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: A chemist designs a galvanic cell that uses these two half-reactions:Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that h

Solution: A chemist designs a galvanic cell that uses these two half-reactions:Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that h

Problem

A chemist designs a galvanic cell that uses these two half-reactions:

Write a balanced equation for the half-reaction that happens at the cathode. 

Write a balanced equation for the half-reaction that happens at the anode.

Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Do you have enough information to calculate the cell voltage under standard conditions?

If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits.

Solution

Based on the half-reactions shown, a chemist designs a galvanic cell. We are asked to write the balanced equations for the half-reactions at the cathode, anode, and overall reaction. And additionally, to calculate the cell voltage if possible.


Assuming the reaction is under acidic conditions, we will follow the following steps to balance the reactions:

Step 1: Separate the whole reaction into two half-reactions

Step 2: Balance the non-hydrogen and non-oxygen elements first

Step 3: Balance oxygen by adding H2O to the side that needs oxygen (1 O: 1 H2O)

Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen (1 H: 1 H+)

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