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 voltaic cell is constructed froman Ni2 +  (aq) - Ni(s) half-cell andan Ag+ (aq) - Ag(s) half-cell.The initial concentration of Ni2 +  (aq) in the Ni2 +   - Ni half-cell is [Ni2 +  ] = 1.50×10−2 M .

Solution: A voltaic cell is constructed froman Ni2 +  (aq) - Ni(s) half-cell andan Ag+ (aq) - Ag(s) half-cell.The initial concentration of Ni2 +  (aq) in the Ni2 +   - Ni half-cell is [Ni2 +  ] = 1.50×10−2 M .

Problem

A voltaic cell is constructed from
an Ni2 +  (aq) - Ni(s) half-cell and
an Ag+ (aq) - Ag(s) half-cell.

The initial concentration of Ni2 +  (aq) in the Ni2 +   - Ni half-cell is [Ni2 +  ] = 1.50×10−2 M . The initial cell voltage is +1.13 V .

By using data in Table 20.1 in the textbook, calculate the standard emf of this voltaic cell.

Solution

We’re being asked to determine the standard cell potential (E°cellof the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:

EOcell = EO cathode - EOanode


When a balanced reaction is given, identify the anode and the cathode half-reactions by determining the changes in oxidation states of each species based on the given reaction:

Recall:

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