Question 1

2A →A2 K,fast B2 + A2 $\rightarrow$  2AB k,slow

Accepted Answer

A) 2 
B) 3 
C) 4 
D) 1 
E) 2 and 3 
A) 2 
B) 3 
C) 4 
D) 1 
E) 2 and 3

Question 2

If the average rate of formation of H2(g)is 3.90 (mol H2).L-1.s-1 for the reaction 2PH3(g)$\rightarrow$ 2P(g)+ 3H2(g),the unique average reaction rate is

Accepted Answer

A) 3.90 mol.L-1.s-1. 
B) 1.30 mol.L-1.s-1. 
C) 2.60 mol.L-1.s-1. 
D) 7.80 mol.L-1.s-1. 
E) 11.7 mol.L-1.s-1. 
A) 3.90 mol.L-1.s-1. 
B) 1.30 mol.L-1.s-1. 
C) 2.60 mol.L-1.s-1. 
D) 7.80 mol.L-1.s-1. 
E) 11.7 mol.L-1.s-1.

Question 3

For the reaction 2A + B $\rightarrow$products
Determine the rate law for the reaction given the following data:

Accepted Answer

A) rate = k[B]2  
B) rate = k[A][B]0  
C) rate = k[A]2  
D) rate = k[A][B] 
E) rate = k[A] 
A) rate = k[B]2  
B) rate = k[A][B]0  
C) rate = k[A]2  
D) rate = k[A][B] 
E) rate = k[A]

Question 4

The concentration-time curves for two sets of reactions,A/B and C/D,are:   
Which of the reactions are first order?

Accepted Answer

A) B and D 
B) A and B 
C) C and D 
D) A and C 
A) B and D 
B) A and B 
C) C and D 
D) A and C

Question 5

The reaction 
2ClO2(g)+ F2(g)$\rightarrow$   2FClO2(g)
Is first order in both ClO2 and F2.When the initial concentrations of ClO2 and F2 are equal,the rate after 25% of the F2 has reacted is what percent of the initial rate?

Accepted Answer

A) 75.0% 
B) 18.8% 
C) 37.5% 
D) 28.1% 
E) 12.5% 
A) 75.0% 
B) 18.8% 
C) 37.5% 
D) 28.1% 
E) 12.5%

Question 6

Given: 
CH4(g)+ Cl2(g)$\rightarrow$  CH3Cl(g)+ HCl(g)
The rate law for this elementary process is

Accepted Answer

A) rate = k[Cl2]. 
B) k[CH3Cl][HCl]. 
C) rate = k[CH4][Cl2]. 
D) rate = k[CH4]. 
E) rate = k[CH4]2.  
A) rate = k[Cl2]. 
B) k[CH3Cl][HCl]. 
C) rate = k[CH4][Cl2]. 
D) rate = k[CH4]. 
E) rate = k[CH4]2.

Question 7

Given: A $\rightarrow$   P rate = k[A] If 20% of A reacts in 5.12 min,calculate the time required for 90% of A to react.

Accepted Answer

A) 52.8 min 
B) 1.05 min 
C) 2.42 min 
D) 3170 min 
E) 22.9 min 
A) 52.8 min 
B) 1.05 min 
C) 2.42 min 
D) 3170 min 
E) 22.9 min

Question 8

For the proposed mechanism A + X → B k1,k-1 (fast)
B $\rightarrow$ products k2 (slow)
What is the rate law?

Accepted Answer

A) rate = (k1k-1)[A][X] 
B) rate = k2[B] 
C) rate = (k1/k2)[A] 
D) rate = (k1k2/ k-1)[A] 
E) rate = (k1k2/ k-1)[A][X] 
A) rate = (k1k-1)[A][X] 
B) rate = k2[B] 
C) rate = (k1/k2)[A] 
D) rate = (k1k2/ k-1)[A] 
E) rate = (k1k2/ k-1)[A][X]

Question 9

Consider the mechanism 
NO2(g)+ F2(g)$\rightarrow$ NO2F(g)+ F(g)k1 (slow)
F(g)+ NO2(g)$\rightarrow$ NO2F(g)k2 (fast)
Give the molecularity of the first step and any intermediates in the mechanism.

