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General Chemistry II - Exam 2 Study Guide | CHM 2046, Study notes of Chemistry

Exam 2 Study Guide Material Type: Notes; Professor: Johnston; Class: General Chemistry II; Subject: Chemistry; University: University of South Florida; Term: Spring 2011;

Typology: Study notes

2010/2011

Uploaded on 03/29/2011

jshirley
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Exam 2 Study Guide/Formula Sheet
Chapter 13
Rate of Reaction
Rate Law
Rate law summary table
Arrhenius Equation
Rate Laws for elementary steps
Chapter 14
Equilibrium Constant
Significance of Equilibrium Equation
Equilibrium constant and chemical equations
1. If you reverse the equation, invert the equilibrium constant.
2. If you multiply the coefficients in the equation by a factor, raise the equilibrium
constant to the same factor.
3. If you add two or more individual chemical equations to obtain an overall
equation, multiply the corresponding equilibrium constants by each other to
obtain the overall equilibrium constant.
Equilibrium Constant-Pressure Reaction Quotient
Direction of a reaction
Q < K Reaction goes to the right.
Q > K Reaction goes to the left.
Q = K Reaction is at equilibrium.
Concentration change on equilibrium
Volume change on equilibrium
Temperature change on equilibrium
Chapter 15
Bronsted Lowry Definition
Strong acids
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Exam 2 Study Guide/Formula Sheet

Chapter 13 Rate of Reaction Rate Law Rate law summary table Arrhenius Equation Rate Laws for elementary steps Chapter 14 Equilibrium Constant Significance of Equilibrium Equation Equilibrium constant and chemical equations

  1. If you reverse the equation, invert the equilibrium constant.
  2. If you multiply the coefficients in the equation by a factor, raise the equilibrium constant to the same factor.
  3. If you add two or more individual chemical equations to obtain an overall equation, multiply the corresponding equilibrium constants by each other to obtain the overall equilibrium constant. Equilibrium Constant-Pressure Reaction Quotient Direction of a reaction Q < K Reaction goes to the right. Q > K Reaction goes to the left. Q = K Reaction is at equilibrium. Concentration change on equilibrium Volume change on equilibrium Temperature change on equilibrium Chapter 15 Bronsted Lowry Definition Strong acids

Weak Acids Acid ionization constant pH pOH pKa Percent ionization of weak acid Strong bases Weak bases Ions as acids and bases pH of salt solution Acid strength and molecular structures Lewis acids and bases