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 1M solution of Cu ( NO3 )2 is placed in a beaker with a strip of Cu metal. A 1 M solution of SnSO4 is placed in a second beaker with a strip of Sn metal. A salt bridge connects the two beakers, and wires to a voltmeter link the two metal electrodes.Write the equation for the overall cell reaction.

Solution: A 1M solution of Cu ( NO3 )2 is placed in a beaker with a strip of Cu metal. A 1 M solution of SnSO4 is placed in a second beaker with a strip of Sn metal. A salt bridge connects the two beakers, and

Problem

A 1M solution of Cu ( NO3 )2 is placed in a beaker with a strip of Cu metal. A 1 M solution of SnSO4 is placed in a second beaker with a strip of Sn metal. A salt bridge connects the two beakers, and wires to a voltmeter link the two metal electrodes.

Write the equation for the overall cell reaction.

Solution

We’re being asked to write the overall balanced equation for a Cu and Sn galvanic cell:


The half cell reactions for Cu and Sn (these potentials can be searched from the internet):

Cu 2+(aq) + 2e- → Cu(s) E = 0.337 V
Sn 2+ (aq) + 2e- → Sn(s) E = -0.136 V


The Anode is where oxidation takes place while the cathode is where reduction takes place. The larger (more +) the reduction potential value is, the more likely that would correspond to reduction and vise versa for oxidation.

Sn will be the anode and Cu will be the cathode reaction.


So the cell notation for the reaction is:

Sn(s) | Sn2+(aq, 1.0 M) || Cu2+(aq, 1.0 M)| Cu(s)


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


Recall the mnemonics LEO GER.

[readmore]

Lose               Gain
Electron         Electrons
Oxidation       Reduction

 lose electrons  oxidation → anode
 gain electrons  reduction → cathode


We’re going to write the overall balanced reaction equation using the following steps:

Step 1: Write the anode reaction.
Step 2: Write the cathode reaction.
Step 3: Balanced anode and cathode reactions.
Step 4: Get the overall reaction.

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