Question 1

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon decompose 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 2

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

Accepted Answer

A)    
B)  M s2 
C)    
D)    
E)    
A)    
B)  M s2 
C)    
D)    
E)

Question 3

Given the following proposed mechanism,predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction)
Mechanism
NO2 + Cl2 → NO2Cl + Cl slow
NO2 + Cl → NO2Cl fast

Accepted Answer

A)  Rate = k[NO2][Cl2] 
B)  Rate = k[NO2]2[Cl2]2 
C)  Rate = k[NO2] [Cl]2 
D)  Rate = k[NO2Cl][Cl]  
E)  Rate = k[NO2Cl]2[Cl] 
A)  Rate = k[NO2][Cl2] 
B)  Rate = k[NO2]2[Cl2]2 
C)  Rate = k[NO2] [Cl]2 
D)  Rate = k[NO2Cl][Cl]  
E)  Rate = k[NO2Cl]2[Cl]

Question 4

Identify an heterogeneous catalyst.

Accepted Answer

A)  CFCs with ozone 
B)  Pd in H2 gas 
C)  KI dissolved in H2O2 
D)  H2SO4 with concentrated HCl 
E)  H3PO4 with an alcohol 
A)  CFCs with ozone 
B)  Pd in H2 gas 
C)  KI dissolved in H2O2 
D)  H2SO4 with concentrated HCl 
E)  H3PO4 with an alcohol

Question 5

Which of the following represents the integrated rate law for a first-order reaction?

Accepted Answer

A)    = - kt 
B)    -
  = -kt 
C)  [A]t - [A]o = kt 
D)  k = Ae(Ea/RT) 
E)    =
 
  + lnA 
A)    = - kt 
B)    -
  = -kt 
C)  [A]t - [A]o = kt 
D)  k = Ae(Ea/RT) 
E)    =
 
  + lnA

Question 6

The second-order reaction 2 Mn(CO)5 → Mn2(CO)10,has a rate constant equal to 3.0 × 109 M-1 s-1 at 25°C.If the initial concentration of Mn(CO)5 is 2.0 × 10-5 M,how long will it take for 90.% of the reactant to disappear?

Accepted Answer

A)  6.7 × 10-16 s 
B)  7.4 × 10-15 s 
C)  1.5 × 10-4 s 
D)  6.0 × 103 s 
A)  6.7 × 10-16 s 
B)  7.4 × 10-15 s 
C)  1.5 × 10-4 s 
D)  6.0 × 103 s

Question 7

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K,what is the rate constant at 366 K?

Accepted Answer

A)  12 s-1 
B)  1.7 s-1 
C)  0.58 s-1 
D)  5.4 × 10-5 s-1 
E)  1.9 × 10-4 s-1 
A)  12 s-1 
B)  1.7 s-1 
C)  0.58 s-1 
D)  5.4 × 10-5 s-1 
E)  1.9 × 10-4 s-1

Question 8

Given the following balanced equation,determine the rate of reaction with respect to [SO2]. 2 SO2(g)+ O2(g)→ 2 SO3(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 9

Given the following rate law,how does the rate of reaction change if the concentration of X is doubled? Rate = k[X][Y]3

Accepted Answer

A)  The rate of reaction will increase by a factor of 2. 
B)  The rate of reaction will increase by a factor of 8. 
C)  The rate of reaction will increase by a factor of 6. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged. 
A)  The rate of reaction will increase by a factor of 2. 
B)  The rate of reaction will increase by a factor of 8. 
C)  The rate of reaction will increase by a factor of 6. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged.

Question 10

If the activation energy for a given compound is found to be 103 kJ/mol,with a frequency factor of 4.0 × 1013 s-1,what is the rate constant for this reaction at 398 K?

Accepted Answer

A)  1.2 s-1 
B)  8.2 s-1 
C)  3.9 × 1010 s-1 
D)  1.7 × 1010 s-1 
E)  2.5 × 107 s-1 
A)  1.2 s-1 
B)  8.2 s-1 
C)  3.9 × 1010 s-1 
D)  1.7 × 1010 s-1 
E)  2.5 × 107 s-1

Question 11

What is the overall reaction order for the reaction that has the rate law: Rate = k[F2]2[NO]?

