Respuesta :
Explanation:
Formula to calculate standard electrode potential is as follows.
[tex]E^{o}_{cell} = E^{0}_{cathode} - E^{0}_{anode}[/tex]
= 0.535 - 1.065
= - 0.53 V
Also, it is known that relation between [tex]E^{o}_{cell}[/tex] and K is as follows.
[tex]E^{o}_{cell} = \frac{RT}{nF} \times ln K[/tex]
ln K = [tex]\frac{nFE^{0}_{cell}}{RT}[/tex]
Substituting the given values into the above formula as follows.
ln K = [tex]\frac{nFE^{0}_{cell}}{RT}[/tex]
= [tex]\frac{2 \times 96485 C mol^{-1} \times -0.53 V}{8.314 l atm/mol K \times 298 K} \times \frac{1 J}{1 V C}[/tex]
ln K = -41.28
K = [tex]e^{-41.28}[/tex]
= [tex]1 \times 10^{-18}[/tex]
Thus, we can conclude that the value of the equilibrium constant for the given reaction is [tex]1 \times 10^{-18}[/tex].
