Question 1

The graph shown below depicts the relationship between concentration and time for the following chemical reaction. o D) -k E) 1/k" class="answers-bank-image d-inline" rel="preload" > The slope of this line is equal to ________.

Accepted Answer

A)  k
B)  -1/k
C)  ln [A]o
D)  -k
E)  1/k

Question 2

The binding of molecules to the surface of a catalyst is referred to as ________.

Accepted Answer

The answer of The binding of molecules to the surface...

Question 3

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2 (g)  → SO2 (g)  + Cl2 (g) 
The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10-6 s-1at 600 K. A vessel is charged with 3.6 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 s is ________ atm.

Accepted Answer

A)  0.85
B)  3.2
C)  1.5
D)  0.19
E)  9.3 × 104

Question 4

For the reaction aA + Bb → cC + dD, the rate law is ________.

Accepted Answer

The answer of For the reaction aA + Bb →...

Question 5

The reaction CH3-N≡C → CH3-C≡N
Is a first-order reaction. At 230.3 °C, k = 6.29 × 10-4s-1. If 3-N≡C → CH3-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10-4s-1. If   is 1.00 × 10-3 initially,   is ________ after 1.000 × 103 s. A) 5.33 × 10-4 B) 2.34 × 10-4 C) 1.88 × 10-3 D) 4.27 × 10-3 E) 1.00 × 10-6" class="answers-bank-image d-inline" rel="preload" > is 1.00 × 10-3 initially, 3-N≡C → CH3-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10-4s-1. If   is 1.00 × 10-3 initially,   is ________ after 1.000 × 103 s. A) 5.33 × 10-4 B) 2.34 × 10-4 C) 1.88 × 10-3 D) 4.27 × 10-3 E) 1.00 × 10-6" class="answers-bank-image d-inline" rel="preload" > is ________ after 1.000 × 103 s.

Accepted Answer

A)  5.33 × 10-4
B)  2.34 × 10-4
C)  1.88 × 10-3
D)  4.27 × 10-3
E)  1.00 × 10-6

Question 6

The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction:
S2O82- (aq)  + 3I- → 2SO4 (aq) + I3- (aq) 
An aqueous solution containing 0.050 M of S2O82- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. 2O82-) reacts with the iodide ion in aqueous solution via the reaction: S2O82- (aq)  + 3I- → 2SO4 (aq) + I3- (aq)  An aqueous solution containing 0.050 M of S2O82- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below.   -The average rate of disappearance of I- between 400.0 s and 800.0 s is ________ M/s. A) 2.8 × 10-5 B) 1.4 × 10-5 C) 5.8 × 10-5 D) 3.6 × 104 E) 2.6 × 10-4" class="answers-bank-image d-inline" rel="preload" >
-The average rate of disappearance of I- between 400.0 s and 800.0 s is ________ M/s.

Accepted Answer

A)  2.8 × 10-5
B)  1.4 × 10-5
C)  5.8 × 10-5
D)  3.6 × 104
E)  2.6 × 10-4

Question 7

The overall reaction order is the sum of the orders of each reactant in the rate law.

Accepted Answer

A) True 
 B)False

Question 8

Under constant conditions, the half-life of a first-order reaction ________.

Accepted Answer

A)  is the time necessary for the reactant concentration to drop to half its original value
B)  is constant
C)  can be calculated from the reaction rate constant
D)  does not depend on the initial reactant concentration
E)  All of the above are correct.

Question 9

If the rate law for the reaction 2A + 3B → products
Is first order in A and second order in B, then the rate law is rate = ________.

Accepted Answer

A)  k[A][B]
B)  k[A]2[B]3
C)  k[A][B]2
D)  k[A]2[B]
E)  k[A]2[B]2

Question 10

In general, as temperature goes up, reaction rate ________.

Accepted Answer

A)  goes up if the reaction is exothermic
B)  goes up if the reaction is endothermic
C)  goes up regardless of whether the reaction is exothermic or endothermic
D)  stays the same regardless of whether the reaction is exothermic or endothermic
E)  stays the same if the reaction is first order

Question 11

The data in the table below were obtained for the reaction:
2 ClO2 (aq)  + 2 OH- (aq)  → ClO3- (aq)  + ClO2- (aq)  + H2O (1)  2 (aq)  + 2 OH- (aq)  → ClO3- (aq)  + ClO2- (aq)  + H2O (1)    -What is the order of the reaction with respect to ClO2? A) 1 B) 0 C) 2 D) 3 E) 4" class="answers-bank-image d-inline" rel="preload" >
-What is the order of the reaction with respect to ClO2?

