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The standard cell potential (Eocell) of the zinc-air battery is 1.65V. If at 25.0oC the partial pressure of oxygen in the air diffusing its cathode is 0.24 atm, what is the cell potential (Ecell)? Assume the cell reaction is:
2 Zn(s) + O2(g) yields 2 ZnO(s)
The standard reduction potentials of the half-reactions in zinc-air batteries are:
ZnO(s) +H2O(l) + 2e- yields Zn(s) + 2OH-(aq) Eored = -1.25V
O2(g) + 2 H2O(l) + 4e- yields 4 OH-(aq) Eored= 0.401
Should use Nernst Equation and answer should be in volts. Thank you!
The standard cell potential (Eocell) of the zinc-air battery is 1.65V. If at 25.0oC the partial pressure of oxygen in the air diffusing its cathode is 0.24 atm, what is the cell potential (Ecell)? Assume the cell reaction is:
2 Zn(s) + O2(g) yields 2 ZnO(s)
The standard reduction potentials of the half-reactions in zinc-air batteries are:
ZnO(s) +H2O(l) + 2e- yields Zn(s) + 2OH-(aq) Eored = -1.25V
O2(g) + 2 H2O(l) + 4e- yields 4 OH-(aq) Eored= 0.401
Should use Nernst Equation and answer should be in volts. Thank you!
Reid WolffLv2
5 Apr 2019
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