Question 1

Given: 2NO2(g)+ F2(g)$\rightarrow$2NO2F(g)
Rate = -$\Delta$[F2]/$\Delta$t
The rate of the reaction can also be expressed as

Accepted Answer

A) -2$\Delta$[NO2]/$\Delta$t. 
B) $\Delta$[NO2F]/$\Delta$t. 
C) $ \begin{array}{l}\frac{1}{2}  \Delta\left[\mathrm{NO}_{2}\right] / \Delta t .\end{array} $ 
D) -$\Delta$[NO2]/$\Delta$t. 
E) $ \begin{array}{l}\frac{1}{2} \Delta\left[\mathrm{NO}_{2} \mathrm{~F}\right] / \Delta t .\end{array} $ 
A) -2$\Delta$[NO2]/$\Delta$t. 
B) $\Delta$[NO2F]/$\Delta$t. 
C) $ \begin{array}{l}\frac{1}{2}  \Delta\left[\mathrm{NO}_{2}\right] / \Delta t .\end{array} $ 
D) -$\Delta$[NO2]/$\Delta$t. 
E) $ \begin{array}{l}\frac{1}{2} \Delta\left[\mathrm{NO}_{2} \mathrm{~F}\right] / \Delta t .\end{array} $

Question 2

A possible mechanism for the reaction A + B + D $\rightarrow$ E + F is
A + B → C
k1,k-1,fast
C + D $\rightarrow$ E + F
k2
where C is a reactive intermediate present in very low concentrations.Calculate the steady state concentration of C in terms of the rate constants for the individual steps and the concentrations of the reactants.

Accepted Answer

[C] = k₁[

Question 3

Consider the reaction
2A $\rightarrow$ B,Rate = k[A]2
If the rate of appearance of B is followed,derive the experimental rate constant.

Accepted Answer

k is deter

Question 4

A reaction has k = 8.39 M-1.s-1.How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

Accepted Answer

A) 5.42 s 
B) 2.00 s 
C) 1.42 s 
D) 8.39 s 
E) 4.00 s 
A) 5.42 s 
B) 2.00 s 
C) 1.42 s 
D) 8.39 s 
E) 4.00 s

Question 5

Given: A + B $\rightarrow$ P rate = k[A][B] Which of the following is true?

Accepted Answer

A) k = ln 2/t1/2 
B) ln [A]t = +kt + ln [A]o 
C) [A]t = [A]o/(1 + kt[A]o) 
D) 1/[A]t = 1/kt 
A) k = ln 2/t1/2 
B) ln [A]t = +kt + ln [A]o 
C) [A]t = [A]o/(1 + kt[A]o) 
D) 1/[A]t = 1/kt

Question 6

The reaction profile for the reaction
[(CN)5CoOH2]2-(aq)+ SCN-(aq)$\rightarrow$[(CN)5CoSCN]3- + H2O(l)
is  
 Identify the structure of B.What do A and C represent?

Accepted Answer

B = [(CN)₅

Question 7

For the reaction A $\rightarrow$  products,the following data were collected.  
 Determine the order of the reaction and calculate the rate constant.

Accepted Answer

second-ord

Question 8

Consider the reaction 2N2O(g)$\rightarrow$ 2N2(g)+ O2(g)
Rate = k[N2O]
For an initial concentration of N2O of 0.50 M,what is the concentration of N2O remaining after 2.0 min if k = 3.4 * 10-3 s-1?

Accepted Answer

A) 0.50 M 
B) 0.55 M 
C) 0.66 M 
D) 0.33 M 
E) 0.17 M 
A) 0.50 M 
B) 0.55 M 
C) 0.66 M 
D) 0.33 M 
E) 0.17 M

Question 9

For the reaction cyclobutane(g)$\rightarrow$  2ethylene(g)at 800 K,the half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

Accepted Answer

A) 2.2 s 
B) 2.6 s 
C) 16 ms 
D) 0.38 s 
E) 0.43 s 
A) 2.2 s 
B) 2.6 s 
C) 16 ms 
D) 0.38 s 
E) 0.43 s

Question 10

Consider the reaction
2A $\rightarrow$B,Rate = k[A]2
If the rate of disappearance of A is followed,derive the experimental rate constant.

