Question 1

What are the units of k in the following rate law?
Rate = k[X][Y]

Accepted Answer

A)    
B)  Ms 
C)    
D)    
E)    
A)    
B)  Ms 
C)    
D)    
E)

Question 2

Which of the following reactions would you predict to have the largest orientation factor?

Accepted Answer

A)  NOCl(g) + NOCl(g) → 2NO(g) + Cl2(g) 
B)  Br2(g) + H2C=CH2(g) → H2BrC-CBrH2(g) 
C)  NH3(g) + BCl3(g) → H3N-BCl3(g) 
D)  H(g) + F(g) → HF(g) 
E)  All of these reactions should have nearly identical orientation factors. 
A)  NOCl(g) + NOCl(g) → 2NO(g) + Cl2(g) 
B)  Br2(g) + H2C=CH2(g) → H2BrC-CBrH2(g) 
C)  NH3(g) + BCl3(g) → H3N-BCl3(g) 
D)  H(g) + F(g) → HF(g) 
E)  All of these reactions should have nearly identical orientation factors.

Question 3

What are the units of k in a zero order reaction?

Accepted Answer

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

Question 4

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

Accepted Answer

A)  6 
B)  4 
C)  24 
D)  6.5 
E)  7.5 
A)  6 
B)  4 
C)  24 
D)  6.5 
E)  7.5

Question 5

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2HI(g)→ H2(g)+ I2(g)
At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 M to 3.50 × 10-2 M.What is the rate constant for the reaction at this temperature?

Accepted Answer

A)  5.12 × 10-4 M-1s-1 
B)  9.69 × 10-2 M-1s-1 
C)  10.3 M-1s-1 
D)  1.95 × 103 M-1s-1 
A)  5.12 × 10-4 M-1s-1 
B)  9.69 × 10-2 M-1s-1 
C)  10.3 M-1s-1 
D)  1.95 × 103 M-1s-1

Question 6

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Accepted Answer

A)  83.4 g 
B)  16.6 g 
C)  50.0 g 
D)  36.6 g 
E)  63.4 g 
A)  83.4 g 
B)  16.6 g 
C)  50.0 g 
D)  36.6 g 
E)  63.4 g

Question 7

Determine the rate law and the value of k for the following reaction using the data provided. NO2(g)+ O3(g)→ NO3(g)+ O2(g)[NO2]i (M)[O3]i (M)Initial Rate
0)10 0.33 1.42
0)10 0.66 2.84
0)25 0.66 7.10

Accepted Answer

A)  Rate = 1360 M-2.5s-1[NO2]2.5[O3] 
B)  Rate = 227 M-2.5s-1[NO2][O3]2.5 
C)  Rate = 43 M-1s-1[NO2][O3] 
D)  Rate = 430 M-2s-1[NO2]2[O3] 
E)  Rate = 130 M-2s-1[NO2][O3]2 
A)  Rate = 1360 M-2.5s-1[NO2]2.5[O3] 
B)  Rate = 227 M-2.5s-1[NO2][O3]2.5 
C)  Rate = 43 M-1s-1[NO2][O3] 
D)  Rate = 430 M-2s-1[NO2]2[O3] 
E)  Rate = 130 M-2s-1[NO2][O3]2

Question 8

A reaction has a rate constant of 4.61 × 10-4 M-1 s-1 at 34°C,and a rate constant of 5.87 × 10-3 M-1 s-1 at 67°C.What is the activation energy?

Accepted Answer

A)  104 kJ/mol 
B)  92.6 kJ/mol 
C)  35.1 kJ/mol 
D)  67.0 kJ/mol 
E)  79.3 kJ/mol 
A)  104 kJ/mol 
B)  92.6 kJ/mol 
C)  35.1 kJ/mol 
D)  67.0 kJ/mol 
E)  79.3 kJ/mol

Question 9

Given the following balanced equation,determine the rate of reaction with respect to [NOCl]. 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

Accepted Answer

A)  Rate = -     
B)  Rate = +     
C)  Rate = -     
D)  Rate = -   
E)  It is not possible to determine without more information. 
A)  Rate = -     
B)  Rate = +     
C)  Rate = -     
D)  Rate = -   
E)  It is not possible to determine without more information.

Question 10

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl2(g)→ COCl2(g)[CO]i (M)[Cl2]i (M)Initial Rate
0)25 0.40 0.696
0)25 0.80 1.97
0)50 0.80 3.94

Accepted Answer

A)  Rate = 11 M-3/2s-1 [CO][Cl2]3/2 
B)  Rate = 36 M-1.8s-1 [CO][Cl2]2.8 
C)  Rate = 17 M-2s-1 [CO][Cl2]2 
D)  Rate = 4.4 M-1/2s-1 [CO][Cl2]1/2 
E)  Rate = 18 M-3/2s-1 [CO]2[Cl2]1/2 
A)  Rate = 11 M-3/2s-1 [CO][Cl2]3/2 
B)  Rate = 36 M-1.8s-1 [CO][Cl2]2.8 
C)  Rate = 17 M-2s-1 [CO][Cl2]2 
D)  Rate = 4.4 M-1/2s-1 [CO][Cl2]1/2 
E)  Rate = 18 M-3/2s-1 [CO]2[Cl2]1/2

Question 11

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Accepted Answer

A)  1 
B)  4 
C)  1.5 
D)  3.5 
E)  2 
A)  1 
B)  4 
C)  1.5 
D)  3.5 
E)  2

Question 12

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→2CO2(g)+ 2H2O(g)
When the rate of disappearance of O2 is 0.23 M s-1,the rate of disappearance of C2H4 is ________ M s-1.

