Question 1

What are the units of a rate constant for a reaction that has an overall order of 3?

Accepted Answer

The answer of What are the units of a rate...

Question 2

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates:
2 NO2 $\rightarrow$NO3 + NO
NO3 + CO $\rightarrow$ CO2 + NO2

Accepted Answer

NO2 + CO

Question 3

Explain the mechanisms by which catalysts function.

Accepted Answer

A catalyst functions by provid

Question 4

Consider the following energy-reaction coordinate diagram.   Give the names for the quantities indicated by A, B and C.

Accepted Answer

A (catalyzed activat

Question 5

The following concentration vs. time data were collected for the reaction:
A + 2B$\rightarrow$C   Calculate   for A, B and C for the following time differences:(a) 0 and 60 s,(b) 900 and 960 s,(c) What is the rate of the reaction for part

Accepted Answer

The answer of The following concentration vs. time data were...

Question 6

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates:
Cl2$\rightarrow$ 2 Cl•
Cl• + CO $\rightarrow$ COCl
COCl + Cl2 $\rightarrow$COCl2 + Cl•
2 Cl• $\rightarrow$ Cl2

Accepted Answer

CO + Cl2

Question 7

Consider the following three molecular pictures that represent the relative numbers of the two reactants involved in one step of the depletion of stratospheric ozone by chlorine atoms:   The equation for the elementary reaction and a molecular picture of the reaction process are shown below:Cl• + O3$\rightarrow$ ClO + O2   If the three samples represented by A, B and C are at the same temperature, what are the rates of reaction of B and C compared to that of A?

Accepted Answer

In B the reaction is

Question 8

Rate data were collected for the following reaction at a constant temperature.2ClO2(aq) + 2 OH-1(aq)$\rightarrow$ClO3-1(aq) + ClO2-1(aq) + H2O(l)   a) Determine the rate law for this reaction.b) Determine the rate constant with appropriate units.

Accepted Answer

a) rate = k[ClO

Question 9

The following mechanism has been suggested for the decomposition of ozone, O3.O3(g)   O2(g) + O(g) (fast equilibrium)
O(g) + O3(g)  $\rarr$ 2 O2(g) (slow)
Consider the following statements in light of this mechanism:
I. The rate law is second order in O3.
II. The rate does not depend on the concentration of O2.
III. The reaction slows with increased O2 concentration.
IV. The rate law is second order.
V. Substances reacting with O atoms will speed up the reaction.Which of the above statements are true?

Accepted Answer

A)  II and V 
B)  II only 
C)  I and IV 
D)  I and III 
E)  II, IV and V 
A)  II and V 
B)  II only 
C)  I and IV 
D)  I and III 
E)  II, IV and V

Question 10

The synthesis of nitrogen monoxide proceeds by the reaction of ammonia with oxygen as shown in the following unbalanced reaction:
NH3(g) + O2(g)  $\rarr$  NO(g) + H2O(g)If O2 is being consumed at a rate of 32 mole/sec, what is the rate of NO production?

Accepted Answer

A)  38. mole/sec 
B)  1.9 x 103 mole/minute 
C)  15 x 103 mole/minute 
D)  32 mole/minute 
E)  1.4 x 105 mole/hour 
A)  38. mole/sec 
B)  1.9 x 103 mole/minute 
C)  15 x 103 mole/minute 
D)  32 mole/minute 
E)  1.4 x 105 mole/hour

Question 11

What is the rate law associated with the following mechanism:
HCl + HCl   H2Cl2
HCl + CH3CHCH2   CH3CHClCH3
H2Cl2 + CH3CHClCH3  $\rarr$ CH3CHClCH3 +2 HCl
Net: HCl(g) + CH3CHCH2(g)  $\rarr$ CH3CHClCH3 (g)

Accepted Answer

A)  rate = k[HCl]2[CH3CHCH2] 
B)  rate = k[HCl]3[CH3CHCH2] 
C)  rate = k[H2Cl2][CH3CHClCH3] 
D)  rate = k[HCl][CH3CHCH2] 
E)  rate = k[HCl]2 
A)  rate = k[HCl]2[CH3CHCH2] 
B)  rate = k[HCl]3[CH3CHCH2] 
C)  rate = k[H2Cl2][CH3CHClCH3] 
D)  rate = k[HCl][CH3CHCH2] 
E)  rate = k[HCl]2

Question 12

The first-order rate constant for the decomposition of trioxane (C3H6O3) is known to be 3.05 x 10-4 s-1 at 519ºK. What is the half life of trioxane at 519ºK?