Accepted Answer

A)  1
B)  0
C)  2
D)  3
E)  4

Question 12

The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction:
S2O82- (aq)  + 3I- → 2SO4 (aq) + I3- (aq) 
An aqueous solution containing 0.050 M of S2O82- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. 2O82-) reacts with the iodide ion in aqueous solution via the reaction: S2O82- (aq)  + 3I- → 2SO4 (aq) + I3- (aq)  An aqueous solution containing 0.050 M of S2O82- ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below.   -The average rate of disappearance of I- in the initial 400.0 s is ________ M/s. A) 6.00 B) 3.8 × 10-5 C) 1.4 × 10-4 D) 2.7 × 104 E) 3.2 × 10-4" class="answers-bank-image d-inline" rel="preload" >
-The average rate of disappearance of I- in the initial 400.0 s is ________ M/s.

Accepted Answer

A)  6.00
B)  3.8 × 10-5
C)  1.4 × 10-4
D)  2.7 × 104
E)  3.2 × 10-4

Question 13

Nitrogen fixation is a difficult process because ________.

Accepted Answer

A)  there is so little nitrogen in the atmosphere
B)  nitrogen exists in the atmosphere primarily as its oxides which are very unreactive
C)  nitrogen is very unreactive, largely due to its triple bond
D)  of the extreme toxicity of nitrogen
E)  of the high polarity of nitrogen molecules preventing them from dissolving in biological fluids, such as those inside cells

Question 14

The reaction below is first order in [H2O2]: 2H2O2 (l)  → 2H2O (l)  + O2 (g) 
A solution originally at 0.600 M H2O2 is found to be 0.075 M after 54 min. The half-life for this reaction is ________ min.

Accepted Answer

A)  6.8
B)  18
C)  14
D)  28
E)  54

Question 15

A possible mechanism for the overall reaction Br2 (g)  + 2NO (g)  → 2NOBr (g) 
Is
NO (g)  + Br2 (g)  2 (g)  + 2NO (g)  → 2NOBr (g)  Is NO (g)  + Br2 (g)    NOBr2 (g) (fast)  NOBr2 (g)  + NO (g)    2NOBr (slow)  The rate law for formation of NOBr based on this mechanism is rate = ________. A) k1[NO]1/2 B) k1[Br2]1/2 C) (k2k1/k-1) [NO]2[Br2] D) (k1/k-1) 2[NO]2 E) (k2k1/k-1) [NO][Br2]2" class="answers-bank-image d-inline" rel="preload" > NOBr2 (g) (fast) 
NOBr2 (g)  + NO (g)  2 (g)  + 2NO (g)  → 2NOBr (g)  Is NO (g)  + Br2 (g)    NOBr2 (g) (fast)  NOBr2 (g)  + NO (g)    2NOBr (slow)  The rate law for formation of NOBr based on this mechanism is rate = ________. A) k1[NO]1/2 B) k1[Br2]1/2 C) (k2k1/k-1) [NO]2[Br2] D) (k1/k-1) 2[NO]2 E) (k2k1/k-1) [NO][Br2]2" class="answers-bank-image d-inline" rel="preload" > 2NOBr (slow) 
The rate law for formation of NOBr based on this mechanism is rate = ________.

Accepted Answer

A)  k1[NO]1/2
B)  k1[Br2]1/2
C)  (k2k1/k-1) [NO]2[Br2]
D)  (k1/k-1) 2[NO]2
E)  (k2k1/k-1) [NO][Br2]2

Question 16

At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN) : CH3NC (g)  → CH3CN (g) 
The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C. 3NC) isomerizes to acetonitrile (CH3CN) : CH3NC (g)  → CH3CN (g)  The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C.   The rate constant for the reaction is ________ s-1. A) -1.9 × 104 B) +1.9 × 104 C) -5.2 × 10-5 D) +5.2 × 10-5 E) +6.2" class="answers-bank-image d-inline" rel="preload" > The rate constant for the reaction is ________ s-1.

