For the reaction 2co3+(aq)+2cl−(aq)→2co2+(aq)+cl2(g) . e∘=0.483 v what is the cell potential at 25 ∘c if the concentrations are [co3+]= 0.765 m , [co2+]= 0.369 m , and [cl−]= 0.486 m , and the pressure of cl2 is pcl2= 9.30 atm ? express your answer with the appropriate units.

Ecell = 0.500 V

Explanation:

For a chemical cell, the cell potential (Ecell) is:

Ecell = E° - (0.0592/n)*logQ (Nernst equation)

Where n is the number of electrons involved in the redox reaction, and Q is the reaction coefficient.

Let's see a half-reaction:

2Co³⁺(aq) → 2Co²⁺(aq)

The charge goes from +6 (2*3) to +4 (2*2), so n = 6 - 4 = 2 electrons.

The reaction coefficient is the multiplication of the concentration of the products elevated by their coefficients, divided by the multiplication of the concentration of the reactants elevated by their coefficients:

Q = ([Cl₂]*[Co⁺²]²)/([Co⁺³]²*[Cl⁻]²)

The concentration of Cl₂ is the number of moles (n) divided by the volume(V), and can be calculated by the ideal gas law:

PV = nRT

n/V = P/RT  (P is the pressure, R is the gas constant, and T is the temperature)

P = 9.30 atm, R = 0.082 atm.L/mol.K, T = 25°C + 273 = 298 K

n/V = [Cl₂] = 9.30/(0.082*298)

[Cl₂] = 0.381 M

Q = [0.381*(0.369)²]/[(0.765)²*(0.486)²]

Q = 0.051877/0.138228

Q = 0.3753

Ecell = 0.483 - (0.0592/2)*log(0.3753)

Ecell = 0.483 - 0.0296*(-0.4256)

Ecell = 0.500 V

5.6⋅10−^19  j

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