Question

In: Chemistry

Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 3 that has an equilibrium...

Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 3 that has an equilibrium constant of K = 5.3×10⁻².

ΔG∘rxn =

E∘cell =

Expert Solution

We have relation, G ⁰_rxn = - 2.303 R T log K , where K is equilibrium constant.

G ⁰_rxn = - 2.303 8.314 J K ^-1 mol ^-1 298 K log 5.3 10 ⁻²

= + 72279 J / mol

= + 7.279 k J / mol

ANSWER : G ⁰_rxn = 7.3 k J / mol

We have relation , G ⁰ = - n F E ⁰ cell

Where n = no. of moles of electrons transferred in the overall reaction.

We have, n = 3 , F = 96487 C / mol & G ⁰ =7.279 k J / mol

72279 J / mol = - 3 96487 C / mol E ⁰ cell

E ⁰ cell = 72279 / ( - 3 96487 )

E ⁰ cell = - 0.2497 V

ANSWER : E ⁰ cell = - 0.25 V

queen_honey_blossom answered 2 years ago

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