Accepted Answer

A) 2,and F(g) 
B) 2,and NO2F(g) 
C) 2,and NO2(g) 
D) 1,and no intermediate 
E) 2,and no intermediate 
A) 2,and F(g) 
B) 2,and NO2F(g) 
C) 2,and NO2(g) 
D) 1,and no intermediate 
E) 2,and no intermediate

Question 10

Given: 2O3(g)$\rightarrow$3O2(g)
Rate = k[O3]2[O2]-1
The overall order of the reaction and the order with respect to [O3] are

Accepted Answer

A) -1 and 3. 
B) 1 and 2. 
C) 0 and 1. 
D) 2 and 2. 
E) 3 and 2. 
A) -1 and 3. 
B) 1 and 2. 
C) 0 and 1. 
D) 2 and 2. 
E) 3 and 2.

Question 11

The rate law for the following mechanism is NO2(g)+ F2(g)$\rightarrow$ NO2F(g)+ F(g)
K1,slow
F(g)+ NO2(g)$\rightarrow$ NO2F(g)
K2,fast

Accepted Answer

A) rate = k2[NO2]2.  
B) rate = k2[NO2][F]. 
C) rate = k1[NO2][F2]. 
D) rate = k1k2[NO2]2.  
E) rate = k1[NO2F][F]. 
A) rate = k2[NO2]2.  
B) rate = k2[NO2][F]. 
C) rate = k1[NO2][F2]. 
D) rate = k1k2[NO2]2.  
E) rate = k1[NO2F][F].

Question 12

The concentration-time dependence for a first-order reaction is:  
 At which point on the curve is the reaction fastest?

Accepted Answer

A) A 
B) B 
C) C 
D) A + t½ 
E) The rates are the same at all points. 
A) A 
B) B 
C) C 
D) A + t½ 
E) The rates are the same at all points.

Question 13

If the rate of reaction increases by a factor of 2.3 when the concentration of reactant increases by a factor of 1.5,the order of the reaction with respect to this reactant is

Accepted Answer

A) 2. 
B) 1. 
C) 1.5. 
D) 4. 
E) 3. 
A) 2. 
B) 1. 
C) 1.5. 
D) 4. 
E) 3.

2A →A₂ K,fast B₂ + A₂ $\rightarrow$ 2AB k,slow

If the average rate of formation of H₂(g)is 3.90 (mol H₂).L^-1.s^-1 for the reaction 2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g),the unique average reaction rate is

For the reaction 2A + B $\rightarrow$ products Determine the rate law for the reaction given the following data: $For the reaction 2A + B \rightarrow products Determine the rate law for the reaction given the following data:$

The concentration-time curves for two sets of reactions,A/B and C/D,are: Which of the reactions are first order?

The reaction 2ClO₂(g)+ F₂(g) $\rightarrow$ 2FClO₂(g) Is first order in both ClO₂ and F₂.When the initial concentrations of ClO₂ and F₂ are equal,the rate after 25% of the F₂ has reacted is what percent of the initial rate?

Given: CH₄(g)+ Cl₂(g) $\rightarrow$ CH₃Cl(g)+ HCl(g) The rate law for this elementary process is

Given: A $\rightarrow$ P rate = k[A] If 20% of A reacts in 5.12 min,calculate the time required for 90% of A to react.

For the proposed mechanism A + X → B k₁,k_-1(fast) B $\rightarrow$ products k₂ (slow) What is the rate law?

Consider the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g)k₁ (slow) F(g)+ NO₂(g) $\rightarrow$ NO₂F(g)k₂ (fast) Give the molecularity of the first step and any intermediates in the mechanism.

Given: 2O₃(g) $\rightarrow$ 3O₂(g) Rate = k[O₃]²[O₂]^-1 The overall order of the reaction and the order with respect to [O₃] are

The rate law for the following mechanism is NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁,slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂,fast

The concentration-time dependence for a first-order reaction is: At which point on the curve is the reaction fastest?

