Consider the following redox reaction : 4 2 2 MnO H H C O Mn H O CO The standard reduction potentials are given as below red E 4 MnO /Mn E 1.51V 2 4 CO /H C O E 0.49V If the equilibrium constant of th

Question

Consider the following redox reaction : 4 2 2 MnO H H C O Mn H O CO The standard reduction potentials are given as below red E 4 MnO /Mn E 1.51V 2 4 CO /H C O E 0.49V If the equilibrium constant of the above reaction is given as Keq = 10x, then the value of x = _______ (nearest integer)

Prashant Kotian · Accepted Answer

Correct answer: .. Cell Rxn ; MnO4 – + H2C2O4  Mn2+ + CO2 cell E = E° op of anode + E° RP of cathode = 0.49 + 1.51 = 2.00V At equilibrium Ecell = 0, cell 0.059 E logK n   (As per NCERT RT 0.059 F  But RT 0.0591 F  can also be taken.) 0.059 logK  logK = 338.98

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