + e Na (s) 2.71 Ni2+ (aq) + 2e Ni (s) 0.257 O2 (g) + 4H+ (aq) + 4e 2H2O (l)   1.229 O2 (g) + 2H2O (l) + 4e 4OH (aq)   0.401 O2 (g) + 2H+ (aq) + 2e H2O2 (aq)   0.695 Pb2+ (aq) + 2e Pb (s) 0.1262 PbSO4 (s) + H+ (aq) + 2e Pb (s) + HSO4 (aq) 0.3588 HSO4 (aq) + 3H+ (aq) + 2e H2SO3 (aq) + H2O (l)   0.172 Sc3+ (aq) + 3e Sc (s) 2.077 Sn2+ (aq) + 2e Sn (s) 0.1375 Sn4+ (aq) + 2e Sn2+ (aq)   0.151 VO2+ (aq) + 2H+ (aq) + e VO2+ (aq) + H2O (l)   0.991 Zn2+ (aq) + 2e Zn (s) 0.7618 A certain half-reaction has a standard reduction potential-0.77 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.60 V of electrical power. The cell will operate under standard conditions Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell c O yes, there is a minimum an have? red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? O yes, there is a maximum red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box no maximim By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell 0 Note: write the half reaction as it would actually occur at the anode

Explanation / Answer

We know that,

E0cell = E0cathode - E0anode   (Formula 1)

The engineer requires overall cell potential atleast 0.60 V of electrical power.

So, let consider E0cell = 0.60 V

Given that, E0cathode = -0.77 V

Apply the data in formula 1,

0.60 V = -0.77 V - E0anode

E0anode = -1.33 V

Standard oxidation potential = -1.33 V

i.e Standard reduction potential = 1.33 V

1. As engineer requires atleast 0.60 V from the cell,

the standard reduction potential must be minimum 1.33 V.

2. As engineer requires atleast 0.60 V from the cell, the cell potential can be more than 0.60 V also.

i.e there is no maximum potential,

when the standard reduction potential more than 1.33 V, the cell potential also will more than 0.60 V.

3. To acheive the minimum cell potential, the following half cells could be used as anode,

Au+ (aq) + e Au (s) E0 = 1.692 V

Au3+ (aq) + 3e Au (s) E0 = 1.498 V

Cl2 (g) + 2e 2Cl (aq) E0 = 1.35827 V

F2 (g) + 2e 2F (aq)   E0 = 2.866 V

MnO4 (aq) + 8H+ (aq) + 5e Mn2+ (aq) + 4H2O (l)   E0 = 1.507 V

H2O2 (aq) + 2H+ (aq) + 2e 2H2O (l) E0 = 1.776 V

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