Ch.18 - ElectrochemistryWorksheetSee all chapters
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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 current of 0.5 amp flows through an electrochemical cell that evolves Cl 2 gas by the oxidation of Cl1-. What number of moles of Cl 2 gas are generated in a period of 30 min?A) 900 moleB) 9.3 x10-3

Solution: A current of 0.5 amp flows through an electrochemical cell that evolves Cl 2 gas by the oxidation of Cl1-. What number of moles of Cl 2 gas are generated in a period of 30 min?A) 900 moleB) 9.3 x10-3

Problem

A current of 0.5 amp flows through an electrochemical cell that evolves Cl 2 gas by the oxidation of Cl1-. What number of moles of Cl 2 gas are generated in a period of 30 min?


A) 900 mole
B) 9.3 x10-3 mole
C) 4.6 x10-3 mole
D) 1.6 x 10-4 mole
E) 7.8 x 10-5 mole

 

Solution

We’re being asked to calculate the number of moles of Cl2 gas evolved from the oxidation of Cl-.

Given:

current = 0.5 A

 Note that amperes (A) = charge/time = C/s

Current = 0.5 C/s

 t = 30 minutes

Since current is in C/s, we will have to convert time from min to s

 Faraday’s constant = 96,485 C/(mol e-)

Constant found in books or on the internet


Let’s first determine how many electrons are involved when Cl2 is generated from the reaction:

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