Respuesta :

The standard EMF is -0.255 V and Gibbs free energy is 24.6 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(5.0×10^-6)

Eocell=0.0592(log5-6log10)

E0cell=0.0592(0.69-5)

E0cell=-0.255 V

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

ΔG0=-nFE0cell

ΔG0=-1×96500×(-0.255)

ΔG0=24607.5

ΔG0=24.6 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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