**Cell Notation for an Electrochemical Cell**Task: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized to Cr³⁺ (aq) and a cathode where Ni²⁺ (aq) is reduced to Ni (s). Assume all aqueous solutions have a concentration of 1 mol/L.---**Cell Notation:**Anode (oxidation half-cell): Cr (s) → Cr³⁺ (aq) + 3e⁻ Cathode (reduction half-cell): Ni²⁺ (aq) + 2e⁻ → Ni (s) **Overall Cell Notation:**Cr (s) | Cr³⁺ (aq, 1 M) || Ni²⁺ (aq, 1 M) | Ni (s)**Explanation:**- The anode side is represented by chromium solid being oxidized to chromium ions in solution.- The cathode side shows nickel ions in the solution being reduced to nickel solid.- The single vertical lines (|) separate different states or phases.- The double vertical lines (||) represent the salt bridge or porous barrier between the two half-cells.- The concentration of the solutions is indicated in parentheses.

Representation of a galvanic cell (Cell notation) i.Galvanic cell consists of two electrodes, anode…

Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized to Cr³+ (aq) and a cathode where Ni2+ (aq) is reduced to Ni (s). Assume all aqueous solutions have a concentration of 1 mol/L.

Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized to Cr³+ (aq) and a cathode where Ni2+ (aq) is reduced to Ni (s). Assume all aqueous solutions have a concentration of 1 mol/L.

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

**Cell Notation for an Electrochemical Cell**

Task: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized to Cr³⁺ (aq) and a cathode where Ni²⁺ (aq) is reduced to Ni (s). Assume all aqueous solutions have a concentration of 1 mol/L.

---

**Cell Notation:**

Anode (oxidation half-cell): Cr (s) → Cr³⁺ (aq) + 3e⁻
Cathode (reduction half-cell): Ni²⁺ (aq) + 2e⁻ → Ni (s)

**Overall Cell Notation:**

Cr (s) | Cr³⁺ (aq, 1 M) || Ni²⁺ (aq, 1 M) | Ni (s)

**Explanation:**

- The anode side is represented by chromium solid being oxidized to chromium ions in solution.
- The cathode side shows nickel ions in the solution being reduced to nickel solid.
- The single vertical lines (|) separate different states or phases.
- The double vertical lines (||) represent the salt bridge or porous barrier between the two half-cells.
- The concentration of the solutions is indicated in parentheses.

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