If the equilibrium constant for a two electron redox reaction at 198 °C is 1500, calculate the ΔG° and E0red.
The value of Gibbs free energy is given by :
∆G = - RT ln K
Where ∆G = Gibbs free energy
T = Temperature in Kelvin
R = gas constant
K = equilibrium constant.
The relation between ∆G and reduction potential is given by :
∆G = - nFE
Using the above relation the value of both the unknowns can be calculated .
The problem is solved in the picture attached below :
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If the equilibrium constant for a two electron redox reaction at 198 °C is 1500
If the equilibrium constant for a two electron redox reaction at 198 oC is 1500, calculate the ΔG° and E0red.
If the equilibrium constant for a two electron redox reaction at 198 oC is 1500, calculate the ΔG° and E0red.
If the equilibrium constant for a two electron redox reaction at 198 oC is 1500, calculate the ΔG° and E0red.
If the equilibrium constant for a two electron redox reaction at 198 °C is 1500, calculate the AG and Ered. Aril 3 (12)
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