Deck 13: Chemical Kinetics

Question 1

A sample of 0.200 moles of NO and 0.300 moles of Cl₂ are placed in a 1.00 liter vessel at 400 K. The reaction 2 NO + Cl₂→2 NOCl occurs and after 5 seconds measurements show that the [Cl₂] has decreased to 0.290 M . Calculate D [NOCl]/ D t for this time interval, in units of mol/L × s.

A) 0.0040
B) - 0.0020
C) 0.0010
D) 0.0020
E) - 0.0040

Answer 1

0.0040

Question 2

Exhibit 13-2 Use the data set below for the reaction of C₄H₉Cl with water to answer the following question(s). C₄H₉Cl + H₂O→C₄H₉OH + HCl
Refer to Exhibit 13-2. What is the average rate of reaction over the time interval from 0.0 seconds to 800.0 seconds?

A) 0.56×10 ^{- 4} M/s
B) 1.00×10 ^{- 4} M/s
C) 1.23×10 ^{- 4} M/s
D) 1.27×10 ^{- 4} M/s
E) 1.31×10 ^{- 4} M/s

Answer 2

1.00×10 ^{- 4} M/s

Question 3

Exhibit 13-3 Consider the following reaction and the corresponding time-concentration table to answer the following question(s). C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g) The concentration of ozone, O₃, was monitored for this reaction as a function of time and is given in the table that follows
Refer to Exhibit 13-3. What is the average rate for the time interval from 20.0 seconds tO₆0.0 seconds?

A) 2.13×10 ^{- 7} M/s
B) 3.5×10 ^{- 7} M/s
C) 3.66×10 ^{- 7} M/s
D) 1.83×10 ^{- 6} M/s
E) 1.40×10 ^{- 5} M/s

Answer 3

2.13×10 ^{- 7} M/s

Question 4

Exhibit 13-3 Consider the following reaction and the corresponding time-concentration table to answer the following question(s). C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g) The concentration of ozone, O₃, was monitored for this reaction as a function of time and is given in the table that follows.
Refer to Exhibit 13-3. What is the average rate for the time interval from 10.0 seconds tO₅ 0.0 seconds?

A) 2.98×10 ^{- 7} M/s
B) 9.13×10 ^{- 7} M/s
C) 1.63×10 ^{- 5} M/s
D) 1.73×10 ^{- 5} M/s
E) 1.83×10 ^{- 5} M/s

Question 5

Exhibit 13-2 Use the data set below for the reaction of C₄H₉Cl with water to answer the following question(s). C₄H₉Cl + H₂O→C₄H₉OH +HCl
Refer to Exhibit 13-2. What is the average rate of reaction over the time interval from 150.0 seconds to 300.0 seconds?

A) 3.80×10 ^{- 5} M/s
B) 1.01×10 ^{- 4} M/s
C) 3.36×10 ^{- 4} M/s
D) 1.28×10 ^{- 4} M/s
E) 1.60×10 ^{- 4} M/s

Question 6

Which of the following would increase the rate of the following reaction?
C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g)
I. Add more O₃ to this reaction.
II. Decrease the temperature.
III. Add a catalyst.

A) I only
B) I and II
C) I and III
D) II and III
E) All of these

Question 7

Exhibit 13-3 Consider the following reaction and the corresponding time-concentration table to answer the following question(s). C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g) The concentration of ozone, O₃, was monitored for this reaction as a function of time and is given in the table that follows
Refer to Exhibit 13-3. What is the average rate for the time interval from 20.0 seconds tO₆0.0 seconds?

A) 2.13×10 ^{- 7} M/s
B) 3.5×10 ^{- 7} M/s
C) 3.66×10 ^{- 7} M/s
D) 1.83×10 ^{- 6} M/s
E) 1.40×10 ^{- 5} M/s

Question 8

Exhibit 13-2 Use the data set below for the reaction of C₄H₉Cl with water to answer the following question(s). C₄H₉Cl + H₂O→C₄H₉OH + HCl
Refer to Exhibit 13-2. What is the average rate of reaction over the time interval from 50.0 seconds tO₅ 00.0 seconds?

