Equilibrium and Kinetics Review
Name: ________________________________ Period: ________
Part 1: LeChatelier’s Principle Determine which direction the listed stress will shift the equilibrium. State how the shift will change
the amounts of each material present to reach a new equilibrium.
2N2(g) + O2(g)  2N2O(g) + heat
Reaction #1:
Stress
Equilibrium Shift
(right, left, none)
N2
inc/dec/no change
O2
inc/dec/no change
N2O
inc/dec/no change
Decrease Pressure
Increase N2 concentration
Increase Heat
Decrease N2O concentration
Reaction #2:
2Al(s) + 6HCl(aq) + heat  2AlCl3(aq) + 3H2(g)
Stress
Equilibrium
Shift (R,L, none)
Al
inc/dec/no change
HCl
inc/dec/no change
AlCl3
inc/dec/no change
H2
inc/dec/no change
Decrease heat
Increase AlCl3 concentration
Decrease H2 concentration
Add Al
Part 2: Equilibrium Expressions and Equilibrium Constants
Reaction #1: 4 HCl(g) + O2(g)  2H2O(g) + 2 Cl2(g) at equilibrium: [HCl] =1.2x10-3M, [O2] = 3.8x10-4M, [H2O]=
0.058M, [Cl2]=0.058M
Write the equilibrium expression
Calculate the value for the equilibrium constant
Reactant or
Product Favored?
Reaction #2: K2O(s) + H2O(l)  2KOH(aq) at equilibrium: [KOH] = 0.05M
Write the equilibrium expression
Calculate the value for the equilibrium constant
Reaction #3: N2(g) + O2(g)  2 NO(g)
Write the equilibrium expression
Reactant or
Product Favored?
at 25°C the K= 6.9 x 10-4 At equilibrium [O2] = 0.0078M, [N2] = 0.041M
Calculate the value of [NO]
Reactant or
Product Favored?
Reaction #4: N2(g) + 3H2(g)  2 NH3(g)
Write the equilibrium expression
at 25°C the K=5.2x10-5 At equilibrium [H2] = 0.80M, [NH3] = 0.0073M
Calculate the value of [N2]
Reactant or
Product Favored?
Kinetics
1. Draw a potential energy diagram for each of the following:
Exothermic Reaction
Endothermic Reaction
a. Label the diagrams with the following: reactants, products, activation energy, activated complex, H.
b. On each of the previous diagrams draw a dashed line to show how the reaction would change with the
addition of a catalyst.
2. Compare the chemical potential energy of products to that of the reactants for an exothermic reaction.
3. Compare the chemical potential energy of products to that of the reactants for an endothermic reaction.
4. Explain how each factor affects reaction rate (Be sure to mention if the rate increases or decreases). Be sure to explain
why this occurs in terms of the Collision Theory:
a. Temperature
b. Surface Area
c. Concentration
d. Catalyst
5. Give two reasons why many collisions between particles do not lead to a chemical reaction.