Accepted Answer

2k; the numerical va

Question 11

A catalyst facilitates a reaction by

Accepted Answer

A) increasing the activation energy for the reverse reaction. 
B) lowering the activation energy of the reaction. 
C) shifting the position of the equilibrium of the reaction. 
D) decreasing the temperature at which the reaction will proceed spontaneously. 
E) making the reaction more exothermic. 
A) increasing the activation energy for the reverse reaction. 
B) lowering the activation energy of the reaction. 
C) shifting the position of the equilibrium of the reaction. 
D) decreasing the temperature at which the reaction will proceed spontaneously. 
E) making the reaction more exothermic.

Question 12

Consider the following mechanism for the destruction of ozone.
O3 + NO $\rightarrow$ NO2 + O2
NO2 + O $\rightarrow$ NO + O2
What is the catalyst in this reaction?

Accepted Answer

The answer of Consider the following mechanism for the destruction...

Question 13

For a second-order reaction,a straight line is obtained from a plot of

Accepted Answer

A) 1/[A] vs t. 
B) ln(1/t)vs [A]. 
C) [A] vs t. 
D) ln[A] vs t. 
E) ln(t)vs [A]. 
A) 1/[A] vs t. 
B) ln(1/t)vs [A]. 
C) [A] vs t. 
D) ln[A] vs t. 
E) ln(t)vs [A].

Question 14

For a given first-order reaction,after 230 s,33% of the reactants remain.Calculate the rate constant for the reaction.

Accepted Answer

A) 207 s-1  
B) 0.00174 s-1  
C) 0.00209 s-1  
D) 0.000756 s-1  
E) 0.00482 s-1  
A) 207 s-1  
B) 0.00174 s-1  
C) 0.00209 s-1  
D) 0.000756 s-1  
E) 0.00482 s-1

Question 15

Consider the following mechanism for the production of phosgene.
Cl2 $\rightarrow$ Cl + Cl
Cl + CO $\rightarrow$ COCl
COCl + Cl $\rightarrow$ COCl2
The molecularity of the first and second elementary reactions is ____ and ____.

Accepted Answer

The answer of Consider the following mechanism for the production...

Question 16

A first-order reaction has a rate constant of 0.00300 s-1.The time required for 60% reaction is

Accepted Answer

A) 153 s. 
B) 73.9 s. 
C) 170 s. 
D) 133 s. 
E) 305 s. 
A) 153 s. 
B) 73.9 s. 
C) 170 s. 
D) 133 s. 
E) 305 s.

Question 17

For the reaction 
HO(g)+ H2(g)$\rightarrow$ H2O(g)+ H(g)
A plot of   versus 1/T gives a straight line with a slope equal to -5.1 * 103 K.What is the activation energy for the reaction?

Accepted Answer

A) 42 kJ.mol-1  
B) 98 kJ.mol-1  
C) 0.61 kJ.mol-1  
D) 5.1 kJ.mol-1  
E) 12 kJ.mol-1  
A) 42 kJ.mol-1  
B) 98 kJ.mol-1  
C) 0.61 kJ.mol-1  
D) 5.1 kJ.mol-1  
E) 12 kJ.mol-1

Question 18

The concentration-time dependence for two first order reactions is:   
Which reaction has the greater t½?

Accepted Answer

the reacti

Question 19

Given: 
2A(g)+ B(g)+ C(g)$\rightarrow$ AC(g)+ BD(g)
The following data were collected for this reaction.

What is the rate law for this reaction?

Accepted Answer

A) rate = k[A]2[B][C] 
B) rate = k[B]2[C] 
C) rate = k[A][C]2 
D) rate = k[A][B][C] 
E) rate = k[A]2[C] 
A) rate = k[A]2[B][C] 
B) rate = k[B]2[C] 
C) rate = k[A][C]2 
D) rate = k[A][B][C] 
E) rate = k[A]2[C]

Question 20

Consider the mechanism
ClO-(aq)+ H2O(l) → HOCl(aq)+ OH-(aq)K,fast
I-(aq)+ HOCl(aq)$\rightarrow$ HOI(aq)+ Cl-(aq)k,slow
HOI(aq)+ OH-(aq)$\rightarrow$OI-(aq)+ H2O(l)k,fast
Draw the reaction profile for this mechanism.

