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Chemical Kinetics

Total questions: 60

Worksheet time: 2hrs 38mins

Name
Class
Date
1.

Which of the following plots will show a linear relationship for a second order reaction?

a)

[A] vs time

b)

1/[A] vs time

c)

ln[A] vs time

d)

[A]2 vs time

2.

The iodide ion reacts with hypochlorite ion in the following way:

OCl- + I- ⟶ OI- + Cl-.

This rapid reaction gives the rate data shown. What is the rate law?

a)

rate = [OCl-]2[I-]

b)

rate = [OCl-][I-]2

c)

rate = [OCl-][I-]

d)

rate = [OCl-]

3.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate law for the reaction?

a)

rate = k[NH3]

b)

rate = k[BF3]2[NH3]

c)

rate = k[BF3][NH3]

d)

rate = k[BF3][NH3]2

4.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?

a)

.01704 M/s

b)

.0852 M/s

c)

.1704 M/s

d)

.852 M/s

5.

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.

a)

doubles

b)

remains unchanged

c)

increases by a factor of 4

d)

is reduced by a factor of 2

6.

What letter represents the activation energy?

a)

A

b)

B

c)

C

d)

D

7.

Given the following rate law,

rate = k[A]2[B]

if [A] were doubled, what must happen to [B] to keep the rate constant?

a)

[B] must quadruple

b)

[B] must double

c)

[B] must be havled

d)

[B] must be quartered

8.

Which of the following best describes why increasing temperature increase reaction rate?

a)

Activation energy is reduced.

b)

Collisions become more frequent.

c)

Collisions become more energetic.

d)

Collisions become more frequent and more energetic.

9.

rate = k[A]

The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

a)

0.7 s

b)

1.4 s

c)

2.8 s

d)

There is not enough information given.

10.

Which species is the catalyst in this reaction mechanism?

a)

R

b)

W

c)

X

d)

There is no catalyst.

11.

What is the rate law for this mechanism?

a)

rate = k[A][B]2

b)

rate = [B][X]

c)

rate = [A]0.5[B]1.5

d)

rate = [W][Y][Z]

12.

The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences?

a)

I

b)

II

c)

III

d)

I and II

13.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing surface area

d)

all of the above

14.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
15.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
16.
Which of the following factors increases only the effectiveness of collisions?
a)
temperature
b)
catalysts
c)
concentration
d)
particle size
17.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
18.
Grinding a seltzer tablet into powder increases the rate of reaction due to...
a)
increased concentration of reactants
b)
increased surface area
c)
increased speed of particles.
d)
better orientation of reactants
19.

For second order reaction, the initial concentration of reactant A is 0.24 M. If the rate constant is 8.1 x 10-2 M-1 s-1, what is the concentration of A after 29 seconds?

a)

0.02 M

b)

0.15 M

c)

0.30 M

d)

0.45 M

20.

Given the following balanced equation :

2NO(g) + Cl2(g) → 2NOCl(g)

If the rate of disappearance of Cl2 is 4.84 x 10-2 Ms-1, what is the rate of disappearance of NO?

a)

1.45 x 10-2 Ms-1

b)

2.42 x 10-2 Ms-1

c)

3.67 x 10-2 Ms-1

d)

9.68 x 10-2 Ms-1

21.

The first order rate constant for the decomposition of 0.5 M compound A at 100oC is 0.03 min-1. Calculate the half-life of A.

a)

1.5 min

b)

8.3 min

c)

23.1 min

d)

66.7 min

22.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment 
23.

What does [ ] denote?

a)

concentration, M

b)

concentration, m

c)

concentration, mass %

d)

squared

24.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
25.
A chemical reaction that produces energy is a /an
a)
endothermic reaction
b)
exothermic reaction 
c)
energy
d)
chemical reaction 
26.
Do the reactants in an exothermic reaction have a higher or lower energy than the products?
a)
Higher
b)
Lower
27.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
28.
Which one of the following is a first order, overall reaction
a)
k1= 1.000 M s-1
b)
k1= 5403.2 M½ s½
c)
k1= 1.23 x 10-6 M-1 s-1
d)
k1= 10.7 s-1
29.
a)

A. is most exothermic

b)

B. is most exothermic

c)

C. is most exothermic

d)

D. is most exothermic

30.
a)
A. has largest Ea
b)
B. has largest Ea
c)
C. has largest Ea
d)
E. has largest Ea
31.
What would be my the overall order of this rate law? 
Rate=[A]2[B]1
a)
0 Order
b)
1st Order
c)
2nd Order
d)
3rd Order
32.
a)
A. is the slowest reaction
b)
B. is the slowest reaction
c)
C. is the slowest reaction
d)
E. is the slowest reaction
33.
For 2A + B → 2C, the rate of production of C has been found to be 12 M/s. During that reaction, the rate of reaction was?
a)
12 M/s
b)
24 M/s
c)
6 M/s
d)
Cannot tell without more data
34.
a)
A. is the fastest reaction
b)
B. is the fastest reaction
c)
C. is the fastest reaction
d)
E. is the fastest reaction
35.
step 1: O3 → O2 + O
step 2: O3 + O → 2 O2

The oxygen atom (O) is considered to be a(n)...
a)
reactant
b)
catalyst
c)
reaction intermediate
d)
activated complex
36.
The reaction of (CH3)3CBr with hydroxide ion proceeds:
(CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?
a)
0.003
b)
0.006
c)
0.009
d)
0.018
37.
In any first order reaction, as the reaction proceeds at constant temperature, which describes the corresponding effects on k (the rate constant) and rate?
a)
k remains the same; rate decreases
b)
k and rate both remain the same
c)
k remains the same; rate increases
d)
k decreases; rate remains the same
38.
a)
rate = k[CO]2[O2]2
b)
rate = k[CO]2[O2]
c)
rate = k[CO][O2]2
d)
rate = k[CO][O2]1/2
39.
a)
IO-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
b)
I-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
c)
IO-, because it was produced in an earlier step and used up in a subsequent step
d)
I-, because it was produced in an earlier step and used up in a subsequent step
40.