If the rate of reaction increases by a factor of 2.3 when the concentration of reactant increases by a factor of 1.5,the order of the reaction with respect to this reactant is

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Exam 15: Chemical Kinetics

2A →A2 K,fast B2 + A2 →\rightarrow→ 2AB k,slow

If the average rate of formation of H2(g)is 3.90 (mol H2).L-1.s-1 for the reaction 2PH3(g) →\rightarrow→ 2P(g)+ 3H2(g),the unique average reaction rate is

For the reaction 2A + B →\rightarrow→ products Determine the rate law for the reaction given the following data:

The concentration-time curves for two sets of reactions,A/B and C/D,are: Which of the reactions are first order?

The reaction 2ClO2(g)+ F2(g) →\rightarrow→ 2FClO2(g) Is first order in both ClO2 and F2.When the initial concentrations of ClO2 and F2 are equal,the rate after 25% of the F2 has reacted is what percent of the initial rate?

Given: CH4(g)+ Cl2(g) →\rightarrow→ CH3Cl(g)+ HCl(g) The rate law for this elementary process is

Given: A →\rightarrow→ P rate = k[A] If 20% of A reacts in 5.12 min,calculate the time required for 90% of A to react.

For the proposed mechanism A + X → B k1,k-1 (fast) B →\rightarrow→ products k2 (slow) What is the rate law?

Consider the mechanism NO2(g)+ F2(g) →\rightarrow→ NO2F(g)+ F(g)k1 (slow) F(g)+ NO2(g) →\rightarrow→ NO2F(g)k2 (fast) Give the molecularity of the first step and any intermediates in the mechanism.

Given: 2O3(g) →\rightarrow→ 3O2(g) Rate = k[O3]2[O2]-1 The overall order of the reaction and the order with respect to [O3] are

The rate law for the following mechanism is NO2(g)+ F2(g) →\rightarrow→ NO2F(g)+ F(g) K1,slow F(g)+ NO2(g) →\rightarrow→ NO2F(g) K2,fast

The concentration-time dependence for a first-order reaction is: At which point on the curve is the reaction fastest?

If the rate of reaction increases by a factor of 2.3 when the concentration of reactant increases by a factor of 1.5,the order of the reaction with respect to this reactant is

The Quantum World

Quantum Mechanics in Action: Atoms

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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2A →A₂ K,fast B₂ + A₂ $\rightarrow$ 2AB k,slow

If the average rate of formation of H₂(g)is 3.90 (mol H₂).L^-1.s^-1 for the reaction 2PH₃(g) $\rightarrow$ 2P(g)+ 3H₂(g),the unique average reaction rate is

For the reaction 2A + B $\rightarrow$ products Determine the rate law for the reaction given the following data: $For the reaction 2A + B \rightarrow products Determine the rate law for the reaction given the following data:$

The reaction 2ClO₂(g)+ F₂(g) $\rightarrow$ 2FClO₂(g) Is first order in both ClO₂ and F₂.When the initial concentrations of ClO₂ and F₂ are equal,the rate after 25% of the F₂ has reacted is what percent of the initial rate?

Given: CH₄(g)+ Cl₂(g) $\rightarrow$ CH₃Cl(g)+ HCl(g) The rate law for this elementary process is

Given: A $\rightarrow$ P rate = k[A] If 20% of A reacts in 5.12 min,calculate the time required for 90% of A to react.

For the proposed mechanism A + X → B k₁,k_-1(fast) B $\rightarrow$ products k₂ (slow) What is the rate law?

Consider the mechanism NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g)k₁ (slow) F(g)+ NO₂(g) $\rightarrow$ NO₂F(g)k₂ (fast) Give the molecularity of the first step and any intermediates in the mechanism.

Given: 2O₃(g) $\rightarrow$ 3O₂(g) Rate = k[O₃]²[O₂]^-1 The overall order of the reaction and the order with respect to [O₃] are

The rate law for the following mechanism is NO₂(g)+ F₂(g) $\rightarrow$ NO₂F(g)+ F(g) K₁,slow F(g)+ NO₂(g) $\rightarrow$ NO₂F(g) K₂,fast