Textbook Example 6N.1

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Textbook Example 6N.1

Postby JamieVu_2C » Sun Feb 23, 2020 1:51 am

Calculate the equilibrium constant at 25.00 degreesC for the reaction . The equilibrium constant for this reaction is actually the solubility product, Ksp = [Ag+][Cl-], for silver chloride.

The two reduction half reactions are

Then, the book states that you reverse the second half reaction, which would become an oxidation half reaction: .

How do you know that AgCl constitutes one half reaction and that Ag alone constitutes the other half reaction? Also, how would you know to reverse the second half reaction for Ag instead of the first half reaction for AgCl?

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Joined: Sat Jul 20, 2019 12:16 am

Re: Textbook Example 6N.1

Postby chemboi » Sun Feb 23, 2020 12:16 pm

Unsure about the first part of your question, but as for why you reverse one of them, its to yield the overall net reaction as given in the problem.

Return to “Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)”

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