Accepted Answer

A)  -1.9 × 104
B)  +1.9 × 104
C)  -5.2 × 10-5
D)  +5.2 × 10-5
E)  +6.2

Question 17

The data in the table below were obtained for the reaction:
2 ClO2 (aq)  + 2 OH- (aq)  → ClO3- (aq)  + ClO2- (aq)  + H2O (1)  2 (aq)  + 2 OH- (aq)  → ClO3- (aq)  + ClO2- (aq)  + H2O (1)    -What is the order of the reaction with respect to OH-? A) 0 B) 1 C) 2 D) 3 E) 4" class="answers-bank-image d-inline" rel="preload" >
-What is the order of the reaction with respect to OH-?

Accepted Answer

A)  0
B)  1
C)  2
D)  3
E)  4

Question 18

Reaction rate data showing temperature dependence obey an equation devised by ________.

Accepted Answer

The answer of Reaction rate data showing temperature dependence obey...

Question 19

In the Arrhenius equation, k = Ae-Ea/RT
________ is the frequency factor.

Accepted Answer

A)  k
B)  A
C)  e
D)  Ea
E)  R

Question 20

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) →B(g) . The following data are obtained for [A] as the reaction proceeds: -3 B) 1.1 × 10-3 C) 4.4 × 10-3 D) 454 E) 9.90 × 10-3" class="answers-bank-image d-inline" rel="preload" >
-The average rate of disappearance of A between 10 s and 20 s is ________ mol/s.

Accepted Answer

A)  2.2 × 10-3
B)  1.1 × 10-3
C)  4.4 × 10-3
D)  454
E)  9.90 × 10-3

Exam 14: Chemical Kinetics

The reaction below is first order in [H₂O₂]: 2H₂O₂ (l) → 2H₂O (l) + O₂ (g) A solution originally at 0.600 M H₂O₂ is found to be 0.075 M after 54 min. The half-life for this reaction is ________ min.

Correct Answer
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Under constant conditions, the half-life of a first-order reaction ________.

Correct Answer
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A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) →B(g) . The following data are obtained for [A] as the reaction proceeds: -The average rate of disappearance of A between 10 s and 20 s is ________ mol/s.

Correct Answer
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Correct Answer
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Reaction rate data showing temperature dependence obey an equation devised by ________.

Correct Answer
verified

Nitrogen fixation is a difficult process because ________.

Correct Answer
verified

For the reaction aA + Bb → cC + dD, the rate law is ________.

Correct Answer
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The data in the table below were obtained for the reaction: 2 ClO₂ (aq) + 2 OH^- (aq) → ClO₃^- (aq) + ClO₂^- (aq) + H₂O (1) -What is the order of the reaction with respect to ClO₂?

Correct Answer
verified

The overall reaction order is the sum of the orders of each reactant in the rate law.

Correct Answer
verified

If the rate law for the reaction 2A + 3B → products Is first order in A and second order in B, then the rate law is rate = ________.

Correct Answer
verified

The binding of molecules to the surface of a catalyst is referred to as ________.

Correct Answer
verified

At elevated temperatures, methylisonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) : CH₃NC (g) → CH₃CN (g) The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C. The rate constant for the reaction is ________ s^-1.

Correct Answer
verified

Correct Answer
verified

In general, as temperature goes up, reaction rate ________.

Correct Answer
verified

In the Arrhenius equation, k = Ae^-Ea/RT ________ is the frequency factor.

Correct Answer
verified

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10^-4s^-1. If is 1.00 × 10^-3 initially, is ________ after 1.000 × 10³ s.

Correct Answer
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Correct Answer
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The graph shown below depicts the relationship between concentration and time for the following chemical reaction. The slope of this line is equal to ________.

Correct Answer
verified

The data in the table below were obtained for the reaction: 2 ClO₂ (aq) + 2 OH^- (aq) → ClO₃^- (aq) + ClO₂^- (aq) + H₂O (1) -What is the order of the reaction with respect to OH^-?

Correct Answer
verified

A possible mechanism for the overall reaction Br₂ (g) + 2NO (g) → 2NOBr (g) Is NO (g) + Br₂(g) NOBr₂ (g) (fast) NOBr₂(g) + NO (g) 2NOBr (slow) The rate law for formation of NOBr based on this mechanism is rate = ________.

Correct Answer
verified

Exam 14: Chemical Kinetics

The reaction below is first order in [H2O2]: 2H2O2 (l) → 2H2O (l) + O2 (g) A solution originally at 0.600 M H2O2 is found to be 0.075 M after 54 min. The half-life for this reaction is ________ min.