A) 0.560×10 ^{- 4} M/s
B) 0.800×10 ^{- 4} M/s
C) 1.13×10 ^{- 4} M/s
D) 1.19×10 ^{- 4} M/s
E) 1.70×10 ^{- 4} M/s

Question 9

Consider the reaction in aqueous solution:
3 I ^- + S₂O₈^{2 -} →I₃ ^- + 2 SO₄^{2 -} . Under a given set of conditions, the concentration of I₃ ^- changes from 0 to 7.6×10 ^{- 4} M in 20 seconds. Calculate D [I ^- ]/ D t (in mol/L × s) for this time interval.

A) 3.8×10 ^{- 5}
B) - 2.5×10 ^{- 5}
C) - 3.8×10 ^{- 5}
D) - 1.1×10 ^{- 4}
E) 7.6×10 ^{- 5}

Question 10

Exhibit 13-2 Use the data set below for the reaction of C₄H₉Cl with water to answer the following question(s). C₄H₉Cl + H₂O→C₄H₉OH + HCl
Refer to Exhibit 13-2. What is the average rate of reaction over the time interval from 100.0 seconds tO₄00.0 seconds?

A) 0.800×10 ^{- 4} M/s
B) 1.01×10 ^{- 4} M/s
C) 1.20×10 ^{- 4} M/s
D) 1.24×10 ^{- 4} M/s
E) 1.60×10 ^{- 4} M/s

Question 11

The diagram below is a time-concentration curve for the reaction CO₂ (g) C (s) + O₂(g). What is the average rate at which CO₂ (g) disappears over the first 25 minutes of the reaction?

A) 0.34 mol/L × min
B) 0.17 mol/L × s
C) 0.04 mol/L × min
D) 0.68 mol/L × hr
E) 0.014 mol/L × min

Question 12

The following are factors that influence the rate of a reaction. Which are stated correctly?
I. The rate increases when the concentration of reactants decreases.
II. The rate increases when a catalyst is added.
III. The rate increases when the temperature increases.

A) I only
B) I and II
C) I and III
D) II and III
E) All of these

Question 13

The rate of a chemical reaction may be influenced by:

A) temperature.
B) concentrations of substances.
C) nature or composition of the substances.
D) stirring the reaction.
E) all of these.

Question 14

Exhibit 13-3 Consider the following reaction and the corresponding time-concentration table to answer the following question(s). C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g) The concentration of ozone, O₃, was monitored for this reaction as a function of time and is given in the table that follows.
Refer to Exhibit 13-3. What is the average rate for the time interval from 40.0 seconds tO₆0 seconds?

A) 1.50×10 ^{- 7} M/s
B) 6.25×10 ^{- 7} M/s
C) 1.10×10 ^{- 5} M/s
D) 1.25×10 ^{- 5} M/s
E) 1.40×10 ^{- 5} M/s

Question 15

Exhibit 13-1 This graph shows the concentration vs. time data needed for the following question(s).
Refer to Exhibit 13-1. What is the average rate at which concentration decreases, measured between 10 and 30 seconds?

A) 530 mol/L × s
B) 1.9×10 ^{- 3} mol/L × s
C) - 1.9×10 ^{- 4} mol/L × s
D) - 530 mol/L × s
E) cannot answer from the data given

Question 16

Exhibit 13-3 Consider the following reaction and the corresponding time-concentration table to answer the following question(s). C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g) The concentration of ozone, O₃, was monitored for this reaction as a function of time and is given in the table that follows.
Refer to Exhibit 13-3. What is the average rate for the time interval from 0.00 seconds tO₅ 0.0 seconds?

A) 3.94×10 ^{- 7} M/s
B) 8.86×10 ^{- 7} M/s
C) 1.17×10 ^{- 5} M/s
D) 2.22×10 ^{- 5} M/s
E) 3.18×10 ^{- 5} M/s

Question 17

Exhibit 13-3 Consider the following reaction and the corresponding time-concentration table to answer the following question(s). C₂H₄ (g) + O₃ (g)→C₂H₄O (g) + O₂ (g) The concentration of ozone, O₃, was monitored for this reaction as a function of time and is given in the table that follows
Refer to Exhibit 13-3. What is the average rate for the time interval from 10.0 seconds tO₅ 0.0 seconds?