How does pressure affect reaction rate?

a)

Increased pressure increases reaction rate because particles collide more frequently

b)

Increased pressure increases reaction rate because particles collide less frequently

c)

Decreased pressure increases reaction rate because particles collide more frequently

d)

Decreased pressure increases reaction rate because particles collide less frequently.

41.

How does concentration affect reaction rate

a)

In all reactions, higher concentration increases the reaction rate because particles collide more frequently

b)

In all reactions, lower concentration increases the reaction rate because particles collide more frequently

c)

In a first order or higher reaction, higher concentration increases the reaction rate because particles collide more frequently

d)

In a first order or higher reaction, lower concentration increases the reaction rate because particles collide more frequently.

42.

In terms of collision theory, a reaction occurs when the molecules collide with sufficient energy to break the bonds already in place. What is this energy called?

a)

activation energy

b)

reaction mechanism

c)

activity series

d)

concentration gradient

43.

Overall reaction order can be determined how?

a)

Adding the powers to which reactant concentrations are raised in the rate law

b)

Multiplying the powers to which reactant concentrations are raised in the rate law

c)

Subtracting the powers to which reactant concentrations are raised in the rate law

d)

Dividing the powers to which reactant concentrations are raised in the rate law.

44.

Excess magnesium powder was added to a beaker containing hydrochloric acid, HCl (aq).

The mass of the beaker and its contents was recorded and plotted against time (line I).

Which change could give line II?

a)

Doubling the mass of powdered Mg

b)

Using the same mass of Mg ribbon

c)

Increasing the temperature

d)

Using the same volume of more concentrated HCl

45.

The diagram represents the Maxwell‒Boltzmann energy distribution curve of the reactants for a chemical reaction with different activation energies, Ea1 and Ea2.


What is the reason why the rate of the reaction with activation energy Ea2 is greater?

a)

More frequent collisions between the particles occur.

b)

More energetic collisions between the particles occur.

c)

A catalyst has been added.

d)

The temperature is higher.

46.

In which flask will the reaction between 2.0 g of magnesium carbonate and 25 mL 1.0 mol L–1 hydrochloric acid occur most rapidly?

a)

A

b)

B

c)

C

d)

D

47.

Which one of the following is a second order, overall reaction

a)

k1= 1.000 M s-1

b)

k1= 5403.2 M½ s½

c)

k1= 1.23 x 10-6 M-1 s-1

d)

k1= 10.7 s-1

48.

Which one of the following is a zero order, overall reaction

a)

k1= 1.000 M s-1

b)

k1= 5403.2 M½ s½

c)

k1= 1.23 x 10-6 M-1 s-1

d)

k1= 10.7 s-1

49.
What is the activation energy?
a)
40 kJ
b)
20 kJ
c)
100 kJ
d)
60 kJ
50.
What is the change of the heat of the reaction (ΔH)?
a)
40 kJ
b)
20 kJ
c)
100 kJ
d)
60 kJ
51.

Which group of particles shows that increasing surface area increases collisions among particles?

a)

Left side

b)

Right side

c)

Cannot be determined by either picture

52.
The order of N2 is
a)
Zero
b)
First
c)
Second
53.
a)
k[NO][Br2]
b)
k[NO]2 [Br2]
c)
k[NO]2
d)
k[Br2]
54.
In Mech II BrO is
a)
Catalyst
b)
Intermediate
55.

Consider the reaction between solid CaCO3 and aqueous HCl. The reaction will be speeded up by an increase in which of the stated conditions?

a)

I only

b)

I and III only

c)

II and III only

d)

I, II and III

56.

What would the rate constant of the reaction be given the following set of experiments?

a)
b)
c)
d)
57.

Using the following data, which is the correct rate law of the sample reaction?

A + 5B + 6C → 3D + 3E

a)
b)
c)
d)
58.
At higher temperature, 2000K, the curve is shifted to the right. Which of the following is true?
a)
fraction of molecules with energy > Ea increases
b)
fraction of molecules with energy > Ea decreases
c)
more particles under the curve
d)
less particles under the curve
59.
Which of the following is FALSE for Maxwell Boltzmann distribution curve?
a)
Area under curve represent number of particles
b)
Increase in temperature will shift the curve to right
c)
High temp, fraction of molecules with energy > Ea increases
d)
At higher temp, area under curve is greater than at low temp
60.

On a Maxwell-Boltzmann distribution curve, a suitable label for the y-axis is

a)

Fraction of particles with Kinetic Energy (E)

b)

Kinetic Energy (E)

c)

Activation Energy (Ea)

d)

Enthalpy

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