A possible mechanism for the decomposition of ozone to oxygen in the atmosphere is $\begin{array}{l} \mathrm{O}_{3}(\mathrm{~g}) \rightleftharpoons \mathrm{O}_{2}(\mathrm{~g})+\mathrm{O}& \text { (fast equilibrium) } \\ \mathrm{O}+\mathrm{O}_{3}(\mathrm{~g}) \rightarrow 2 \mathrm{O}_{2}(\mathrm{~g})& \text { (slow) } \end{array}$ What is a rate law that is consistent with this mechanism?

A) rate = k[O3] B) rate = k[O3]2 C) rate = k[O3] × [O] D) rate = k[O3]2 × [O2] E) rate = k[O3]2 × [O2]?1 A) rate = k[O3] B) rate = k[O3]2 C) rate = k[O3] × [O] D) rate = k[O3]2 × [O2] E) rate = k[O3]2 × [O2]?1

For the reaction below,if the rate of appearance of Br2 is 0.180 mol/L⋅s,what is the rate of disappearance of NOBr? 2NOBr(g)→ 2NO(g)+ Br2(g)

A) -0.360 mol/L⋅s B) -0.090 mol/L⋅s C) 0.090 mol/L⋅s D) 0.180 mol/L⋅s E) 0.360 mol/L⋅s A) -0.360 mol/L⋅s B) -0.090 mol/L⋅s C) 0.090 mol/L⋅s D) 0.180 mol/L⋅s E) 0.360 mol/L⋅s

A possible reaction mechanism for the reaction of nitrogen dioxide with carbon monoxide is $\begin{array}{l} 2 \mathrm{NO}_{2}(g) \rightarrow \mathrm{NO}_{3}(g)+\mathrm{NO}(g)&(slow) \\ \mathrm{NO}_{3}(g)+\mathrm{CO}(g) \rightarrow \mathrm{NO}_{2}(g)+\mathrm{CO}_{2}(g) &(fast) \end{array} $ What is the overall reaction and the most probable rate law for the reaction?

A) NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO2] B) NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO2]2 C) NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO3]×[CO] D) 2NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO2]×[ NO3]×[CO] E) 2NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO3]×[CO] A) NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO2] B) NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO2]2 C) NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO3]×[CO] D) 2NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO2]×[ NO3]×[CO] E) 2NO2(g)+ CO(g)? NO(g)+ CO2(g);rate = k[NO3]×[CO]

The reaction of NO and O2 produces NO2. 2 NO(g)+ O2(g)→ 2 NO2(g) The reaction is second-order with respect to NO(g)and first-order with respect to O2(g).At a given temperature,the rate constant,k,equals 4.7 × 102 M-2s-1.What is the rate of reaction when the initial concentrations of NO and O2 are 0.025 M and 0.015 M,respectively?

A) 2.6 × 10-3 M/s B) 4.4 × 10-3 M/s C) 0.18 M/s D) 2.0 × 10-8 M/s E) 3.8 × 102 M/s A) 2.6 × 10-3 M/s B) 4.4 × 10-3 M/s C) 0.18 M/s D) 2.0 × 10-8 M/s E) 3.8 × 102 M/s

For the second-order reaction below,the initial concentration of A is 1.34 M.If k = 7.61 × 10?4 M1s?1,what is the concentration of A after 18.3 minutes? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

A) 0.504 M B) 0.581 M C) 0.632 M D) 0.836 M E) 1.12 M A) 0.504 M B) 0.581 M C) 0.632 M D) 0.836 M E) 1.12 M

Exam 11: Rate of Reaction

A possible mechanism for the decomposition of ozone to oxygen in the atmosphere is ()\rightleftharpoons()+ (fast equilibrium) +()\rightarrow2() (slow) What is a rate law that is consistent with this mechanism?

(Multiple Choice)

4.8/5

(37)

Question 21

Ozone in the upper atmosphere is important to life on earth because it converts harmful UV radiation to heat.How does the release of CFCs into the atmosphere affect the concentration of ozone in the upper atmosphere?