Accepted Answer

A)  3.28 x 103 s 
B)  6.93 x103 s 
C)  0.693 hour 
D)  0.631 hour 
E)  0.328 hour 
A)  3.28 x 103 s 
B)  6.93 x103 s 
C)  0.693 hour 
D)  0.631 hour 
E)  0.328 hour

Question 13

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol-1. At what temperature would the rate constant for this reaction be ten times that of 500oC?

Accepted Answer

Question 14

Hydrogen peroxide decomposes according to the equation:
2 H2O2(aq) $\rightarrow$ 2 H2O(l) + O2(g)
At 27°C and 1 atm, a 50.0 ml sample of hydrogen peroxide decomposes at a rate that produces 10.0 ml/sec of O2(g). Assuming ideal behavioura) Determine the moles of oxygen produced per second.b) Determine the change in molarity of H2O2 per second.

Accepted Answer

a) 4.03 x10^-4</

Question 15

Heterogeneous catalysts are used in industrial processes because
I. they utilize more of the catalyst atoms.
II. it is easier to separate the products from the catalyst.
III. higher operating temperatures are readily obtained.
IV. they are more selective.Which of the above statements are true?

Accepted Answer

A)  I, II and III 
B)  II and III 
C)  III and IV 
D)  I and IV 
E)  II and IV 
A)  I, II and III 
B)  II and III 
C)  III and IV 
D)  I and IV 
E)  II and IV

Question 16

For a hypothetical reaction, the activation energy is Eact = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M-1s-1. Determine what the rate constant would be if the temperature was 400$\degree$C.

Accepted Answer

k = 0.0028

Question 17

In which order do the following steps typically occur for reactions facilitated by heterogeneous catalysts:
I. Desorption of material
II. Adsorption on materials on catalyst surface
III. Reaction to form products
IV. Movement of bound species over catalyst surface

Accepted Answer

A)  II, I, III, IV 
B)  II, IV, III, I 
C)  II, I, IV, III 
D)  II, III, IV, I 
E)  IV, II, III, I 
A)  II, I, III, IV 
B)  II, IV, III, I 
C)  II, I, IV, III 
D)  II, III, IV, I 
E)  IV, II, III, I

What are the units of a rate constant for a reaction that has an overall order of 3?

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO₂ $\rightarrow$ NO₃ + NO NO₃ + CO $\rightarrow$ CO₂ + NO₂

Explain the mechanisms by which catalysts function.

Consider the following energy-reaction coordinate diagram. Give the names for the quantities indicated by A, B and C.

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: Cl₂ $\rightarrow$ 2 Cl• Cl• + CO $\rightarrow$ COCl COCl + Cl₂ $\rightarrow$ COCl₂ + Cl• 2 Cl• $\rightarrow$ Cl₂

The synthesis of nitrogen monoxide proceeds by the reaction of ammonia with oxygen as shown in the following unbalanced reaction: NH₃(g) + O₂(g) $\rarr$ NO(g) + H₂O(g)If O₂ is being consumed at a rate of 32 mole/sec, what is the rate of NO production?

The first-order rate constant for the decomposition of trioxane (C₃H₆O₃) is known to be 3.05 x 10^-4 s^-1 at 519ºK. What is the half life of trioxane at 519ºK?

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol^-1. At what temperature would the rate constant for this reaction be ten times that of 500^oC?

Heterogeneous catalysts are used in industrial processes because I. they utilize more of the catalyst atoms. II. it is easier to separate the products from the catalyst. III. higher operating temperatures are readily obtained. IV. they are more selective.Which of the above statements are true?

For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400 $\degree$ C.