Accepted Answer

A)  0.15 
B)  0.077 
C)  0.69 
D)  0.35 
E)  0.46 
A)  0.15 
B)  0.077 
C)  0.69 
D)  0.35 
E)  0.46

Question 13

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Accepted Answer

A)  0.143 hr 
B)  2.28 hr 
C)  6.99 hr 
D)  22.7 hr 
A)  0.143 hr 
B)  2.28 hr 
C)  6.99 hr 
D)  22.7 hr

Question 14

A reaction has a rate constant of 5.5 × 10-2 M-1s-1.If you start with an initial concentration of 3.82M,what is the half-life?

Accepted Answer

A)  3.82 s 
B)  7.0 s 
C)  12.6 s 
D)  4.76 s 
A)  3.82 s 
B)  7.0 s 
C)  12.6 s 
D)  4.76 s

Question 15

Which of the following represents the equation for a zero-order half-life?

Accepted Answer

A)  t 1/2 =   
B)  t 1/2 =   
C)  t 1/2 =   
D)  t 1/2 =   
E)  t 1/2 =   
A)  t 1/2 =   
B)  t 1/2 =   
C)  t 1/2 =   
D)  t 1/2 =   
E)  t 1/2 =

What are the units of k in the following rate law? Rate = k[X][Y]

Which of the following reactions would you predict to have the largest orientation factor?

What are the units of k in a zero order reaction?

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Determine the rate law and the value of k for the following reaction using the data provided. NO₂(g)+ O₃(g)→ NO₃(g)+ O₂(g)[NO₂]_i(M)[O₃]_i (M)Initial Rate 0)10 0.33 1.42 0)10 0.66 2.84 0)25 0.66 7.10

A reaction has a rate constant of 4.61 × 10^-4 M^-1 s^-1 at 34°C,and a rate constant of 5.87 × 10^-3 M^-1 s^-1 at 67°C.What is the activation energy?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl]. 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl₂(g)→ COCl₂(g)[CO]_i(M)[Cl₂]_i (M)Initial Rate 0)25 0.40 0.696 0)25 0.80 1.97 0)50 0.80 3.94

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

The combustion of ethylene proceeds by the reaction C₂H₄(g)+ 3O₂(g)→2CO₂(g)+ 2H₂O(g) When the rate of disappearance of O₂ is 0.23 M s^-1,the rate of disappearance of C₂H₄ is ________ M s^-1.

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

A reaction has a rate constant of 5.5 × 10^-2 M^-1s^-1.If you start with an initial concentration of 3.82M,what is the half-life?

Which of the following represents the equation for a zero-order half-life?

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Exam 15: Chemical Kinetics

What are the units of k in the following rate law? Rate = k[X][Y]

Which of the following reactions would you predict to have the largest orientation factor?

What are the units of k in a zero order reaction?

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Determine the rate law and the value of k for the following reaction using the data provided. NO2(g)+ O3(g)→ NO3(g)+ O2(g)[NO2]i (M)[O3]i (M)Initial Rate 0)10 0.33 1.42 0)10 0.66 2.84 0)25 0.66 7.10

A reaction has a rate constant of 4.61 × 10-4 M-1 s-1 at 34°C,and a rate constant of 5.87 × 10-3 M-1 s-1 at 67°C.What is the activation energy?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl]. 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl2(g)→ COCl2(g)[CO]i (M)[Cl2]i (M)Initial Rate 0)25 0.40 0.696 0)25 0.80 1.97 0)50 0.80 3.94

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→2CO2(g)+ 2H2O(g) When the rate of disappearance of O2 is 0.23 M s-1,the rate of disappearance of C2H4 is ________ M s-1.

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

A reaction has a rate constant of 5.5 × 10-2 M-1s-1.If you start with an initial concentration of 3.82M,what is the half-life?

Which of the following represents the equation for a zero-order half-life?

Essentials: Units, Measurements, and Problem Solving

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The Quantum Mechanical Model of the Atom

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Gases

Liquids, Solids, and Intermolecular Forces

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Determine the rate law and the value of k for the following reaction using the data provided. NO₂(g)+ O₃(g)→ NO₃(g)+ O₂(g)[NO₂]_i(M)[O₃]_i (M)Initial Rate 0)10 0.33 1.42 0)10 0.66 2.84 0)25 0.66 7.10

A reaction has a rate constant of 4.61 × 10^-4 M^-1 s^-1 at 34°C,and a rate constant of 5.87 × 10^-3 M^-1 s^-1 at 67°C.What is the activation energy?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl]. 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl₂(g)→ COCl₂(g)[CO]_i(M)[Cl₂]_i (M)Initial Rate 0)25 0.40 0.696 0)25 0.80 1.97 0)50 0.80 3.94

The combustion of ethylene proceeds by the reaction C₂H₄(g)+ 3O₂(g)→2CO₂(g)+ 2H₂O(g) When the rate of disappearance of O₂ is 0.23 M s^-1,the rate of disappearance of C₂H₄ is ________ M s^-1.

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

A reaction has a rate constant of 5.5 × 10^-2 M^-1s^-1.If you start with an initial concentration of 3.82M,what is the half-life?