A) 2.98×10 ^{- 7} M/s
B) 9.13×10 ^{- 7} M/s
C) 1.63×10 ^{- 5} M/s
D) 1.73×10 ^{- 5} M/s
E) 1.83×10 ^{- 5} M/s

Question 18

Exhibit 13-1 This graph shows the concentration vs. time data needed for the following question(s).
Refer to Exhibit 13-1. What is the instantaneous rate at which concentration decreases at 30 s?

A) - 1.1×10 ^{- 4} mol/L × s
B) - 1.1×10 ^{- 2} mol/L × s
C) 1.1×10 ^{- 3} mol/L × s
D) 893 mol/L × s
E) cannot answer from the data given

Question 19

The rate of reaction is influenced by:

A) concentration of the reactants.
B) temperature.
C) time.
D) none of these.
E) more than one of these.

Question 20

Oxygen gas is formed by the following reaction:
2 NO (g)→O₂ (g) + N₂ (g). If during a given time period the rate of formation of O₂ is 0.054 mol/L × s, what is D [NO]/ D t in mol/L × s?

A) 0.054
B) - 0.054
C) 0.11
D) - 0.11
E) - 0.027

Question 21

Which units listed below is the best choice for a rate constant, k , of a second order rate law?
Rate = k [A]²

A) M/sec
B) M²/sec²
C) M ^{- 1}sec ^{- 1}
D) 1/sec
E) M ^{- 2}sec ^{- 1}

Question 22

What units would be used for the rate constant , k , of a third order rate law ?

A) M/sec
B) M³/sec³
C) M ^{- 1}sec ^{- 1}
D) 1/sec
E) M ^{- 2}sec ^{- 1}

Question 23

Consider the following reaction. 3 O₂ (g)→2 O₃ (g) At a given instant, the rate of disappearance of [O₂] is 2.35×10 ^{- 5} M/sec. What is the rate of appearance of [O₃] for this reaction at this moment?

A) 1.57×10 ^{- 5} M/sec
B) 2.35×10 ^{- 5} M/sec
C) 3.53×10 ^{- 5} M/sec
D) 4.70×10 ^{- 5} M/sec
E) 7.05×10 ^{- 5} M/sec

Question 24

Consider the following unbalanced reaction :
NO (g) + O₂ (g)→N₂O₃ (g) After balancing this reaction, how fast is [O₂] decreasing when [NO] is decreasing at a rate of 1.60×10 ^{- 4} mol/L × sec?

A) 4.0×10 ^{- 5} mol/L × sec
B) 8.0×10 ^{- 5} mol/L × sec
C) 1.6×10 ^{- 4} mol/L × sec
D) 3.2×10 ^{- 4} mol/L × sec
E) 6.4×10 ^{- 4} mol/L × sec

Question 25

Consider the combustion of methane as shown below:
CH₄ (g) + 2 O₂ (g)→CO₂ (g) + 2 H₂O (g) What is the rate expression for each substance in this equation?

A) Rate = -D [CH₄]/ D t = -D [O₂]/ D t = D [CO₂]/ D t = D [H₂O]/ D t
B) Rate = -D [CH₄]/ D t = -D [O₂]/2 D t = D [CO₂]/ D t = D [H₂O]/2 D t
C) Rate = D [CH₄]/ D t = D [O₂]/ D t = -D [CO₂]/ D t = -D [H₂O]/ D t
D) Rate = -D [CH₄]/ D t = - 2 D [O₂]/ D t = D [CO₂]/ D t = 2 D [H₂O]/ D t
E) Rate = -D [CH₄]/2 D t = - 2 D [O₂]/ D t = D [CO₂]/2 D t = 2 D [H₂O]/ D t

Question 26

Consider the following reaction:
N₂ (g) + 3 H₂ (g)→2 NH₃ (g) What is the rate expression for each substance in this equation?