(Multiple Choice)

4.9/5

(33)

Question 22

For the reaction below,if the rate of appearance of Br₂ is 0.180 mol/L⋅s,what is the rate of disappearance of NOBr? 2NOBr(g)→ 2NO(g)+ Br₂(g)

(Multiple Choice)

4.9/5

(38)

Question 23

For the first-order reaction below,the initial concentration of A is 0.80 M.What is the half-life of the reaction if the concentration of A decreases to 0.10 M in 54 seconds? $\mathrm{A} \rightarrow \mathrm{B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ rate $=k[\mathrm{~A}]$

(Multiple Choice)

4.9/5

(36)

Question 24

For a certain reaction,the activation energy is 52.1 kJ/mole.By what ratio will the rate constant change if the temperature is decreased from 175°C to 75°C?

(Multiple Choice)

4.9/5

(27)

Question 25

A possible reaction mechanism for the reaction of nitrogen dioxide with carbon monoxide is 2(g)\rightarrow(g)+(g) (slow) (g)+(g)\rightarrow(g)+(g) (fast) What is the overall reaction and the most probable rate law for the reaction?

(Multiple Choice)

4.9/5

(35)

Question 26

Which of the following expressions corresponds to the integrated rate equation for a first-order decomposition reaction?

(Multiple Choice)

4.9/5

(36)

Question 27

Determine the overall reaction order for the chemical expression and rate expression below. 2NO(g)+ Cl₂(g)→ 2NOCl(g) Rate = k[NO]² × [Cl₂]

(Multiple Choice)

4.8/5

(36)

Question 28

For the second-order decomposition reaction, $2 \mathrm{~A} \rightarrow \mathrm{B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\text { rate }=k[\mathrm{~A}]^{2}$ Which of the following relationships yields a straight line plot?

(Multiple Choice)

4.9/5

(34)

Question 29

The effect of a catalyst on a chemical reaction is to

(Multiple Choice)

4.8/5

(41)

Question 30

The rate of reaction for the formation of carbon monoxide is measured at 1.24 mol/L⋅hr.What is the rate of formation of carbon monoxide in units of mol/L⋅s? CH₃CHO(g)→ CH₄(g)+ CO(g)

(Multiple Choice)

4.8/5

(33)

Question 31

What are the units of the rate constant for the rate expression for the following chemical equation? 2NO(g)+ Cl₂(g)→ 2NOCl(g) Rate = k[NO]² × [Cl₂]

(Multiple Choice)

4.9/5

(41)

Question 32

For the first-order reaction below,the concentration of product B after 24.2 seconds is 0.322 M. If k = 8.75 × 10−² s−¹,what was the initial concentration of A? A → 2B Rate = k[A]

(Multiple Choice)

4.9/5

(45)

Question 33

For the overall reaction 2A + B ? C Which of the following mechanisms are consistent with a rate equation of rate = k[A]²×[B]?

(Multiple Choice)

4.8/5

(36)

Question 34

A first-order reaction has a half-life of 2.10 hours.How much time is required for the reactant to be reduced to 33.0% of its initial concentration?

(Multiple Choice)

5.0/5

(38)

Question 35

The elementary steps for a catalyzed reaction are shown below.Identify the catalyst.Identify the reactive intermediate. H₂O₂(aq)+ I−(aq)→ H₂O(l)+ IO−(aq) IO−(aq)+ H₂O₂(aq)→ H₂O(l)+ O₂(g)+ I−(aq)

(Multiple Choice)

4.9/5

(37)

Question 36

Which equation is used to calculate the half-life of the first-order equation below? $\mathrm{A} \rightarrow 2 \mathrm{~B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\text { rate }=k[\mathrm{~A}]$

(Multiple Choice)

5.0/5

(29)

Question 37

The reaction of NO and O₂ produces NO₂. 2 NO(g)+ O₂(g)→ 2 NO₂(g) The reaction is second-order with respect to NO(g)and first-order with respect to O₂(g).At a given temperature,the rate constant,k,equals 4.7 × 10² M^-2s^-1.What is the rate of reaction when the initial concentrations of NO and O₂ are 0.025 M and 0.015 M,respectively?

