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+] = 0.190 M, [Co2+] = 0.205 M, and [Cl-] = 0.144 M, and the pressure of Cl2 is PCl2 = 7.30 atm?

Question

Eddie Mcneil

Chemistry

29 June, 10:52

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+] = 0.190 M, [Co2+] = 0.205 M, and [Cl-] = 0.144 M, and the pressure of Cl2 is PCl2 = 7.30 atm?

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Answers (1)

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Carlo Vance · Answer 1

Ecel = 0,04 V

Explanation:

Apply the Nerst equation,

Ecel = Ecelº - (RT/nF) * lnQ

where R=8,314 J/molK, T=25ºC=298K and F = 96 485 Coulombs/mol e - and n=number of moles of electrons transferred in the balanced equation. Q is cocient of products and reactives power to respective coefficients, if is a gas apply partial pressure

Write the semiequation redox and verify the numbers of electron for balance. In this case you don't need to change nothing

2Cl - (aq) →Cl2 (g) + 2e-

2CO3 + (aq) + 2e-→2CO2 + (aq)

2Cl - (aq) + 2CO3 + (aq) →2CO2 + (aq) + Cl2 (g)

Hence

Ecel = 0.483 V - 0.013Ln ([CO2+]^2*PCl2] / [CO3+]^2*[Cl-]^2)

Ecel = 0.483 V - 0.013Ln ([0.205]^2 * 7.3] / [0.19]^2*[0.144]^2)

Ecel = 0,04 V