Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and standard potentials (both written as reduction reactions) in an aqueous basic solution. Cr3+(aq) → Cr2+(aq) E°(Cr3+/Cr2+) = −0.40 V IO−(aq) → I2(aq) E°( IO−/I2) = +1.60 V The pH of this cell is 14, and the concentrations of species are: Cr3+ is 0.5 M, Cr2+is 0.2 M, IO− is 0.5 M and I2 is 0.8 M.
Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and standard potentials (both written as reduction reactions) in an aqueous basic solution. Cr3+(aq) → Cr2+(aq) E°(Cr3+/Cr2+) = −0.40 V IO−(aq) → I2(aq) E°( IO−/I2) = +1.60 V The pH of this cell is 14, and the concentrations of species are: Cr3+ is 0.5 M, Cr2+is 0.2 M, IO− is 0.5 M and I2 is 0.8 M.
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Chapter1: Chemical Foundations
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Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and standard potentials (both written as reduction reactions) in an aqueous basic solution.
Cr3+(aq) → Cr2+(aq) E°(Cr3+/Cr2+) = −0.40 V
IO−(aq) → I2(aq) E°( IO−/I2) = +1.60 V
The pH of this cell is 14, and the concentrations of species are: Cr3+ is 0.5 M, Cr2+is 0.2 M, IO− is 0.5 M and I2 is 0.8 M.
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