Respuesta :

The standard EMF is 0.107 V and Gibbs free energy is 10.3 kJ/mol

The relation between standard EMF and equilibrium constant is as follows;

E0cell=0.0592/n logK

Substituting the values, we get

E0cell=0.0592/1 log(65)

Eocell=0.0592(1.81)

E0cell=0.107V

The relation between Gibbs free energy and E0cell is as follows;

ΔG0=-nFE0cell

ΔG0=-1×96500×(0.107)

ΔG0=10325.5

ΔG0=10.3 kJ/mol

  • The equilibrium constant can be calculated using the Nernst equation and the relationship between standard cell potential and free energy.
  • The Nernst equation calculates electrochemical cell potential from standard cell potential, gas constant, temperature, number of moles of electrons, Faraday's constant, and the reaction quotient.
  • The reaction quotient is the equilibrium constant at equilibrium.

Learn more about the equilibrium constant at:

brainly.com/question/10038290

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