🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
HomeStudy Guides420,000US230,000

CHM 132 Study Guide - Final Guide: Magnesium Chloride, Mercury Battery, Royal Aircraft Factory F.E.2

113 views14 pages
School
University of Rochester
Department
Chemistry
Course
CHM 132
Professor
Kara Bren

For unlimited access to Study Guides, a Grade+ subscription is required.

Document Summary

Electrochemistry - a branch of chemistry that deals with the exploitation of spontaneous oxidation-reduction reactions to obtain electrical energy and the use of electrical energy to drive nonspontaneous reactions important in industrial extraction of certain elements. A galvanic cell (also called voltaic cell) is a device that uses a spontaneous oxidation-reduction reaction to produce electric current. The following are some examples of spontaneous oxidation-reduction reactions: Me: cr(s) + 3agno3(aq) cr(no3)3(aq) + 3ag(s) nie: Cr(s) + 3ag+(aq) cr3+(aq) + 3ag(s) nie: mno4. Redox reactions can be broken into two half-reactions: Reduction half-reaction: cu2+(aq) + 2 e- cu(s) (aq) + 5fe2+(aq) + 8h+(aq) mn2+(aq) + 5fe3+(aq) + 4h2o(l) (aq) + 8h+(aq) + 5e- mn2+(aq) + 4h2o(l) Heat produced in an exothermic reaction is normally lost as heat. However, it can be trapped and converted into electrical energy if the reactants involved are not in direct contact with each other.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers

Related Documents

CHM 132 Chapter Notes - Chapter 11: Galvanic Cell, Membrane Potential, Voltmeter
silverbee937
CHM 132
Final Exam
Study Guide
CHM 132 Study Guide - Midterm Guide: Membrane Potential, Galvanic Cell, Reaction Quotient
silverbee937
CHM 132
Final Exam
Study Guide
CHM 132 Study Guide - Final Guide: Heat Capacity, Nernst Equation, Galvanic Cell
silverbee937

Related Questions

It is a Chemistry homework.

1. Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential.

(a) Al and Co(II)
Cathode: ____

Anode: ______

Ecell =

(b) Cd(II) and Ag(I)

cathode: ___

anode: ___

Ecell= ____

(c) Cr(III) and Sc(III)

cathode: ___

Anode:_____

Ecell:____

2. A voltaic cell contains two half-cells. One half-cell contains a titanium electrode immersed in a 1.00 M Ti(NO3)3 solution. The second half-cell contains a zinc electrode immersed in a 1.00 M Zn(NO3)2 solution.

Ti3+(aq) + 3 e− → Ti(s)

E⁰red  = −1.370 V
Zn2+(aq) + 2 e− → Zn(s)

E⁰red  = −0.762 V

(a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell.

(b) Write the overall balanced equation for the voltaic cell. (Include states-of-matter under the given conditions in your answer.)

3. ΔG° and E° can be said to measure the same thing, and are convertible by the equation

ΔG° = −nFE⁰cell 

where n is the total number of moles of electrons being transferred, and F is the Faraday constant 9.64853415 ✕ 104 C/mol. The free energy (ΔG°) of a spontaneous reaction is always negative.

For each of the electrochemical cells below, calculate the free energy of the system and state whether the reaction is spontaneous or non-spontaneous as written based on the cathode and anode assignment given. (Use the table of Standard Electrode Potentials.)

(a) The cathode is Zn(II) and the anode is Co(II).

free energy: ____ kJ

spontaneity: _____

Show transcribed image text