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Calculate the equilibrium constant K for the following reaction at 25°C from standard electrode potentials. Fe³(aq) + Cu(s) = Fe²(aq) + Cu²(aq)
The equation is not balanced. Use standard reduction electrode potentials.

Respuesta :

The equilibrium constant K for the following reaction at 25°C from standard electrode potentials is Antilog (37.5).

What is chemical equilibrium?

Chemical equilibrium is the condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs.

Reduction Half-Reaction

[tex]Fe^{3+}[/tex](aq)+[tex]e^-[/tex] →[tex]Fe^{2+}[/tex](aq)

Standard reduction electrode potentials = +0.77

Oxidation Half-Reaction

Cu(s) = [tex]Cu^{+2}[/tex](aq) + 2[tex]e^-[/tex]

Standard reduction electrode potentials = -0.34

E° cell= E°cathode- E°anode

E° cell= +0.77+0.34

E° cell=1.11

E°cell= 0.0592÷n logK

From the redox reaction equations above, n=2

1.11 V= 0.0592÷2 logK

37.5 =  logK

K= Antilog (37.5)

Hence,  the equilibrium constant K for the following reaction at 25°C from standard electrode potentials is Antilog (37.5).

Learn more about chemical equilibrium here:

https://brainly.com/question/4289021

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