Correct AnswerverifiedShow Answer

Under constant conditions, the half-life of a first-order reaction ________.

Correct AnswerverifiedShow Answer

A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) →B(g) . The following data are obtained for [A] as the reaction proceeds: -The average rate of disappearance of A between 10 s and 20 s is ________ mol/s.

Correct AnswerverifiedShow Answer

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2 (g) → SO2 (g) + Cl2 (g) The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10-6 s-1at 600 K. A vessel is charged with 3.6 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 s is ________ atm.

Correct AnswerverifiedShow Answer

Reaction rate data showing temperature dependence obey an equation devised by ________.

Correct AnswerverifiedShow Answer

Nitrogen fixation is a difficult process because ________.

Correct AnswerverifiedShow Answer

For the reaction aA + Bb → cC + dD, the rate law is ________.

Correct AnswerverifiedShow Answer

The data in the table below were obtained for the reaction: 2 ClO2 (aq) + 2 OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (1) -What is the order of the reaction with respect to ClO2?

Correct AnswerverifiedShow Answer

The overall reaction order is the sum of the orders of each reactant in the rate law.

Correct AnswerverifiedShow Answer

If the rate law for the reaction 2A + 3B → products Is first order in A and second order in B, then the rate law is rate = ________.

Correct AnswerverifiedShow Answer

The binding of molecules to the surface of a catalyst is referred to as ________.

Correct AnswerverifiedShow Answer

At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN) : CH3NC (g) → CH3CN (g) The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C. The rate constant for the reaction is ________ s-1.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

In general, as temperature goes up, reaction rate ________.

Correct AnswerverifiedShow Answer

In the Arrhenius equation, k = Ae-Ea/RT ________ is the frequency factor.

Correct AnswerverifiedShow Answer

The reaction CH3-N≡C → CH3-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10-4s-1. If is 1.00 × 10-3 initially, is ________ after 1.000 × 103 s.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The graph shown below depicts the relationship between concentration and time for the following chemical reaction. The slope of this line is equal to ________.

Correct AnswerverifiedShow Answer

The data in the table below were obtained for the reaction: 2 ClO2 (aq) + 2 OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (1) -What is the order of the reaction with respect to OH-?

Correct AnswerverifiedShow Answer

A possible mechanism for the overall reaction Br2 (g) + 2NO (g) → 2NOBr (g) Is NO (g) + Br2 (g) NOBr2 (g) (fast) NOBr2 (g) + NO (g) 2NOBr (slow) The rate law for formation of NOBr based on this mechanism is rate = ________.

Correct AnswerverifiedShow Answer

The reaction below is first order in [H₂O₂]: 2H₂O₂ (l) → 2H₂O (l) + O₂ (g) A solution originally at 0.600 M H₂O₂ is found to be 0.075 M after 54 min. The half-life for this reaction is ________ min.

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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The data in the table below were obtained for the reaction: 2 ClO₂ (aq) + 2 OH^- (aq) → ClO₃^- (aq) + ClO₂^- (aq) + H₂O (1) -What is the order of the reaction with respect to ClO₂?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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At elevated temperatures, methylisonitrile (CH₃NC) isomerizes to acetonitrile (CH₃CN) : CH₃NC (g) → CH₃CN (g) The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C. The rate constant for the reaction is ________ s^-1.

Correct Answer
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Correct Answer
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Correct Answer
verified

In the Arrhenius equation, k = Ae^-Ea/RT ________ is the frequency factor.

Correct Answer
verified

The reaction CH₃-N≡C → CH₃-C≡N Is a first-order reaction. At 230.3 °C, k = 6.29 × 10^-4s^-1. If is 1.00 × 10^-3 initially, is ________ after 1.000 × 10³ s.

Correct Answer
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Correct Answer
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Correct Answer
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The data in the table below were obtained for the reaction: 2 ClO₂ (aq) + 2 OH^- (aq) → ClO₃^- (aq) + ClO₂^- (aq) + H₂O (1) -What is the order of the reaction with respect to OH^-?

Correct Answer
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A possible mechanism for the overall reaction Br₂ (g) + 2NO (g) → 2NOBr (g) Is NO (g) + Br₂(g) NOBr₂ (g) (fast) NOBr₂(g) + NO (g) 2NOBr (slow) The rate law for formation of NOBr based on this mechanism is rate = ________.

Correct Answer
verified