In the activity, click on the e∘cell and keq quantities to observe how they are related. use this relation to calculate keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. the two half-reactions that occur in the cell arecu2+(aq)+2e−→cu(s) and fe(s)→fe2+(aq)+2e−

The of the reaction is 0.78 V and respectively.

Explanation:

For the given half reactions:

Oxidation half reaction:

Reduction half reaction:

Net reaction:

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the of the reaction, we use the equation:

Putting values in above equation, we get:

To calculate equilibrium constant, we use the relation between Gibbs free energy, which is:

and,

Equating these two equations, we get:

where,

n = number of electrons transferred = 2

F = Faraday's constant = 96500 C

= standard electrode potential of the cell = 0.78 V

R = Gas constant = 8.314 J/K.mol

T = temperature of the reaction =

= equilibrium constant of the reaction = ?

Putting values in above equation, we get:

Hence, the of the reaction is 0.78 V and respectively.

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