Question 1

The rate law for this reaction is rate = __________.

Accepted Answer

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

Question 2

Of the following, __________ will lower the activation energy for a reaction.

Accepted Answer

A) increasing the concentrations of reactants 
B) raising the temperature of the reaction 
C) adding a catalyst for the reaction 
D) removing products as the reaction proceeds 
E) increasing the pressure 
A) increasing the concentrations of reactants 
B) raising the temperature of the reaction 
C) adding a catalyst for the reaction 
D) removing products as the reaction proceeds 
E) increasing the pressure

Question 3

The rate constant for this reaction is __________ s-1.

Accepted Answer

A) 0.013 
B) 0.030 
C) 0.14 
D) 3.0 
E) 3.1 × 10-3 
A) 0.013 
B) 0.030 
C) 0.14 
D) 3.0 
E) 3.1 × 10-3

Question 4

The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

Accepted Answer

A) True 
 B)False

Question 5

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 6

The half-life for a first order rate law depends on the starting concentration.

Accepted Answer

A) True 
 B)False

Question 7

A particular first-order reaction has a rate constant of 1.35 × 102s-1 at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?

Accepted Answer

A) 9.56 × 103 
B) 2.85 × 104 
C) 576 
D) 4.33 × 1087 
E) 1.36 × 102 
A) 9.56 × 103 
B) 2.85 × 104 
C) 576 
D) 4.33 × 1087 
E) 1.36 × 102

Question 8

A particular first-order reaction has a rate constant of 1.35 × 102s-1 at 25.0°C. What is the magnitude of k at 75.0°C if Ea = 85.6 kJ/mol?

Accepted Answer

A) 3.47 × 104 
B) 1.92 × 104 
C) 670 
D) 3.85 × 106 
E) 1.36 × 102 
A) 3.47 × 104 
B) 1.92 × 104 
C) 670 
D) 3.85 × 106 
E) 1.36 × 102

Question 9

At elevated temperatures, methylisonitrile (CH3NC)isomerizes to acetonitrile (CH3CN): CH3NC (g)→ CH3CN (g)
At the start of an experiment, there are 0.200 mol of reactant and 0 mol of product in the reaction vessel. After 25 min, 0.106 mol of reactant (CH3NC)remain. There are __________ mol of product (CH3CN)in the reaction vessel.

Accepted Answer

A) 0.022 
B) 0.106 
C) 0.200 
D) 0.306 
E) 0.094 
A) 0.022 
B) 0.106 
C) 0.200 
D) 0.306 
E) 0.094

Question 10

A catalyst can increase the rate of a reaction __________.

Accepted Answer

A) by changing the value of the frequency factor (
A)  
B) by increasing the overall activation energy (Ea)of the reaction 
C) by lowering the activation energy of the reverse reaction 
D) by providing an alternative pathway with a lower activation energy 
E) All of these are ways that a catalyst might act to increase the rate of reaction. 
A) by changing the value of the frequency factor (
A)  
B) by increasing the overall activation energy (Ea)of the reaction 
C) by lowering the activation energy of the reverse reaction 
D) by providing an alternative pathway with a lower activation energy 
E) All of these are ways that a catalyst might act to increase the rate of reaction.

Question 11

A catalyst that is present in a different phase from the reacting molecules is called a __________ catalyst.

Accepted Answer

The answer of A catalyst that is present in a...

Question 12

The concentration of S2O82- remaining at 1600 s is __________ M.

Accepted Answer

A) 0.036 
B) 0.014 
C) 0.043 
D) 0.064 
E) 0.029 
A) 0.036 
B) 0.014 
C) 0.043 
D) 0.064 
E) 0.029

Question 13

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

Accepted Answer

A) True 
 B)False

Question 14

At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2 (g)→ NO (g)+   O2 (g)
The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1 at 300 °C. If the initial [NO2] is 0.260 M, it will take __________ s for the concentration to drop to 0.150 M.

Accepted Answer

A) 3.34 
B) 0.0880 
C) 1.01 
D) 0.299 
E) 5.19 
A) 3.34 
B) 0.0880 
C) 1.01 
D) 0.299 
E) 5.19

Question 15

The reaction A (aq)→ B (aq)is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds:   The rate constant for this reaction is __________ s-1.

Accepted Answer

A) 0.23 
B) 1.0 
C) 0.17 
D) 0.12 
E) -0.12 
A) 0.23 
B) 1.0 
C) 0.17 
D) 0.12 
E) -0.12

Question 16

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 17

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by __________.

Accepted Answer

The answer of The relationship of absorbed light to the...

Question 18

The earth's ozone layer is located in the __________.

Accepted Answer

The answer of The earth's ozone layer is located in...

Question 19

The mechanism for formation of the product X is: A + B → C + D (slow)
B + D → X (fast)
The intermediate reactant in the reaction is __________.

Accepted Answer

A) A 
B) B 
C) C 
D) D 
E) X 
A) A 
B) B 
C) C 
D) D 
E) X

Question 20

How many moles of B are present at 30 s?

Accepted Answer

A) 2.4 × 10-3 
B) 0.15 
C) 0.073 
D) 1.7 × 10-3 
E) 0.051 
A) 2.4 × 10-3 
B) 0.15 
C) 0.073 
D) 1.7 × 10-3 
E) 0.051

Exam 14: Chemical Kinetics

The rate law for this reaction is rate = __________.

Of the following, __________ will lower the activation energy for a reaction.

The rate constant for this reaction is __________ s-1.

The concentration of reactants or products at any time during the reaction can be calculated from the integrated rate law.

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 = __________.

The half-life for a first order rate law depends on the starting concentration.

A particular first-order reaction has a rate constant of 1.35 × 102s-1 at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?

A particular first-order reaction has a rate constant of 1.35 × 102s-1 at 25.0°C. What is the magnitude of k at 75.0°C if Ea = 85.6 kJ/mol?

A catalyst can increase the rate of a reaction __________.

A catalyst that is present in a different phase from the reacting molecules is called a __________ catalyst.

The concentration of S2O82- remaining at 1600 s is __________ M.

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

At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2 (g)→ NO (g)+ O2 (g) The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1 at 300 °C. If the initial [NO2] is 0.260 M, it will take __________ s for the concentration to drop to 0.150 M.

The reaction A (aq)→ B (aq)is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds: The rate constant for this reaction is __________ s-1.

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

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by __________.

The earth's ozone layer is located in the __________.

The mechanism for formation of the product X is: A + B → C + D (slow) B + D → X (fast) The intermediate reactant in the reaction is __________.

How many moles of B are present at 30 s?

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

The rate constant for this reaction is __________ s^-1.

A particular first-order reaction has a rate constant of 1.35 × 10²s^-1 at 25.0°C. What is the magnitude of k at 95.0°C if E_a = 55.5 kJ/mol?

A particular first-order reaction has a rate constant of 1.35 × 10²s^-1 at 25.0°C. What is the magnitude of k at 75.0°C if E_a = 85.6 kJ/mol?

The concentration of S₂O₈^2- remaining at 1600 s is __________ M.

The reaction A (aq)→ B (aq)is first order in [A]. A solution is prepared with [A] = 1.22 M. The following data are obtained as the reaction proceeds: The rate constant for this reaction is __________ s^-¹.