Accepted Answer

There will be 3 peak

Given: 2NO₂(g)+ F₂(g) $\rightarrow$ 2NO₂F(g) Rate = - $\Delta$ [F₂]/ $\Delta$ t The rate of the reaction can also be expressed as

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of appearance of B is followed,derive the experimental rate constant.

A reaction has k = 8.39 M^-1.s^-1.How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

Given: A + B $\rightarrow$ P rate = k[A][B] Which of the following is true?

For the reaction A $\rightarrow$ products,the following data were collected. $For the reaction A \rightarrow products,the following data were collected. Determine the order of the reaction and calculate the rate constant.$ Determine the order of the reaction and calculate the rate constant.

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O] For an initial concentration of N₂O of 0.50 M,what is the concentration of N₂O remaining after 2.0 min if k = 3.4 * 10^-3 s^-1?

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)at 800 K,the half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of disappearance of A is followed,derive the experimental rate constant.

A catalyst facilitates a reaction by

Consider the following mechanism for the destruction of ozone. O₃ + NO $\rightarrow$ NO₂ + O₂ NO₂ + O $\rightarrow$ NO + O₂ What is the catalyst in this reaction?

For a second-order reaction,a straight line is obtained from a plot of

For a given first-order reaction,after 230 s,33% of the reactants remain.Calculate the rate constant for the reaction.

Consider the following mechanism for the production of phosgene. Cl₂ $\rightarrow$ Cl + Cl Cl + CO $\rightarrow$ COCl COCl + Cl $\rightarrow$ COCl₂ The molecularity of the first and second elementary reactions is and .

A first-order reaction has a rate constant of 0.00300 s^-1.The time required for 60% reaction is

The concentration-time dependence for two first order reactions is: Which reaction has the greater t_½?

Given: 2A(g)+ B(g)+ C(g) $\rightarrow$ AC(g)+ BD(g) The following data were collected for this reaction. $Given: 2A(g)+ B(g)+ C(g) \rightarrow AC(g)+ BD(g) The following data were collected for this reaction. What is the rate law for this reaction?$ What is the rate law for this reaction?

Consider the mechanism ClO^-(aq)+ H₂O(l) → HOCl(aq)+ OH^-(aq)K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq)k,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l)k,fast Draw the reaction profile for this mechanism.

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Exam 15: Chemical Kinetics

Given: 2NO2(g)+ F2(g) →\rightarrow→ 2NO2F(g) Rate = - Δ\DeltaΔ [F2]/ Δ\DeltaΔ t The rate of the reaction can also be expressed as

Consider the reaction 2A →\rightarrow→ B,Rate = k[A]2 If the rate of appearance of B is followed,derive the experimental rate constant.

A reaction has k = 8.39 M-1.s-1.How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

Given: A + B →\rightarrow→ P rate = k[A][B] Which of the following is true?

The reaction profile for the reaction [(CN)5CoOH2]2-(aq)+ SCN-(aq) →\rightarrow→ [(CN)5CoSCN]3- + H2O(l) is Identify the structure of B.What do A and C represent?

For the reaction A →\rightarrow→ products,the following data were collected. Determine the order of the reaction and calculate the rate constant.

Consider the reaction 2N2O(g) →\rightarrow→ 2N2(g)+ O2(g) Rate = k[N2O] For an initial concentration of N2O of 0.50 M,what is the concentration of N2O remaining after 2.0 min if k = 3.4 * 10-3 s-1?

For the reaction cyclobutane(g) →\rightarrow→ 2ethylene(g)at 800 K,the half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

Consider the reaction 2A →\rightarrow→ B,Rate = k[A]2 If the rate of disappearance of A is followed,derive the experimental rate constant.

A catalyst facilitates a reaction by

Consider the following mechanism for the destruction of ozone. O3 + NO →\rightarrow→ NO2 + O2 NO2 + O →\rightarrow→ NO + O2 What is the catalyst in this reaction?

