Use the tabulated half-cell potentials to calculate the equilibrium constant (k) for the following balanced redox reaction at 25°c. 2 al(s) + 3 mg2+(aq) → 2 al3+(aq) + 3 mg(s) a) 1.1 × 1072 b) 8.9 × 10-73 c) 1.1 × 10-72 d) 1.0 × 1024 e) 4.6 × 1031

Thus the value of equilibrium constant for the balanced redox reaction at 25°C is

Explanation:

Here Al undergoes oxidation by loss of electrons, thus act as anode. magnesium undergoes reduction by gain of electrons and thus act as cathode.

Where both are standard reduction potentials.

The standard emf of a cell is related to Gibbs free energy by following relation:

= gibbs free energy

n= no of electrons gained or lost = 6

F= faraday's constant

= standard emf

The Gibbs free energy is related to equilibrium constant by following relation:

R = gas constant = 8.314 J/Kmol

T = temperature in kelvin =

K = equilibrium constant

Thus the value of equilibrium constant for the balanced redox reaction at 25°C is

5.6⋅10−^19  j

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