A) Rate = D [N₂]/ D t = D [H₂]/ D t = D [NH₃]/ D t
B) Rate = D [N₂]/ D t = D [H₂]/3 D t = D [NH₃]/2 D t
C) Rate = -D [N₂]/ D t = -D [H₂]/3 D t = D [NH₃]/2 D t
D) Rate = D [N₂]/ D t = 3 D [H₂]/ D t = - 2 D [NH₃]/ D t
E) Rate = -D [N₂]/ D t = - 3 D [H₂]/ D t = 2 D [NH₃]/ D t

Question 27

Exhibit 13-4 Use the information below for the reaction 2 A + B→C to answer the following question(s). Initial rates were measured at different molar concentrations.
Refer to Exhibit 13-4. What is the order of this reaction in [B]?

A) 1
B) 2
C) 0
D) - 1
E) none of these

Question 28

If the unit for a particular rate constant is M ^{- 1}sec ^{- 1}, what is the order of the rate law?

A) zero order
B) 1^st order
C) 2^nd order
D) 3^rd order
E) - 1 order

Question 29

Exhibit 13-4 Use the information below for the reaction 2 A + B→C to answer the following question(s). Initial rates were measured at different molar concentrations
Refer to Exhibit 13-4. What is the order of this reaction in [A]?

A) 1
B) 2
C) 0
D) - 1
E) none of these

Question 30

Consider the following unbalanced reaction :
NO (g) + O₂ (g)→N₂O₃ (g) After balancing this reaction, how is the rate expressions for each substance in this equation related?

A) Rate = D [NO]/ D t = D [O₂]/ D t = D [N₂O₃]/ D t
B) Rate = -D [NO]/ D t = -D [O₂]/3 D t = D [N₂O₃]/2 D t
C) Rate = - 2 D [NO]/ D t = -D [O₂]/3 D t = D [N₂O₃]/2 D t
D) Rate = 4 D [NO]/ D t = D [O₂]/ D t = - 2 D [N₂O₃]/ D t
E) Rate = -D [NO]/4 D t = -D [O₂]/ D t = D [N₂O₃]/2 D t

Question 31

If the reaction A + B→C has the rate law:
Rate = k [A]²[B], the units of the rate constant are:

A) s ^{- 1}
B) mol/L × s
C) L/mol × s
D) L²/mol² × s
E) L³/mol³ × s

Question 32

Consider the following unbalanced reaction :
NO (g) + O₂ (g)→N₂O₃ (g) How fast is N₂O₃ being formed when the [NO] is disappearing at a rate of 3.2×10 ^{- 4} M/s?

A) 4.0×10 ^{- 5} M/s
B) 1.6×10 ^{- 4} M/s
C) 3.2×10 ^{- 4} M/s
D) 6.4×10 ^{- 4} M/s
E) 2.6×10 ^{- 3} M/s

Question 33

The reaction A + B→C gave the following initial rate data:
Rate [A] [B] (mol/L × s) 0.03 0.03 3.0×10 ^{- 4} 0.06 0.06 1.2×10 ^{- 3} 0.06 0.09 2.7×10 ^{- 3} The rate law for this reaction is:
Rate =

A) k [B]²
B) k [A][B]²
C) k [A][B] ^{- 3}
D) k [A]²
E) k [A]²[B]

Question 34

For the aqueous reaction 2 Cr³⁺ + 3 IO₄ ^- + 10 OH ^- →2 CrO₄^{2 -} + 3 IO₃ ^- + 5 H₂O, under a given set of conditions, the rate of appearance of CrO₄^{2 -} is 3.0×10 ^{- 4} mol/L × s. What is the rate of disappearance of IO₄ ^- ?

A) 2.0×10 ^{- 4} mol/L × s
B) 3.0×10 ^{- 4} mol/L × s
C) 4.5×10 ^{- 4} mol/L × s
D) 6.0×10 ^{- 4} mol/L × s
E) none of these

Question 35

The decomposition of N₂O₅ proceeds according to the following equation:
2 N₂O₅ (g)→4 NO₂ (g) + O₂ (g) If the rate of decomposition of N₂O₅ at a particular instant in a reaction vessel is 5.3×10 ^{- 5} M/s, what is the rate of appearance of NO₂?

