Question 1

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 2

The reaction A → B is first order in [A]. Consider the following data.   The rate constant for this reaction is ________ s-1.

Accepted Answer

A) 0.014 
B) 0.030 
C) 0.013 
D) 3.0 
E) 3.1 × 10-3 
A) 0.014 
B) 0.030 
C) 0.013 
D) 3.0 
E) 3.1 × 10-3

Question 3

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

Accepted Answer

A) True 
 B)False

Question 4

For the elementary reaction NO3 + CO → NO2 + CO2
The molecularity of the reaction is ________, and the rate law is

Accepted Answer

A) 2, k[NO3][CO] 
B) 4, k[NO3][CO][NO2][CO2] 
C) 2, k[NO2][CO2] 
D) 2, k[NO3][CO]/[NO2][CO2] 
E) 4, k[NO2][CO2]/[NO3][CO] 
A) 2, k[NO3][CO] 
B) 4, k[NO3][CO][NO2][CO2] 
C) 2, k[NO2][CO2] 
D) 2, k[NO3][CO]/[NO2][CO2] 
E) 4, k[NO2][CO2]/[NO3][CO]

Question 5

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 20 s and 40 s is ________ mol/s.

Accepted Answer

A) 8.5 × 10-4 
B) 1.7 × 10-3 
C) 590 
D) 7.1 × 10-3 
E) 1.4 × 10-3 
A) 8.5 × 10-4 
B) 1.7 × 10-3 
C) 590 
D) 7.1 × 10-3 
E) 1.4 × 10-3

Question 6

The reaction 2NO2 → 2NO + O2
Follows second-order kinetics. At 300 °C, [NO2] drops from 0.0100 M to 0.00650 M in 100.0 s. The rate constant for the reaction is ________ M-1s-1.

Accepted Answer

A) 0.096 
B) 0.65 
C) 0.81 
D) 1.2 
E) 0.54 
A) 0.096 
B) 0.65 
C) 0.81 
D) 1.2 
E) 0.54

Question 7

The concentration of S2O82- remaining at 800 s is ________ M.

Accepted Answer

A) 0.046 
B) 0.076 
C) 4.00 × 10-3 
D) 0.015 
E) 0.041 
A) 0.046 
B) 0.076 
C) 4.00 × 10-3 
D) 0.015 
E) 0.041

Question 8

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 magnitude of the rate constant for the reaction?

Accepted Answer

A) 1.15 × 104 
B) 4.6 
C) 230 
D) 115 
E) 713 
A) 1.15 × 104 
B) 4.6 
C) 230 
D) 115 
E) 713

Question 9

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 (g) → 2NO (g) + O2 (g)
In a particular experiment at 300 °C, [NO2] drops from 0.0100 to 0.00800 M in 100 s. The rate of appearance of O2 for this period is ________ M/s.

Accepted Answer

A) 1.0 × 10-5 
B) 2.0 × 10-5 
C) 4.0 × 10-5 
D) 2.0 × 10-3 
E) 4.0 × 10-3 
A) 1.0 × 10-5 
B) 2.0 × 10-5 
C) 4.0 × 10-5 
D) 2.0 × 10-3 
E) 4.0 × 10-3

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

The initial concentration of reactant in a first-order reaction is 0.27 M. The rate constant for the reaction is 0.75 s-1. What is the concentration (mol/L)of reactant after 1.8 s?

Accepted Answer

A) 6.0 
B) 1.7 
C) 0.070 
D) 0.012 
E) 1.0 
A) 6.0 
B) 1.7 
C) 0.070 
D) 0.012 
E) 1.0

Question 12

Reaction rates are affected by reactant concentrations and temperature. This is accounted for by the ________.

Accepted Answer

The answer of Reaction rates are affected by reactant concentrations...

Question 13

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-1at 300 °C. If the initial [NO2] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M.

Accepted Answer

A) 3.34 
B) 0.0880 
C) 2.29 
D) 0.299 
E) 17.5 
A) 3.34 
B) 0.0880 
C) 2.29 
D) 0.299 
E) 17.5

Question 14

Of the following, only ________ is a valid unit for reaction rate.

Accepted Answer

A) M/s 
B) mmol/mL 
C) mol/g 
D) g/L 
E) atm/g 
A) M/s 
B) mmol/mL 
C) mol/g 
D) g/L 
E) atm/g

Question 15

A reaction was found to be second order in carbon monoxide concentration. The rate of the reaction ________ if the [CO] is doubled, with everything else kept the same.

Accepted Answer

A) doubles 
B) remains unchanged 
C) triples 
D) increases by a factor of 4 
E) is reduced by a factor of 2 
A) doubles 
B) remains unchanged 
C) triples 
D) increases by a factor of 4 
E) is reduced by a factor of 2

Question 16

The overall order of a reaction is 1. The units of the rate constant for the reaction are ________.

Accepted Answer

A) M/s 
B) M-1s-1 
C) 1/s 
D) 1/M 
E) s/M2 
A) M/s 
B) M-1s-1 
C) 1/s 
D) 1/M 
E) s/M2

Question 17

The rate law of the overall reaction A + B → C
Is rate = k[A]2. Which of the following will not increase the rate of the reaction?