(Multiple Choice)

4.9/5

(38)

Question 38

For the second-order reaction below,the initial concentration of A is 1.34 M.If k = 7.61 × 10?⁴ M¹s?¹,what is the concentration of A after 18.3 minutes? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$

(Multiple Choice)

4.8/5

(32)

Question 39

For a given reaction,the rate constant doubles when the temperature is increased from 45.0°C to 73.0°C.What is the activation energy for this reaction? (R = 8.31 J/K⋅mol)

(Multiple Choice)

4.8/5

(32)

Question 40

Showing 21 - 40 of 44

Exam 11: Rate of Reaction

A possible mechanism for the decomposition of ozone to oxygen in the atmosphere is ()\rightleftharpoons()+ (fast equilibrium) +()\rightarrow2() (slow) What is a rate law that is consistent with this mechanism?

Ozone in the upper atmosphere is important to life on earth because it converts harmful UV radiation to heat.How does the release of CFCs into the atmosphere affect the concentration of ozone in the upper atmosphere?

For the reaction below,if the rate of appearance of Br2 is 0.180 mol/L⋅s,what is the rate of disappearance of NOBr? 2NOBr(g)→ 2NO(g)+ Br2(g)

For the first-order reaction below,the initial concentration of A is 0.80 M.What is the half-life of the reaction if the concentration of A decreases to 0.10 M in 54 seconds? A→B \mathrm{A} \rightarrow \mathrm{B} A→B \quad \quad \quad \quad \quad rate =k[ A] =k[\mathrm{~A}] =k[ A]

For a certain reaction,the activation energy is 52.1 kJ/mole.By what ratio will the rate constant change if the temperature is decreased from 175°C to 75°C?

A possible reaction mechanism for the reaction of nitrogen dioxide with carbon monoxide is 2(g)\rightarrow(g)+(g) (slow) (g)+(g)\rightarrow(g)+(g) (fast) What is the overall reaction and the most probable rate law for the reaction?

Which of the following expressions corresponds to the integrated rate equation for a first-order decomposition reaction?

Determine the overall reaction order for the chemical expression and rate expression below. 2NO(g)+ Cl2(g)→ 2NOCl(g) Rate = k[NO]2 × [Cl2]

For the second-order decomposition reaction, 2 A→B 2 \mathrm{~A} \rightarrow \mathrm{B} 2 A→B \quad \quad \quad \quad \quad \quad rate =k[ A]2\text { rate }=k[\mathrm{~A}]^{2} rate =k[ A]2 Which of the following relationships yields a straight line plot?

The effect of a catalyst on a chemical reaction is to

The rate of reaction for the formation of carbon monoxide is measured at 1.24 mol/L⋅hr.What is the rate of formation of carbon monoxide in units of mol/L⋅s? CH3CHO(g)→ CH4(g)+ CO(g)

What are the units of the rate constant for the rate expression for the following chemical equation? 2NO(g)+ Cl2(g)→ 2NOCl(g) Rate = k[NO]2 × [Cl2]

For the first-order reaction below,the concentration of product B after 24.2 seconds is 0.322 M. If k = 8.75 × 10−2 s−1,what was the initial concentration of A? A → 2B Rate = k[A]

For the overall reaction 2A + B ? C Which of the following mechanisms are consistent with a rate equation of rate = k[A]2×[B]?

A first-order reaction has a half-life of 2.10 hours.How much time is required for the reactant to be reduced to 33.0% of its initial concentration?