In which order do the following steps typically occur for reactions facilitated by heterogeneous catalysts: I. Desorption of material II. Adsorption on materials on catalyst surface III. Reaction to form products IV. Movement of bound species over catalyst surface

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

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Exam 13: Kinetics: Mechanisms and Rates of Reactions

What are the units of a rate constant for a reaction that has an overall order of 3?

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO2 →\rightarrow→ NO3 + NO NO3 + CO →\rightarrow→ CO2 + NO2

Explain the mechanisms by which catalysts function.

Consider the following energy-reaction coordinate diagram. Give the names for the quantities indicated by A, B and C.

The following concentration vs. time data were collected for the reaction: A + 2B →\rightarrow→ C Calculate for A, B and C for the following time differences:(a) 0 and 60 s,(b) 900 and 960 s,(c) What is the rate of the reaction for part

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: Cl2 →\rightarrow→ 2 Cl• Cl• + CO →\rightarrow→ COCl COCl + Cl2 →\rightarrow→ COCl2 + Cl• 2 Cl• →\rightarrow→ Cl2

Rate data were collected for the following reaction at a constant temperature.2ClO2(aq) + 2 OH-1(aq) →\rightarrow→ ClO3-1(aq) + ClO2-1(aq) + H2O(l) a) Determine the rate law for this reaction.b) Determine the rate constant with appropriate units.

The synthesis of nitrogen monoxide proceeds by the reaction of ammonia with oxygen as shown in the following unbalanced reaction: NH3(g) + O2(g) →\rarr→ NO(g) + H2O(g)If O2 is being consumed at a rate of 32 mole/sec, what is the rate of NO production?

What is the rate law associated with the following mechanism: HCl + HCl H2Cl2 HCl + CH3CHCH2 CH3CHClCH3 H2Cl2 + CH3CHClCH3 →\rarr→ CH3CHClCH3 +2 HCl Net: HCl(g) + CH3CHCH2(g) →\rarr→ CH3CHClCH3 (g)

The first-order rate constant for the decomposition of trioxane (C3H6O3) is known to be 3.05 x 10-4 s-1 at 519ºK. What is the half life of trioxane at 519ºK?

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol-1. At what temperature would the rate constant for this reaction be ten times that of 500oC?

Heterogeneous catalysts are used in industrial processes because I. they utilize more of the catalyst atoms. II. it is easier to separate the products from the catalyst. III. higher operating temperatures are readily obtained. IV. they are more selective.Which of the above statements are true?

For a hypothetical reaction, the activation energy is Eact = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M-1s-1. Determine what the rate constant would be if the temperature was 400 °\degree° C.

In which order do the following steps typically occur for reactions facilitated by heterogeneous catalysts: I. Desorption of material II. Adsorption on materials on catalyst surface III. Reaction to form products IV. Movement of bound species over catalyst surface

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: 2 NO₂ $\rightarrow$ NO₃ + NO NO₃ + CO $\rightarrow$ CO₂ + NO₂

Write the overall equation of reaction for the following mechanism and identify the reaction intermediates: Cl₂ $\rightarrow$ 2 Cl• Cl• + CO $\rightarrow$ COCl COCl + Cl₂ $\rightarrow$ COCl₂ + Cl• 2 Cl• $\rightarrow$ Cl₂

The synthesis of nitrogen monoxide proceeds by the reaction of ammonia with oxygen as shown in the following unbalanced reaction: NH₃(g) + O₂(g) $\rarr$ NO(g) + H₂O(g)If O₂ is being consumed at a rate of 32 mole/sec, what is the rate of NO production?

The first-order rate constant for the decomposition of trioxane (C₃H₆O₃) is known to be 3.05 x 10^-4 s^-1 at 519ºK. What is the half life of trioxane at 519ºK?

The activation energy for the high temperature conversion cyclopropane to propene is 270 kJ mol^-1. At what temperature would the rate constant for this reaction be ten times that of 500^oC?

For a hypothetical reaction, the activation energy is E_act = 50.2 kJ/mol and it has an Arrhenius constant of 22.3 M^-1s^-1. Determine what the rate constant would be if the temperature was 400 $\degree$ C.