Give the equilibrium constant for the following reaction at 298 K.
In the given cell reaction, cupric ion is being reduced to copper and Sn+2 is being oxidized to Sn+4. The standard reduction potential of the former is 0.340 V and the standard oxidation potential of the latter is -0.154 V. The standard electrode potential is equal to the sum of the standard reduction potential and standard oxidation potential. The value of standard electrode potential is equal to 0.340 – 0.154 = 0.186 V. The relationship between standard Gibbs free energy and standard electrode potential can be depicted as ∆Go = -nFEocell. The value of n = 2 mol and F = 96500 C/mol. The value of standard Gibbs free energy can be calculated as follows:
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