A) 5.3×10 ^{- 5} M/s
B) 2.7×10 ^{- 5} M/s
C) 1.1×10 ^{- 4} M/s
D) 1.3×10 ^{- 5} M/s
E) 2.1×10 ^{- 4} M/s

Question 36

Consider the conversion of oxygen, O₂, to ozone, O₃, as shown below:
3 O₂ (g)→2 O₃ (g) How is the rate expression for oxygen related to the rate expression for ozone?

A) Rate = -D [O₂]/ D t = D [O₃]/ D t
B) Rate = -D [O₂]/2 D t = D [O₃]/3 D t
C) Rate = -D [O₂]/3 D t = D [O₃]/2 D t
D) Rate = - 3 D [O₂]/ D t = 2 D [O₃]/ D t
E) Rate = 3 D [O₂]/ D t = - 2 D [O₃]/2 D t

Question 37

Exhibit 13-5 Use the data below for NO + Cl₂→NOCl₂ to answer the following question(s):

Refer to Exhibit 13-5. The order in Cl₂ is:

A) 1
B) 2
C) 3
D) zero
E) none of these

Question 38

Exhibit 13-5 Use the data below for NO + Cl₂→NOCl₂ to answer the following question(s):

Refer to Exhibit 13-5. The order in NO is:

A) 1
B) 2
C) 3
D) zero
E) none of these

Question 39

For the reaction 2 O₃ (g)→3 O₂ (g), under a given set of conditions the rate of appearance of O₂ is 6.1×10 ^{- 5} mol/L × s. What is the rate of the disappearance of O₃ under the same conditions?

A) 2.0×10 ^{- 5} mol/L × s
B) 4.1×10 ^{- 5} mol/L × s
C) 1.2×10 ^{- 4} mol/L × s
D) 6.1×10 ^{- 5} mol/L × s
E) none of these

Question 40

Exhibit 13-4 Use the information below for the reaction 2 A + B→C to answer the following question(s). Initial rates were measured at different molar concentrations.
Refer to Exhibit 13-4. What units are appropriate for the specific rate constant in the rate law?

A) L/mol × s
B) s ^{- 1}
C) mol/L × s
D) The rate constant is dimensionless.
E) none of these

Question 41

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-8. Which units listed below is the best choice for the rate constant, k , of the reaction above?

A) M/sec
B) M²/sec²
C) M ^{- 1}sec ^{- 1}
D) 1/sec
E) M ^{- 2}sec ^{- 1}

Question 42

Exhibit 13-6 The following question(s)
Refer to the table of experimental initial rate data below.
Refer to Exhibit 13-6. The overall order of the reaction is:

A) 1st
B) 2nd
C) 3rd
D) 4th
E) zero

Question 43

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-8. What is the rate law for this reaction?

A) Rate = k [NO₂][CO]
B) Rate = k [NO₂][CO]²
C) Rate = k [NO₂]²[CO]
D) Rate = k [NO₂]²[CO]²
E) Rate = k [NO₂]²

Question 44

A reaction follows the rate law:
The overall order of the reaction is:

A) 1st
B) 2nd
C) 3rd
D) impossible rate law
E) none of these

Question 45

Exhibit 13-7 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-7. What is the overall order of the rate law above?

A) zero order
B) first order
C) second order
D) third order
E) fourth order

Question 46

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-8. What is the overall order of the rate law above?

A) zero order
B) first order
C) second order
D) third order
E) fourth order

Question 47

For NO + NO₂ + O₂→NO₃ + NO₂, the initial rate data in the table were collected. Initial Rate Expt. No. [NO], ( M ) [NO₂], ( M ) [O₂], ( M ) (mol/L × s) 1 1.0 0.5 0.1 0.250 2 2.0 0.5 0.1 0.500 3 2.0 1.0 0.1 2.00 4 2.0 0.5 0.2 0.500 5 2.0 2.0 0.2 8.00 The order of the reaction with respect to each reactant is:
NO NO₂ O₂

A) 1st 2nd 0
B) 1st 1st 1st
C) 2nd 1st 2nd
D) 0 0 1st
E) 1st 2nd 2nd

Question 48

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-8. What is the numerical value for the rate constant, k , of the reaction above?