The elementary steps for a catalyzed reaction are shown below.Identify the catalyst.Identify the reactive intermediate. H2O2(aq)+ I−(aq)→ H2O(l)+ IO−(aq) IO−(aq)+ H2O2(aq)→ H2O(l)+ O2(g)+ I−(aq)

Which equation is used to calculate the half-life of the first-order equation below? A→2 B \mathrm{A} \rightarrow 2 \mathrm{~B} A→2 B \quad \quad \quad \quad \quad \quad \quad \quad rate =k[ A]\text { rate }=k[\mathrm{~A}] rate =k[ A]

For the second-order reaction below,the initial concentration of A is 1.34 M.If k = 7.61 × 10?4 M1s?1,what is the concentration of A after 18.3 minutes? 2 A→B rate =k[ A]22 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}2 A→B rate =k[ A]2

For a given reaction,the rate constant doubles when the temperature is increased from 45.0°C to 73.0°C.What is the activation energy for this reaction? (R = 8.31 J/K⋅mol)

Matter and Measurements

Atoms, molecules, and Ions

Mass Relations in Chemistry;stoichiometry

Reactions in Aqueous Solution

Gases

Electronic Structure and the Periodic Table

Covalent Bonding

Thermochemistry

Liquids and Solids

Solutions

Gaseous Chemical Equilibrium

Acids and Bases

Equilibria in Acid-Base Solutions

Complex Ion and Precipitation Equilibria

Spontaneity of Reaction

Electrochemistry

Nuclear Reactions

Complex Ions

Chemistry of the Metals

Chemistry of the Nonmetals

Organic Chemistry

Organic Polymers, natural and Synthetic

Filters

For the reaction below,if the rate of appearance of Br₂ is 0.180 mol/L⋅s,what is the rate of disappearance of NOBr? 2NOBr(g)→ 2NO(g)+ Br₂(g)

For the first-order reaction below,the initial concentration of A is 0.80 M.What is the half-life of the reaction if the concentration of A decreases to 0.10 M in 54 seconds? $\mathrm{A} \rightarrow \mathrm{B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ rate $=k[\mathrm{~A}]$

Determine the overall reaction order for the chemical expression and rate expression below. 2NO(g)+ Cl₂(g)→ 2NOCl(g) Rate = k[NO]² × [Cl₂]

For the second-order decomposition reaction, $2 \mathrm{~A} \rightarrow \mathrm{B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\text { rate }=k[\mathrm{~A}]^{2}$ Which of the following relationships yields a straight line plot?

The rate of reaction for the formation of carbon monoxide is measured at 1.24 mol/L⋅hr.What is the rate of formation of carbon monoxide in units of mol/L⋅s? CH₃CHO(g)→ CH₄(g)+ CO(g)

What are the units of the rate constant for the rate expression for the following chemical equation? 2NO(g)+ Cl₂(g)→ 2NOCl(g) Rate = k[NO]² × [Cl₂]

For the first-order reaction below,the concentration of product B after 24.2 seconds is 0.322 M. If k = 8.75 × 10−² s−¹,what was the initial concentration of A? A → 2B Rate = k[A]

For the overall reaction 2A + B ? C Which of the following mechanisms are consistent with a rate equation of rate = k[A]²×[B]?

The elementary steps for a catalyzed reaction are shown below.Identify the catalyst.Identify the reactive intermediate. H₂O₂(aq)+ I−(aq)→ H₂O(l)+ IO−(aq) IO−(aq)+ H₂O₂(aq)→ H₂O(l)+ O₂(g)+ I−(aq)

Which equation is used to calculate the half-life of the first-order equation below? $\mathrm{A} \rightarrow 2 \mathrm{~B}$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\text { rate }=k[\mathrm{~A}]$

For the second-order reaction below,the initial concentration of A is 1.34 M.If k = 7.61 × 10?⁴ M¹s?¹,what is the concentration of A after 18.3 minutes? $2 \mathrm{~A} \rightarrow \mathrm{B} \quad\quad\quad\quad\quad \text { rate }=k[\mathrm{~A}]^{2}$