For a second-order reaction,a straight line is obtained from a plot of

For a given first-order reaction,after 230 s,33% of the reactants remain.Calculate the rate constant for the reaction.

Consider the following mechanism for the production of phosgene. Cl2 →\rightarrow→ Cl + Cl Cl + CO →\rightarrow→ COCl COCl + Cl →\rightarrow→ COCl2 The molecularity of the first and second elementary reactions is ____ and ____.

A first-order reaction has a rate constant of 0.00300 s-1.The time required for 60% reaction is

For the reaction HO(g)+ H2(g) →\rightarrow→ H2O(g)+ H(g) A plot of versus 1/T gives a straight line with a slope equal to -5.1 * 103 K.What is the activation energy for the reaction?

The concentration-time dependence for two first order reactions is: Which reaction has the greater t½?

Given: 2A(g)+ B(g)+ C(g) →\rightarrow→ AC(g)+ BD(g) The following data were collected for this reaction. What is the rate law for this reaction?

Consider the mechanism ClO-(aq)+ H2O(l) → HOCl(aq)+ OH-(aq)K,fast I-(aq)+ HOCl(aq) →\rightarrow→ HOI(aq)+ Cl-(aq)k,slow HOI(aq)+ OH-(aq) →\rightarrow→ OI-(aq)+ H2O(l)k,fast Draw the reaction profile for this mechanism.

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Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Chemical Equilibria

Acids and Bases

Aqueous Equilibria

Electrochemistry

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

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Given: 2NO₂(g)+ F₂(g) $\rightarrow$ 2NO₂F(g) Rate = - $\Delta$ [F₂]/ $\Delta$ t The rate of the reaction can also be expressed as

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of appearance of B is followed,derive the experimental rate constant.

A reaction has k = 8.39 M^-1.s^-1.How long does it take for the reactant concentration to drop from 0.0840 M to 0.0220 M?

Given: A + B $\rightarrow$ P rate = k[A][B] Which of the following is true?

For the reaction A $\rightarrow$ products,the following data were collected. $For the reaction A \rightarrow products,the following data were collected. Determine the order of the reaction and calculate the rate constant.$ Determine the order of the reaction and calculate the rate constant.

Consider the reaction 2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g) Rate = k[N₂O] For an initial concentration of N₂O of 0.50 M,what is the concentration of N₂O remaining after 2.0 min if k = 3.4 * 10^-3 s^-1?

For the reaction cyclobutane(g) $\rightarrow$ 2ethylene(g)at 800 K,the half-life is 0.43 s.Calculate the time needed for the concentration of cyclobutane to fall to 1/64 of its initial value.

Consider the reaction 2A $\rightarrow$ B,Rate = k[A]² If the rate of disappearance of A is followed,derive the experimental rate constant.

Consider the following mechanism for the destruction of ozone. O₃ + NO $\rightarrow$ NO₂ + O₂ NO₂ + O $\rightarrow$ NO + O₂ What is the catalyst in this reaction?

Consider the following mechanism for the production of phosgene. Cl₂ $\rightarrow$ Cl + Cl Cl + CO $\rightarrow$ COCl COCl + Cl $\rightarrow$ COCl₂ The molecularity of the first and second elementary reactions is and .

A first-order reaction has a rate constant of 0.00300 s^-1.The time required for 60% reaction is

The concentration-time dependence for two first order reactions is: Which reaction has the greater t_½?

Given: 2A(g)+ B(g)+ C(g) $\rightarrow$ AC(g)+ BD(g) The following data were collected for this reaction. $Given: 2A(g)+ B(g)+ C(g) \rightarrow AC(g)+ BD(g) The following data were collected for this reaction. What is the rate law for this reaction?$ What is the rate law for this reaction?

Consider the mechanism ClO^-(aq)+ H₂O(l) → HOCl(aq)+ OH^-(aq)K,fast I^-(aq)+ HOCl(aq) $\rightarrow$ HOI(aq)+ Cl^-(aq)k,slow HOI(aq)+ OH^-(aq) $\rightarrow$ OI^-(aq)+ H₂O(l)k,fast Draw the reaction profile for this mechanism.