Question 1

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

Accepted Answer

A) True 
 B)False

Question 2

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

Accepted Answer

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

Question 3

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

Accepted Answer

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

Question 4

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 
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 5

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. 
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 6

The peroxydisulfate ion (SS1U1B12S1U1B0OS1U1B18S1U1B0S1U1P12-S1S1P0)reacts with the iodide ion in aqueous solution via the reaction:
SS1U1B12S1U1B0OS1U1B18S1U1B0S1U1P12-S1S1P0 (aq) + 3IS1U1P1-S1S1P0 → 2SOS1U1B14S1U1B0 (aq)+ IS1U1B13S1U1B0S1U1P1-S1S1P0 (aq)
An aqueous solution containing 0.050 M of SS1U1B12S1U1B0OS1U1B18S1U1B0S1U1P12-S1S1P0 ion and 0.072 M of IS1U1P1-S1S1P0 is prepared, and the progress of the reaction followed by measuring [IS1U1P1-S1S1P0]. 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.

Accepted Answer

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

Question 7

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 8

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

Accepted Answer

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

Question 9

The peroxydisulfate ion (SS1U1B12S1U1B0OS1U1B18S1U1B0S1U1P12-S1S1P0)reacts with the iodide ion in aqueous solution via the reaction:
SS1U1B12S1U1B0OS1U1B18S1U1B0S1U1P12-S1S1P0 (aq) + 3IS1U1P1-S1S1P0 → 2SOS1U1B14S1U1B0 (aq)+ IS1U1B13S1U1B0S1U1P1-S1S1P0 (aq)
An aqueous solution containing 0.050 M of SS1U1B12S1U1B0OS1U1B18S1U1B0S1U1P12-S1S1P0 ion and 0.072 M of IS1U1P1-S1S1P0 is prepared, and the progress of the reaction followed by measuring [IS1U1P1-S1S1P0]. 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.

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 
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 10

The data in the table below were obtained for the reaction:
2 ClOS1U1B12S1U1B0 (aq) + 2 OHS1U1P1-S1S1P0 (aq) → ClOS1U1B13S1U1B0S1U1P1-S1S1P0 (aq) + ClOS1U1B12S1U1B0S1U1P1-S1S1P0 (aq) + HS1U1B12S1U1B0O (1)  
-What is the order of the reaction with respect to OH-?

Accepted Answer

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

Question 11

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

Question 12

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.

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 
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 13

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.

Accepted Answer

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

Question 14

The data in the table below were obtained for the reaction:
2 ClOS1U1B12S1U1B0 (aq) + 2 OHS1U1P1-S1S1P0 (aq) → ClOS1U1B13S1U1B0S1U1P1-S1S1P0 (aq) + ClOS1U1B12S1U1B0S1U1P1-S1S1P0 (aq) + HS1U1B12S1U1B0O (1)  
-What is the order of the reaction with respect to ClO2?

Accepted Answer

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

Question 15

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 
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 16

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

Accepted Answer

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

Question 17

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.

Accepted Answer

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

Question 18

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 = ________.

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 
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 19

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

Question 20

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 
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

Exam 14: Chemical Kinetics

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

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

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

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

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

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

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

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-?

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.

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.

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.

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?

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 = ________.

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

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.

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 = ________.

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.

Nitrogen fixation is a difficult process because ________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

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

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^-?

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.

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.

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.

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?

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 = ________.