General Chemistry 1B. Lecture 15. Chemical Equilibrium, Part II

UCI Chem 1B General Chemistry (Winter 2013)
Lec 15. General Chemistry -- Chemical Equilibrium Part 2 --
Instructor: Donald R. Blake, Ph.D.

License: Creative Commons BY-NC-SA

Description: UCI Chem 1B is the second quarter of General Chemistry and covers the following topics: properties of gases, liquids, solids; changes of state; properties of solutions; stoichiometry; thermochemistry; and thermodynamics.

This video is part of a 17-lecture undergraduate-level course titled "General Chemistry" taught at UC Irvine by Professor Donald R. Blake.

Recorded March 7, 2013.

Index of Topics:
0:00:28 Reaction Quotient
0:02:25 Writing Equilibrium Constants
0:09:55 Equilibrium Concentrations for the Reaction
0:16:54 Equilibrium Constant Kp
0:20:58 Free Energy vs Progress of Reaction
0:22:36 Equilibrium Constant and Free Energy
0:23:56 Equilibrium
0:24:40 Reaction Quotient
0:28:47 Equilibria Involving Condensed Phases
0:29:43 Vapor Color Intensity
0:31:21 Consider the Following Equilibrium...
0:36:52 Adding Equilibrium Reactions
0:41:40 Writing Equilibrium Constants
0:43:10 Chemical Kinetics and Chemical Equilibrium
0:45:31 Summary of Concepts
0:46:44 Multiple Equilibria
0:47:03 Carbonic Acid Ionizes in Water
0:49:19 Dr. Hess Returns
0:54:11 Reverse Equation 1 and Multiply by Two
0:56:28 Methane and Water
0:59:12 Isomerization Equilibrium Constant

[mina_ashraf]

At a certain temperature K for the reaction 2NO2 (reversible reaction arrows) N2O4 is 7.5 liters/mole. If 2.0 moles
of NO2 are placed in a 2.0-liter container and permitted to react at this temperature, calculate
the concentration of N2O4 at equilibrium.

can anyone explain how to solve this please ?

[celesteadeanes]

What is he using for volume for PV n rT?

[JeameePotpot]

Just found out my professor copied your slides 😂