A) 5.0×10 ^{- 5}
B) 0.50
C) 2.0
D) 5.0
E) 50

Question 49

Exhibit 13-7 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-7. What is the initial rate of this reaction when the concentration of the two reactants are [BF₃] = 0.500 M and [NH₃] = 0.500 M?

A) 0.213 M/sec
B) 0.25 M/sec
C) 0.426 M/sec
D) 0.852 M/sec
E) 3.41 M/sec

Question 50

The reaction CO + Cl₂→COCl₂ was studied by the initial rate method and the following data were obtained:
The rate law is:

A) Rate = k [CO][Cl₂]
B) Rate = k [CO][Cl₂]^1/2
C) Rate = k [CO]²[Cl₂]
D) Rate = k [CO][Cl₂]²
E) Rate = k [Cl₂]

Question 51

The following table of data was obtained for the gas phase reaction:
What is the rate law?

A) Rate =
B) Rate =
C) Rate =
D) Rate =
E) Rate =

Question 52

Exhibit 13-7 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-7. What is the numerical value for the rate constant, k , of the reaction above?

A) 0.852
B) 3.41
C) 13.6
D) 54.5
E) 109

Question 53

Exhibit 13-6 The following question(s)
Refer to the table of experimental initial rate data below.
Refer to Exhibit 13-6. The value of the rate constant is:

A) 0.033
B) 0.11
C) 0.26
D) 0.33
E) 3.3

Question 54

For H₂O₂ + 3 I ^- + 2 H⁺→2 H₂O + I₃ ^- , the effect on the rate of reaction brought about by doubling the concentration of I ^- without changing the other concentrations would be:

A) increase by a factor of 3.
B) increase by a factor of 8.
C) decrease by a factor of 1/3.
D) increase by a factor of 9.
E) cannot be determined from information given.

Question 55

The following table of initial rate data was obtained for: The rate law is:

A) Rate = k [MnO₄^{2 -} ]²
B) Rate = k [H₃IO₆^{2 -} ]
C) Rate = k [MnO₄^{2 -} ]²[H₃IO₆^{2 -} ]
D) Rate = k [MnO₄^{2 -} ][H₃IO₆^{2 -} ]
E) none of these

Question 56

What is the overall reaction order for the reaction that obeys the rate law below?
Rate = k [O₃]²[O₂] ^{- 1}

A) 1
B) 2
C) 3
D) 0
E) - 1

Question 57

Exhibit 13-7 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-7. What is the rate law for this reaction?

A) Rate = k [BF₃][NH₃]
B) Rate = k [F₃BNH₃]
C) Rate = k [BF₃]²[NH₃]
D) Rate = k [BF₃]²[NH₃]²
E) Rate = k [BF₃]²

Question 58

Exhibit 13-7 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-7. Which units listed below is the best choice for the rate constant, k , of the reaction above?

A) M/sec
B) M²/sec²
C) M ^{- 1}sec ^{- 1}
D) 1/sec
E) M ^{- 2}sec ^{- 1}

Question 59

The reaction 2 O₃→3 O₂ has the rate law:
Rate = k [O₃]²[O₂] ^{- 1} Calculate k , given that the rate of the reaction is 2.8×10 ^{- 4} mol/L × s for the initial concentrations [O₃]_o = 0.050 M and [O₂]_o = 0.010 M .

A) 1.1×10 ^{- 3} s ^{- 1}
B) 5.6×10 ^{- 5} s ^{- 1}
C) 5.6×10 ^{- 7} s ^{- 1}
D) 1.4×10 ^{- 3} s ^{- 1}
E) 7.0×10 ^{- 9} s ^{- 1}

Question 60

The following initial rate data were collected for the reaction:
The rate law is:

A) Rate = k [No]²[H₂]²
B) Rate = k [NO][H₂]
C) Rate = k [NO]²[H₂]
D) Rate = k [NO][H₂]²
E) Rate = k [NO]²[H₂]²

Question 61

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s). 2 NO (g) + O₂ (g)→2 NO₂ (g)
Refer to Exhibit 13-10. What is the overall order of the rate law above?

