CHEM 1050 Lecture Notes - Lecture 8: Nernst Equation, Magnesium Chloride, Chemical Equation

54 views15 pages

magentafly264

12 Oct 2016

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Electrochemical cell: if e is positive, then the reaction favours _____________. Thermodynamics: if g is negative, then the reaction favours ______________. G = n f e and g = n f e n = total number of electrons transferred in the reaction. = charge in coulombs on 1 mole of electrons (c/mol or j v. = e na = 1. 6022 10. E = standard cell potential (or voltage) (v = j c. What this also allows us to do is to calculate values of e from g values or from equilibrium constant values, i. e. , given any one of e , g or keq, we can calculate the others. At 298 k, rt/f = 0. 025693 v, e = (0. 025693/n)lnkeq. {at 298 k, 2. 303rt/f = 0. 0591 v and therefore e = (0. 0591/n)log10 keq. This constant is used when we have log base 10. } Example: calculate the equilibrium constant and g at 298 k for the reaction:

Related Questions

chem1220:

Â± Cell Potential and Equilibrium
18 of 28
Constants | Periodic Table
The equilibrium constant, K, for a redox reaction is related to the standard potential, E?, by the equation
lnK=nFE?RT
where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e?) , R (the gas constant) is equal to 8.314 J/(mol?K) , and T is the Kelvin temperature.
Standard reduction potentials
Reduction half-reaction E? (V)
Ag+(aq)+e??Ag(s) 0.80
Cu2+(aq)+2e??Cu(s) 0.34
Sn4+(aq)+4e??Sn(s) 0.15
2H+(aq)+2e??H2(g) 0
Ni2+(aq)+2e??Ni(s) ?0.26
Fe2+(aq)+2e??Fe(s) ?0.45
Zn2+(aq)+2e??Zn(s) ?0.76
Al3+(aq)+3e??Al(s) ?1.66
Mg2+(aq)+2e??Mg(s) ?2.37

Part A Part complete
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ?C) for the following reaction:
Fe(s)+Ni2+(aq)?Fe2+(aq)+Ni(s)
Express your answer numerically.
View Available Hint(s)
K = 2.68Ã10^6 Correct
When E?>0 and K>1 the reaction favors the products.

Part B
Calculate the standard cell potential (E?) for the reaction
X(s)+Y+(aq)?X+(aq)+Y(s)
if K = 7.87Ã10?3.

Express your answer to three significant figures and include the appropriate units.

E? = ?

CHEM 1050 Lecture Notes - Lecture 8: Nernst Equation, Magnesium Chloride, Chemical Equation

Document Summary

Get access

Related textbook solutions

Chemistry: Structure and Properties

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related Documents

CHEM 1050 Lecture Notes - Lecture 23: Electrical Network, Ampere, Lead

CHEM 1050 Lecture Notes - Lecture 19: Glucono Delta-Lactone, Bayerischer Rundfunk, Bromine

CHEM 1050 Study Guide - Final Guide: Lithium Polymer Battery, Standard Hydrogen Electrode, Mercury Battery

Related Questions