---
title: "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.  | 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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url: "https://nerd-notes.com/ubq/121411/"
date_modified: "2026-08-23T05:02:09+00:00"
---

# 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.

| 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 \(298\text{ K}\)?

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.

| 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 \(298\text{ K}\)?

- **A.** \(K_1 = (K_2)^4\)
- **B.** \(K_1 = (K_2)^2\)
- **C.** \(K_1 = 4K_2\)
- **D.** \(K_1 = 2K_2\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121411/*