Ch.18 - ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Determine the cell notation for the redox reaction given below    3 Cl2(g) + 2 Fe(s) → 6 Cl (aq) + 2 Fe3+(aq)A) Fe(s) | Fe 3+(aq) || Cl 2(g), Cl(aq) | PtB) Cl (aq) | Cl 2(g) | Pt || Fe 3+(aq) | Fe(s)   C) Fe(s) | Fe3+(aq) || Cl 2(g) | Cl  (aq) | PtD) Fe(s) | Cl 2(g) || Fe 3+(aq) | Cl  (aq) | PtE) Pt | Cl 2(g) | Cl  (aq) || Fe3+(aq) | Fe(s)

Solution: Determine the cell notation for the redox reaction given below    3 Cl2(g) + 2 Fe(s) → 6 Cl− (aq) + 2 Fe3+(aq)A) Fe(s) | Fe 3+(aq) || Cl 2(g), Cl−(aq) | PtB) Cl− (aq) | Cl 2(g) | Pt || Fe 3+(aq) | Fe(

Problem

Determine the cell notation for the redox reaction given below

    3 Cl2(g) + 2 Fe(s) → 6 Cl (aq) + 2 Fe3+(aq)

A) Fe(s) | Fe 3+(aq) || Cl 2(g), Cl(aq) | Pt

B) Cl (aq) | Cl 2(g) | Pt || Fe 3+(aq) | Fe(s)   

C) Fe(s) | Fe3+(aq) || Cl 2(g) | Cl  (aq) | Pt

D) Fe(s) | Cl 2(g) || Fe 3+(aq) | Cl  (aq) | Pt

E) Pt | Cl 2(g) | Cl  (aq) || Fe3+(aq) | Fe(s)

Solution

We’re being asked to determine the cell notation for the redox reaction shown below:

    3 Cl2(g) + 2 Fe(s) → 6 Cl(aq) + 2 Fe3+(aq)


When writing a cell notation, we use the following format – “as easy as ABC


To determine the cell notation of the reaction, we will use the following steps:

Step 1: Separate the reaction into two half-reactions.
Step 2: Determine the anode and the cathode.
Step 3: Write the cell notation of the reaction.

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