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Ch.6 - Chemical EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 - Chemical Measurements
Ch.2 - Tools of the Trade
Ch.3 - Experimental Error
Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods
Ch.6 - Chemical Equilibrium
Ch.7 - Activity and the Systematic Treatment of Equilibrium
Ch.8 - Monoprotic Acid-Base Equilibria
Ch.9 - Polyprotic Acid-Base Equilibria
Ch.10 - Acid-Base Titrations
Ch.11 - EDTA Titrations
Ch.12 - Advanced Topics in Equilibrium
Ch.13 - Fundamentals of Electrochemistry
Ch.14 - Electrodes and Potentiometry
Ch.15 - Redox Titrations
Ch.16 - Electroanalytical Techniques
Ch.17 - Fundamentals of Spectrophotometry
BONUS: Chemical Kinetics
The Equilibrium State
The Reaction Quotient
Le Chatelier's Principle
Chemical Thermodynamics: Enthalpy
Chemical Thermodynamics: Entropy
Chemical Thermodynamics: Gibbs Free Energy
Solubilty Product Constant
Protic Acids and Bases
The pH Scale
Acid Strength

The reaction quotient, Q, is useful in determining if a chemical reaction is at equilibrium. 

The Reaction Quotient

Concept #1: Comparing Q to K determines which direction the reaction shifts in order to reach equilibrium. 

When Q = K then our chemical reaction is at equilibrium and no shifting will occur. 

If Q is larger than K then the reaction will shift in the reverse direction to attain equilibrium. 

If Q is smaller than K then the reaction will shift in the forward direction to attain equilibrium. 

Example #1: Consider the hypothetical reaction below

3 A (g) + B (g) ↔ 2 C (g)           Kc = 1.5 x 10-3

Which of the following statements is correct if the initial concentrations are [A] = 0.85 M, [B] = 0.36 M, and [C] = 0.005 M.

A. At equilibrium, the amount of C will increase.

B. At equilibrium, the amount of A will increase.

C. At equilibrium, the amount of B will increase and C will increase.

D. At equilibrium, the amount of A will increase and B will decrease.

E. The reaction is at equilibrium.

Reaction Quotient Calculations

Example #2: For the reaction: 2 CO2 (g)  2 CO g) +  2 O2  (g),  the equilibrium constant is 7.22 x 10-4 at 400 K, while the reaction quotient is 6.63 x 10-2. If initially we have 0.20 atm CO2, 0.30 atm CO and 0.15 atm O2, which of the following statements is not true?

a) The pressure of CO2 will be greater than 0.20 atm.

b) The pressure of CO will be less than 0.30 atm.

c) The pressure of O2 will be greater than 0.15 atm.

d) The pressure of O2 will be less than 0.15 atm.

e) The reaction will favor reactants. 

Example #3: For the following reaction:

3 H2 (g) +  N2 (g)  2 NH3 (g)

Keq = 25. At a particular time, the following concentrations are measured for the given compounds: [H2] = 0.005 M, [N2] = 0.170 M and [NH3] = 3.12 x 102 M. Which of the following statements is true?

a) The concentration of H2 will increase.

b) The equilibrium constant will increase.

c) The concentration of NH3 will increase.

d) The concentration of N2 will decrease.

e) No change will occur.