Since the emf of a cell is always the algebraic sum of two electrode potentials or...

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Since the emf of a cell is always the algebraic sum of two electrode potentials or of two half-cell potentials, it is convenient to calculate each electrode potential separately. For example, for the electrode reaction Zn +2e Zn (3.7) -> we have RT In (Zn) OZn = (3.8) 2F (Zn) where (Zn) represents the activity of zinc ions (molality x activity coefficient); (Zn) is the activity of metallic zinc, the latter being a pure solid and equal, there- fore, to unity; and o2, is the standard potential of zinc (equilibrium potential of zinc in contact with Zn at unit activity). Since it is more convenient to work with logarithms to the base 10, the value of the coefficient RT/F is multiplied by the conversion factor 2.303. Then, from the value of R= 8.314J/deg-mole, T = 298.2 K, and F= 96,500 Cleq, the coefficient 2.303 RT/F at 25°C becomes 0.0592V. This coefficient appears frequently in expavcians ranaanting notentials or emf. ?Verify this number is correct Since the emf of a cell is always the algebraic sum of two electrode potentials or of two half-cell potentials, it is convenient to calculate each electrode potential separately. For example, for the electrode reaction Zn +2e Zn (3.7) -> we have RT In (Zn) OZn = (3.8) 2F (Zn) where (Zn) represents the activity of zinc ions (molality x activity coefficient); (Zn) is the activity of metallic zinc, the latter being a pure solid and equal, there- fore, to unity; and o2, is the standard potential of zinc (equilibrium potential of zinc in contact with Zn at unit activity). Since it is more convenient to work with logarithms to the base 10, the value of the coefficient RT/F is multiplied by the conversion factor 2.303. Then, from the value of R= 8.314J/deg-mole, T = 298.2 K, and F= 96,500 Cleq, the coefficient 2.303 RT/F at 25°C becomes 0.0592V. This coefficient appears frequently in expavcians ranaanting notentials or emf. ?Verify this number is correct

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