Honors Chemistry
Name: ______________________________________ Date: _______________ Mods: ___________
Ch. 14 & 15 Review Packet (Kinetics & Equilibrium)
1) Determine if the reaction rate increases or decreases (a or b) with each of the following
changes:
a. Causes reaction rate to speed up
b. Causes reaction rate to slow down
______ Grind up solid reactants
______ Increase reactant concentrations
______ Add a catalyst
______ Decrease temperature of reaction
______ Increase activation energy
______ Decrease reactant concentrations
______ Increase temperature of reaction
______ Dissolve solid reactants to form aqueous solutions
______ Decrease activation energy
2) Based on your knowledge of zero order, first order, and second order reactants, answer the
following questions:
a. For the reaction A + B  C, two trials of the reaction were completed where the
concentration of reactant B was kept constant. Increasing the concentration of reactant
A from 1.0 M to 2.0 M causes the rate of the reaction to increase by a factor of 4.
Reactant A is therefore a _________________ order reactant.
b. For A + B  C + D, two trials of the reaction were completed where the concentration
of reactant A was kept constant. The concentration of reactant B was decreased by
one-half between trial 1 and trial 2, and the reaction rate was reduced to one-half the
original rate. Reactant B is therefore a _________________ order reactant.
3) For the reaction 2 A + 3 B  3 C + 2 D, if the concentration of A is doubled, the reaction rate
doubles. If the concentration of B is quadrupled, there is no change in the rate of the reaction.
Determine the order of reaction with respect to each reactant and the overall order of reaction.
Write the rate law for the reaction.
a. Order of reactant A: ___________
c. Rate Law:
b. Order of reactant B: ___________
4) Use the following reaction as an example of how a rate law can be determined from
experimental data:
CH3CHO (g)  CH4 (g) + CO (g)
Trial 1
Trial 2
Trial 3
a.
Experimental Data from the Decomposition of CH3CHO
Initial Concentration [CH3CHO]
Initial Concentration [CO]
Initial Rate (M/s)
0.30
0.20
0.60
0.10
0.30
0.067
0.10
0.20
0.067
Determining the order with respect to CH3CHO:
From this evaluation, the order of CH3CHO is _________.
b.
Determining the order with respect to CO:
From this evaluation, the order of CO is _________.
c.
What is the rate law expression for this reaction?
5) Balance the equations below and write the equilibrium expressions for each reaction:
a. ___ Pb(OH)2 (aq) + ___ HCl (aq)
a.
 ___ H2O (l) + ___ PbCl2 (s)
b. ___ RbNO3 (aq) + ___ BeF2 (aq)
b.
 ___ Be(NO3)2 (aq) + ___ RbF (aq)
c. ___ NaF (aq) + ___ Br2 (l)
c.
 ___ NaBr (aq) + ___ F2 (g)
d. ___ NaClO3 (aq)  ___ NaCl (aq) + ___ O2 (g)
d.
6) Place a check mark next to all of the possible stresses which would cause the equilibrium
reaction below to shift is a way which decreases the concentration of F2?
N2 (g) + 3 F2 (g)
2 NF3 (g)
∆H = – 127 kJ
_______ increase the volume of the reaction container
_______ decrease the volume of the reaction container
_______ increase the temperature
_______ decrease the temperature
_______ increase [N2]
_______ decrease [N2]
_______ increase [NF3]
_______ decrease [NF3]
7) For an equilibrium expression (at a given temperature), the equilibrium constant (Keq) can be
determined.
a. If Keq > 1, the ____________________ (products of reactants) predominate/are favored
b. If Keq < 1, the ____________________ (products of reactants) predominate/are favored
8) Determine which reaction (1 or 2) the statements below best describe:
Rxn #1:
Rxn #2:
COCl2 (g) + heat
CO (g) + Cl2 (g)
2 NO2 (g)
N2O4 (g) + heat
Keq = 2.2 x 10–10
Keq = 215
a. ______ At equilibrium, the forward reaction is favored
b. ______ At equilibrium, the reverse reaction is favored
c. ______ Decreasing temperature favors the forward reaction
d. ______ Increasing the volume favors the forward reaction
e. ______ Decreasing the volume favors the forward reaction
f.
______ At equilibrium, there is a higher concentration of reactants than products
g. ______ At equilibrium, there is a higher concentration of products than reactants
9) Given the equilibrium expression of CO(g) + 2 H2 (g) CH3OH(g), if the equilibrium
concentrations are [CO] = 0.0911 M, [H2] = 0.0822 M, [CH3OH] = 0.00892 M, what is the value
of the equilibrium constant? Does the equilibrium favor reactants or products?
10) Once a system has reached equilibrium, are the following true (T) or false (F)?
a. _____ The reaction is finished, no more products are forming.
b. _____ The concentrations of the reactants and the products are equal.
c. _____ The concentrations are no longer changing.
d. _____ The reaction is not over, but will continue forever if isolated.
e. _____ The speed at which products form equals the speed at which reactants form.
11) For the reaction below, if the Keq at 145ᵒC is 0.0533, If [SiH4] = 0.34M; [O2] = 0.22M; [SiO2] =
0.35M; and [H2O] = 0.20M, what would be the reaction quotient (Q) of this reaction? In which
direction would this reaction need to proceed in order to achieve equilibrium?
SiH4 (g) + 2 O2 (g)  SiO2 (g) + 2 H2O (g)
12) Use Le Chatelier’s Principle to determine which direction the reaction below will shift when
each of the following stresses are applied.
O2 (g) + 2 H2 (g)  2 H2O (g)
ΔH = –125.7 kJ
a. The temperature is increased ________________
b. The concentration of H2 decreases _________________
c. The concentration of H2O increases _________________
d. The volume of the container decreases ________________
e. The concentration of O2 increases _______________
13) Initially, 1.50 M N2 (g) and 3.50 M H2 (g) were combine in a container at 700 °C. As a result of
the reaction, the equilibrium concentration of NH3 (g) was 0.540 M. What is the value of the
equilibrium constant for this reaction at the given temperature of 700 °C.
N2 (g) + 3 H2 (g)  + 2 NH3 (g)
I
C
E
14) Given the reaction below, if initial concentrations of H2 (g) and I2 (g) were both 0.10 M and the
Keq (at 600 Kelvin) is 0.016, what will be the concentrations of the reactants and product at
equilibrium?
H2 (g) + I2 (g)  2 HI (g)
I
C
E