Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 1 that has an equilibrium constant of K = 28?

What would be the answer to this fine question. How would you do something like this?

Thanks :)

ΔG∘rxn = ......kj

E∘cell = ......V

dGo = -RTlnK

dGo = -nFE

To calculate ΔG∘rxn, you can use the equation:

ΔG∘rxn = -RT ln(K)

where ΔG∘rxn is the change in Gibbs free energy, R is the gas constant (8.314 J/(mol·K)), and T is the temperature in Kelvin.

To calculate E∘cell, you can use the equation:

E∘cell = (0.0592 V / n) log(K)

where E∘cell is the standard cell potential, n is the number of electrons transferred in the redox reaction, and log represents the logarithm with base 10.

Since the given question states that n = 1 and K = 28, we can plug those values into the equations.

ΔG∘rxn = -RT ln(K)
ΔG∘rxn = -(8.314 J/(mol·K)) * T * ln(28)
Note: To get the value in kilojoules (kJ), you can divide by 1000.

E∘cell = (0.0592 V / 1) log(K)
E∘cell = (0.0592 V) log(28)

To obtain the numerical values, you would need to know the temperature at which the reaction is taking place. Plug in the appropriate temperature in Kelvin (T), and calculate ΔG∘rxn and E∘cell using the given equations.