AP Chemistry
9.9 Cell Potential and Free Energy
9.5 Free Energy and Equilibrium
A student investigates the thermodynamics of two different oxidation-reduction reactions occurring in separate electrochemical cells at \(298\text{ K}\). Data for each reaction are summarized in the table below.
Which of the following mathematical expressions correctly relates the equilibrium constant of Reaction 1, \(K_1\), to the equilibrium constant of Reaction 2, \(K_2\), at \(298\text{ K}\)?
| Reaction | Standard cell potential (\(E^\circ\)) | Moles of \(e^-\) transferred per mole of reaction (\(n\)) | Equilibrium constant (\(K\)) |
|---|---|---|---|
| 1 | \(+0.60\text{ V}\) | \(2\) | \(K_1\) |
| 2 | \(+0.30\text{ V}\) | \(1\) | \(K_2\) |
Which of the following mathematical expressions correctly relates the equilibrium constant of Reaction 1, \(K_1\), to the equilibrium constant of Reaction 2, \(K_2\), at \(298\text{ K}\)?
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