Agalvanic cell consists of a iron electrode in 1 m fe(no3)2 and a copper electrode in 1 m cu(no3)2. what is the equilibrium constant for this reaction at 25oc?

Keq = 5.33*10²⁶

Explanation:

Based on the standard reduction potential table:

E°(Fe2+/Fe) = -0.45 V

E°(Cu2+/Cu) = +0.34 V

Since the reduction potential of copper is greater than iron, the former acts as the cathode and the latter as anode.

The half reactions are:

Cathode (Reduction):

Anode (Oxidation):

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Overall reaction:

The Gibbs free energy change at 25 C is related to the standard emf (E°) of the cell as well as the equilibrium constant K as:

here:

R = 8.314 J/mol-K

T = 25 C = 25+273 = 298 K

n = number of electrons involved = 2

F = 96500 Coulomb/mol e-

Keq = 5.33*10²⁶

the law of conservation of mass states that in a chemical reaction, the total mass of reactants is equal to the total mass of products. because atoms are only rearranged in a chemical reaction, there must be the same number of sodium atoms and chlorine atoms in both the reactants and products

1.solid

2.carbon dioxide

3.helium