A) zero order
B) first order
C) second order
D) third order
E) fourth order

Question 62

If the overall chemical reaction A + B→C + D is studied and found to have the rate law:
Rate = k [A]², which statement is correct?

A) A plot of log[A] vs. time gives a straight line.
B) A plot of 1/[A] vs. time gives a straight line.
C) A plot of [A] vs. time gives a straight line.
D) The above is an impossible rate law.
E) A plot of 2.30 log vs. time gives a straight line.

Question 63

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s). 2 NO (g) + 2 H₂ (g)→N₂ (g) + 2 H₂O (g)
Refer to Exhibit 13-11. What is the rate law for this reaction?

A) Rate = k [NO]²[H₂]²
B) Rate = k [NO]²[H₂]¹
C) Rate = k [NO]¹[H₂]²
D) Rate = k [NO]¹[H₂]¹
E) Rate = k [NO]²

Question 64

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq)→2 Cl ^- (aq) + 2 CO₂ (g) + HgCl₂ (s)
Refer to Exhibit 13-12. What units would be used for the rate constant for the reaction above?

A) M/sec
B) M²/sec²
C) M ^{- 1}sec ^{- 1}
D) 1/sec
E) M ^{- 2}sec ^{- 1}

Question 65

Exhibit 13-9 Use the reaction below to answer the following question(s). Phosgene is a toxic gas prepared by the reaction of carbon monoxide with chlorine:
CO (g) + Cl₂ (g)→COCl₂ (g) The following data were obtained in a kinetic study of its formation.
Refer to Exhibit 13-9. What is the overall order of the rate law for this reaction?

A) zero order
B) first order
C) second order
D) third order
E) fourth order

Question 66

Graphical analysis can be used to determine the rate law for a general reaction of reactant "A" going to product "B". Which function of the molar concentration of reactant "A" when plotted versus time is associated with a second order rate law?

A) [A]
B) 1/[A]
C) ln[A]
D) [A]²
E) ln[A]²

Question 67

Consider the Integral Time-Concentration plots for each of the following:
Zero, first and second order rate laws. Which of these plots have a negative slope ?
I. Zero order rate law
II. First order rate law
III. Second order rate law

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 68

Exhibit 13-9 Use the reaction below to answer the following question(s). Phosgene is a toxic gas prepared by the reaction of carbon monoxide with chlorine:
CO (g) + Cl₂ (g)→COCl₂ (g) The following data were obtained in a kinetic study of its formation.
Refer to Exhibit 13-9. Using Experiment 3 data, what is the numerical value for the rate constant , k , for this reaction?

A) k = 4.81×10 ^{- 30}
B) k = 1.44×10 ^{- 29}
C) k = 1.60×10 ^{- 29}
D) k = 4.81×10 ^{- 29}
E) k = 6.92×10²⁸

Question 69

Exhibit 13-9 Use the reaction below to answer the following question(s). Phosgene is a toxic gas prepared by the reaction of carbon monoxide with chlorine:
CO (g) + Cl₂ (g)→COCl₂ (g) The following data were obtained in a kinetic study of its formation.
Refer to Exhibit 13-9. What is the rate law for this reaction?

A) Rate = k [CO][Cl₂][COCl₂]
B) Rate = k [CO][Cl₂]
C) Rate = k [CO]²[Cl₂]
D) Rate = k [CO] [Cl₂]²
E) Rate = k [CO]²[Cl₂]²

Question 70

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq)→2 Cl ^- (aq) + 2 CO₂ (g) + HgCl₂ (s)
Refer to Exhibit 13-12. What is the rate law for this reaction?

