WorksheetsAP Chem Unit 6
Total questions: 24
Worksheet time: 13mins
A kinetics experiment is set up to measure the rate of the combustion of organic material (wood) with oxygen gas, O2, by measuring the volume of carbon dioxide gas, CO2, generated at 25°C and 1 atm as a function of time.
In general, which does NOT increase the rate of reaction?
Select ALL that apply
increasing the activation energy
increasing the temperature of the reaction
increasing the particle size by using a large block of wood instead of fine particles of sawdust
increasing the concentration of oxygen reacting with the organic material
For the reaction
2A + B → products
use the experimental data provided to determine the rate law.
rate = k [A] [B]
rate = k [A]
rate = k [A] [B]0
rate = k [A]2
A student collects the following kinetics data for a reaction. Based on the data, how would you classify the reaction? Why?
First Order.
Concentration is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is first order.
Zero Order.
Concentration is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is zero order.
Second Order.
Concentration is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is second order.
First Order.
ln(Concentration) is halved after 3.00 min and again after another 3.00min. Thus the half-life of the reaction is constant, so the reaction is first order.
Consider the equation for the decomposition of N2O5(g) and the experimentally determined rate law below.
2N2O5(g) ⇌ 4NO2(g) + O2(g)
rate=k[N2O5]
What are the units for the rate constant, k, with the time measured in minutes?
M-1min-1
M-2min-1
min-1
M-3min-1
An increase in temperature will increase the rate of
an ENDOthermic reaction ONLY
an EXOthermic reaction ONLY
BOTH ENDOthermic and EXOthermic reactions
NEITHER ENDOthermic nor EXOthermic reactions
The rate of formation of NO2(g) in the reaction
2 N2O5(g) → 4 NO2(g) + O2(g)
is 5.78 (mol NO2)/L/s. What is the rate at which N2O5 decomposes?
5.78
(mol N2O5)/L/s
0.723
(mol N2O5)/L/s
2.89
(mol N2O5)/L/s
11.6
(mol N2O5)/L/s
X + Y → Z
The rate law for the hypothetical reaction shown above is as follows:
Rate = k[X][Y]2
Which of the following changes to the system is true? Select ALL that apply.
An increase in the temperature will increase the rate
Doubling the concentration of X will increase the rate more than doubling the concentration of Y
Doubling the concentration of X will increase the rate less than doubling the concentration of Y
Doubling the concentration of X will increase the rate the same as doubling the concentration of Y
Which of the following values correspond to the values of the reaction orders x and y for NO and H2?
x=2, y=1
x=2, y=2
x=1, y=1
x=1, y=2
Which of the following values correspond to the overall reaction order?
3
0
1
2
In the reaction,
NO + O3 → NO2 + O2
the N atom in the NO molecule must strike a terminal O atom in the O3 molecule. Which of the diagrams below would most likely result in the formation of the products?
The graph shows how the concentration of reactant changes over time for the reaction
A → products
How would you best describe the order of the reaction with respect to A and the half-life of A?
The reaction is first order with respect to A.
The half-life is 100sec.
The reaction is zero order with respect to A.
The half-life is 100sec.
The reaction is first order with respect to A.
The half-life is 200sec.
The reaction is zero order with respect to A.
The half-life is 200sec.
The table shows the results from a rate study of the reaction
A + B → products
Starting with known concentrations of A and B in experiment 1, the rate of formation of products was measured. If the reaction was zero order with respect to A and zero order with respect to B, the initial rate of formation of products in experiment 2 would be
X
2X
4X
X/2
Using the graph, what is the rate law of the reaction
HO2(g) → products
and how could you determine the units of the rate constant, k?
rate = k[HO2]
k = -slope
rate = k[HO2]2
k = -slope
rate = k[HO2]2
k = slope
rate = k[HO2]
k = slope
Which of the following best represents the activated complex for the following reaction?
H2 + I2 → 2HI
Which of the following best represents the activated complex and location of the activated complex in the energy profile for the following reaction?
2BrNO → 2NO + Br2
2NH3(g) → 3H2(g) + N2(g)
The data shown was collected at 298K and 1 atmosphere of pressure for the reaction shown above.
Which of the following corresponds to the concentration of N2 at t = 3 seconds?
3.4x10-1 mol/L
1.7x10-1 mol/L
5.1x10-1 mol/L
0.4x10-1
2NH3(g) → 3H2(g) + N2(g)
The data shown was collected at 298K and 1 atmosphere of pressure for the reaction shown above.
Which of the following corresponds to the concentration of H2 at t = 3 seconds?
3.4x10-1 mol/L
1.7x10-1 mol/L
5.1x10-1 mol/L
0.4x10-1
Which of the following is a graph that describes the pathway of reaction that is exothermic and has a large activation energy?
X + Y → Z
The rate law for the hypothetical reaction shown above is as follows:
Rate = k[X]
Which of the following changes to the system is true? Select ALL that apply.
An increase in the temperature will increase the rate, by increasing the value of k.
Doubling the concentration of X will increase the rate more than doubling the concentration of Y
Doubling the concentration of Y will increase the rate of reaction but no effect the value of k.
Doubling the concentration of Y will have no effect on the rate of reaction and no effect the value of k.
NO + O3 → NO2 + O2
The rate law for the reaction shown is rate = k[NO]0[O3]1. Which of the following mixtures of NO and O3 gas has the fastest initial rate?
A mechanism for the decomposition of ozone,
2 O3(g) → 3 O2(g)
is
Step 1: O3 → O2 + O
Step 2: O + O3 → O2 + O2
What is the molecularity for the first and second elementary reactions?
Step 1:
Unimolecular
Step 2:
Bimolecular
Step 1:
Bimolecular
Step 2:
Bimolecular
Step 1:
Termolecular
Step 2:
Quadmolecular
Step 1:
Unimolecular
Step 2:
Unimolecular
Consider the reaction
2 NO2(g) + F2(g) → 2 NO2F(g)
Select ALL of the proper expression(s) for the rate of this reaction?
The reaction pathways below represent the same reaction at the same temperature. Which represents the reaction in the presence of a catalyst?
If 93.75 percent of a sample of pure 209Po decays in 40 days, what is the half-life of 209Po?
10 days
40 days
20 days
160 days
