1. 3) Given the following spontaneous reaction occurring in an electrochemical c

ID: 933360 • Letter: 1

Question

3) Given the following spontaneous reaction occurring in an electrochemical cell under standard condition (25C, 1 atm, 1 mol/L)

3 Cl2(g) + 2 Fe(s) ? 6 Cl - (aq) + 2 Fe3+(aq)

Cl2(g) + 2 e - ? 2 Cl - (aq) E = +1.36 V Eq.1

Fe3+(aq) + 3 e - ? Fe(s) E = -0.04 V Eq.2

(3). What is the standard free energy change (DG) of the battery reaction?

(4). If the above battery reaction reaches its equilibrium, then what is the equilibrium constant K ?

3. 3 Cl2(g) + 2 Fe(s) ------> 6 Cl - (aq) + 2 Fe3+(aq)

Reduction Cl2(g) + 2 e- ---------------------> 2 Cl - (aq) Eo = +1.36 V

oxidation Fe3+(aq) + 3 e - -----------------> Fe(s) Eo = -0.04 V

Eo cell = Eo red - Eo ox = 1.36 - (-0.04) = 1.4V

delta G = -nFEocell

n = chane in electrons = 6 e-

F = 96500F

So, delta G = - 6 x 96500 x 1.4 = -810600J = -810.6kJ

4. delta G = -RTlnK

-810600 = -8.314 J/K/mol x 298Kx lnK

ln K = 327.17

K = e^(327.17)

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