A) Rate = k [HgCl₂] [C₂O₄^{2 -} ]
B) Rate = k [HgCl₂]²[C₂O₄^{2 -} ]
C) Rate = k [HgCl₂] [C₂O₄^{2 -} ]²
D) Rate = k [HgCl₂]²[C₂O₄^{2 -} ]²
E) Rate = k [HgCl₂] [C₂O₄^{2 -} ]^1/2

Question 71

Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s).
Refer to Exhibit 13-8. What is the initial rate of this reaction when the concentration of the two reactants are [NO₂] = 0.500 M and [CO] = 0.25 M?

A) 0.063 M/sec
B) 0.13 M/sec
C) 0.50 M/sec
D) 0.63 M/sec
E) 2.0 M/sec

Question 72

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s). 2 NO (g) + O₂ (g)→2 NO₂ (g)
Refer to Exhibit 13-10. What is the numerical value for the rate constant, k , of the reaction above?

A) 2.3×10 ^{- 5}
B) 0.17
C) 0.83
D) 0.90
E) 1.1

Question 73

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq)→2 Cl ^- (aq) + 2 CO₂ (g) + HgCl₂ (s)
Refer to Exhibit 13-12. What is the initial rate for this reaction when the concentration of [HgCl₂] equals 0.18 M and that of C₂O₄^{2 -} equals 0.12 M?

A) 2.2×10 ^{- 5} M/sec
B) 2.5×10 ^{- 5} M/sec
C) 2.8×10 ^{- 5} M/sec
D) 3.1×10 ^{- 5} M/sec
E) 3.10×10 ^{- 5} M/sec

Question 74

Exhibit 13-11 Consider the data that were collected for the rate of disappearance of NO in the reaction below to answer the following question(s). 2 NO (g) + 2 H₂ (g)→N₂ (g) + 2 H₂O (g)
Refer to Exhibit 13-11. What is the value and units of the rate constant, k , for this reaction?

A) 0.062 M ^{- 1}s ^{- 1}
B) 0.62 M ^{- 2}s ^{- 1}
C) 6.2 M ^{- 3}s ^{- 1}
D) 1.2 M ^{- 2}sec ^{- 1}
E) 12 M ^{- 3}s ^{- 1}

Question 75

Exhibit 13-10 Consider the gas phase reaction and initial rate data below to answer the following question(s). 2 NO (g) + O₂ (g)→2 NO₂ (g)
Refer to Exhibit 13-10. What is the rate law for this reaction?

A) Rate = k [NO][O₂]
B) Rate = k [NO][O₂]²
C) Rate = k [NO]²[O₂]
D) Rate = k [NO]²[O₂]²
E) Rate = k [NO]²

Question 76

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq)→2 Cl ^- (aq) + 2 CO₂ (g) + HgCl₂ (s)
Refer to Exhibit 13-12. What is the numerical value of the rate constant , k , for the reaction above?

A) 5.0×10 ^{- 4}
B) 1.3×10 ^{- 3}
C) 7.9×10 ^{- 3}
D) 8.7×10 ^{- 3}
E) 5.3×10 ^{- 2}

Question 77

For a reaction with the rate law below:
Rate = k [A]

A) a plot of ln[A] vs. time gives a straight line.
B) a plot of 1/[A] vs. 1/time gives a straight line.
C) a plot of [A] vs. time gives a straight line.
D) a plot of 1/[A] vs. time gives a straight line.
E) a plot of log vs. 1/time gives a straight line.

Question 78

Exhibit 13-12 Consider the aqueous reaction and data below to answer the following question(s). 2 HgCl₂ (aq) + C₂O₄^{2 -} (aq)→2 Cl ^- (aq) + 2 CO₂ (g) + HgCl₂ (s)
Refer to Exhibit 13-12. What is the overall order of the rate law?

A) zero order
B) first order
C) second order
D) third order
E) fourth order

Question 79

Consider the Time-Concentration plots for each of the following:
Zero, first and second order rate laws. Which of these plots have a positive slope ?
I. Zero order rate law
II. First order rate law
III. Second order rate law

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 80

Exhibit 13-13 Graphical analysis can be used to determine the rate law for a general reaction of reactant "A" going to products "B" and "C".
A→B + C
Refer to Exhibit 13-13. Which of the Time-Concentration plots shown below would be expected if a particular reaction follows a second order rate law ?

A)
B)
C)
D)
E)