I need the equilibrium constant for part C Consider the following two half-react

Question

I need the equilibrium constant for part C

Consider the following two half-reactions and their standard reduction potentials. Answer the three questions below. O_3(g) + H_2O(t) + 2e^- rightarrow O_2(g) + 2OH^-(aq) E degree = 1.246 V Clo^-_3 (aq) + 3 H_2 O(l) + 6e^- rightarrow Cl^-(aq) + 6OH^-(aq) E degree = 0.622 V (a) Calculate E degree for the spontaneous redox reaction that occurs when these two half-reactions are coupled. (b) Calculate the value of Delta G degree for the reaction. (c) Determine the equilibrium constant for the reaction.

Explanation / Answer

First

E° = Ered - Eox

Ered = the species with higher potentil, Eox = the species with lower potential

so

E° = 1.2466 - 0.622 = 0.6246

for

dG

dG = -nF*E°

n = 6 electrons are transferrred, F = 96500 C/mol farady constant

dG = -6*96500*0.6246 = -361643.4J/mol = - 361.64 kJ/mo

c)

For equilibrium

dG° = -RT*ln(K)

361643.4 = 8.314¨*298*ln(K)

K = exp(361643.4/(8.314*298))

K = 2.469*10^63

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