Accepted Answer

A) increasing the concentration of reactant A 
B) increasing the concentration of reactant B 
C) increasing the temperature of the reaction 
D) adding a catalyst for the reaction 
E) All of these will increase the rate. 
A) increasing the concentration of reactant A 
B) increasing the concentration of reactant B 
C) increasing the temperature of the reaction 
D) adding a catalyst for the reaction 
E) All of these will increase the rate.

Question 18

The kinetics of the reaction below were studied and it was determined that the reaction rate did not change when the concentration of B was tripled. The reaction is ________ order in B. A + B → P

Accepted Answer

A) zero 
B) first 
C) second 
D) third 
E) one-half 
A) zero 
B) first 
C) second 
D) third 
E) one-half

Question 19

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 disappearance of A between 20 s and 30 s is ________ mol/s.

Accepted Answer

A) 5.0 × 10-4 
B) 1.6 × 10-2 
C) 1.5 × 10-3 
D) 670 
E) 0.15 
A) 5.0 × 10-4 
B) 1.6 × 10-2 
C) 1.5 × 10-3 
D) 670 
E) 0.15

Question 20

The rate of disappearance of HBr in the gas phase reaction 2HBr (g) → H2 (g) + Br2 (g)
Is 0.190 M s-1 at 150 °C. The rate of appearance of Br2 is ________ M s-1.

Accepted Answer

A) 2.63 
B) 0.095 
C) 0.0361 
D) 0.380 
E) 0.436 
A) 2.63 
B) 0.095 
C) 0.0361 
D) 0.380 
E) 0.436

Exam 14: Chemical Kinetics

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

The reaction A → B is first order in [A]. Consider the following data. The rate constant for this reaction is ________ s-1.

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

For the elementary reaction NO3 + CO → NO2 + CO2 The molecularity of the reaction is ________, and the rate law is

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 20 s and 40 s is ________ mol/s.

The reaction 2NO2 → 2NO + O2 Follows second-order kinetics. At 300 °C, [NO2] drops from 0.0100 M to 0.00650 M in 100.0 s. The rate constant for the reaction is ________ M-1s-1.

The concentration of S2O82- remaining at 800 s is ________ M.

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 magnitude of the rate constant for the reaction?

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 (g) → 2NO (g) + O2 (g) In a particular experiment at 300 °C, [NO2] drops from 0.0100 to 0.00800 M in 100 s. The rate of appearance of O2 for this period is ________ M/s.

A catalyst can increase the rate of a reaction ________.

The initial concentration of reactant in a first-order reaction is 0.27 M. The rate constant for the reaction is 0.75 s-1. What is the concentration (mol/L)of reactant after 1.8 s?

Reaction rates are affected by reactant concentrations and temperature. This is accounted for by the ________.

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-1at 300 °C. If the initial [NO2] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M.

Of the following, only ________ is a valid unit for reaction rate.

A reaction was found to be second order in carbon monoxide concentration. The rate of the reaction ________ if the [CO] is doubled, with everything else kept the same.

The overall order of a reaction is 1. The units of the rate constant for the reaction are ________.

The rate law of the overall reaction A + B → C Is rate = k[A]2. Which of the following will not increase the rate of the reaction?

The kinetics of the reaction below were studied and it was determined that the reaction rate did not change when the concentration of B was tripled. The reaction is ________ order in B. A + B → P

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 disappearance of A between 20 s and 30 s is ________ mol/s.

The rate of disappearance of HBr in the gas phase reaction 2HBr (g) → H2 (g) + Br2 (g) Is 0.190 M s-1 at 150 °C. The rate of appearance of Br2 is ________ M s-1.

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

The reaction A → B is first order in [A]. Consider the following data. The rate constant for this reaction is ________ s^-1.

For the elementary reaction NO₃ + CO → NO₂ + CO₂ The molecularity of the reaction is ________, and the rate law is

The reaction 2NO₂ → 2NO + O₂ Follows second-order kinetics. At 300 °C, [NO₂] drops from 0.0100 M to 0.00650 M in 100.0 s. The rate constant for the reaction is ________ M^-1s^-1.

The concentration of S₂O₈^2- remaining at 800 s is ________ M.

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 magnitude of the rate constant for the reaction?

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂ (g) → 2NO (g) + O₂ (g) In a particular experiment at 300 °C, [NO₂] drops from 0.0100 to 0.00800 M in 100 s. The rate of appearance of O₂ for this period is ________ M/s.

The initial concentration of reactant in a first-order reaction is 0.27 M. The rate constant for the reaction is 0.75 s^-1. What is the concentration (mol/L)of reactant after 1.8 s?

The rate law of the overall reaction A + B → C Is rate = k[A]². Which of the following will not increase the rate of the reaction?

The rate of disappearance of HBr in the gas phase reaction 2HBr (g) → H₂(g) + Br₂ (g) Is 0.190 M s^-1 at 150 °C. The rate of appearance of Br₂ is ________ M s^-1.