Respuesta :
The standard EMF is -0.0351 V and Gibbs free energy is 6.77 kJ/mol
The relation between standard EMF and equilibrium constant is as follows;
E0cell=0.0592/n logK
Substituting the values, we get
E0cell=0.0592/2 log(0.065)
Eocell=0.0592(-1.187)
E0cell=0.0296(-1.187)
E0cell=-0.0351 V
The relation between Gibbs free energy and E0cell is as follows;
ΔG0=-nFE0cell
ΔG0=-2×96500×(-0.0351)
ΔG0=6774.3
ΔG0=6.77 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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