Accepted Answer

A)  zero order 
B)  first order 
C)  second order 
D)  third order 
A)  zero order 
B)  first order 
C)  second order 
D)  third order

Question 12

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of Cl2 loss is 4.24 × 10-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

Accepted Answer

A)  4.24 × 10-2 M/s 
B)  2.12 × 10-2 M/s 
C)  1.06 × 10-1 M/s 
D)  8.48 × 10-2 M/s 
E)  1.61 × 10-2 M/s 
A)  4.24 × 10-2 M/s 
B)  2.12 × 10-2 M/s 
C)  1.06 × 10-1 M/s 
D)  8.48 × 10-2 M/s 
E)  1.61 × 10-2 M/s

Question 13

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K.Determine the activation energy for this reaction.

Accepted Answer

A)  160. kJ/mol 
B)  240. kJ/mol 
C)  417 kJ/mol 
D)  127 kJ/mol 
E)  338 kJ/mol 
A)  160. kJ/mol 
B)  240. kJ/mol 
C)  417 kJ/mol 
D)  127 kJ/mol 
E)  338 kJ/mol

Question 14

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3 O2(g)→ 2 CO2(g)+ 2 H2O(g)
When the rate of disappearance of   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 15

Carbon-14 has a half-life of 5720 years and this is a first-order reaction.If a piece of wood has converted 75% of the carbon-14,then how old is it?

Accepted Answer

A)  11440 years 
B)  2375 years 
C)  4750 years 
D)  4290 years 
E)  1430 years 
A)  11440 years 
B)  2375 years 
C)  4750 years 
D)  4290 years 
E)  1430 years

Question 16

What is the overall order of the following reaction,given the rate law? X + 2Y → 4Z Rate = k[X][Y]

Accepted Answer

A)  3rd order 
B)  5th order 
C)  2nd order 
D)  1st order 
E)  6th order 
A)  3rd order 
B)  5th order 
C)  2nd order 
D)  1st order 
E)  6th order

Question 17

Give the characteristic of a zero-order reaction having only one reactant.

Accepted Answer

A)  The rate of the reaction is not proportional to the concentration of the reactant. 
B)  The rate of the reaction is proportional to the square of the concentration of the reactant. 
C)  The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D)  The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E)  The rate of the reaction is directly proportional to the concentration of the reactant. 
A)  The rate of the reaction is not proportional to the concentration of the reactant. 
B)  The rate of the reaction is proportional to the square of the concentration of the reactant. 
C)  The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D)  The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E)  The rate of the reaction is directly proportional to the concentration of the reactant.

Question 18

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

Accepted Answer

A)  decrease by a factor of 1/25.0. 
B)  decrease by a factor of 1/5.00. 
C)  increase by a factor of 5.00. 
D)  increase by a factor of 25.0. 
A)  decrease by a factor of 1/25.0. 
B)  decrease by a factor of 1/5.00. 
C)  increase by a factor of 5.00. 
D)  increase by a factor of 25.0.

Question 19

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k[X][Y]

Accepted Answer

A)  The rate of reaction will increase by a factor of 2. 
B)  The rate of reaction will increase by a factor of 4. 
C)  The rate of reaction will decrease by a factor of 5. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged. 
A)  The rate of reaction will increase by a factor of 2. 
B)  The rate of reaction will increase by a factor of 4. 
C)  The rate of reaction will decrease by a factor of 5. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged.

Question 20

Given the following balanced equation,determine the rate of reaction with respect to [HCl]. H2(g)+ Cl2(g)→ 2 HCl(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.

Exam 14: Chemical Kinetics

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

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

Given the following proposed mechanism,predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast

Identify an heterogeneous catalyst.

Which of the following represents the integrated rate law for a first-order reaction?

The second-order reaction 2 Mn(CO)5 → Mn2(CO)10,has a rate constant equal to 3.0 × 109 M-1 s-1 at 25°C.If the initial concentration of Mn(CO)5 is 2.0 × 10-5 M,how long will it take for 90.% of the reactant to disappear?

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K,what is the rate constant at 366 K?

Given the following balanced equation,determine the rate of reaction with respect to [SO2]. 2 SO2(g)+ O2(g)→ 2 SO3(g)

Given the following rate law,how does the rate of reaction change if the concentration of X is doubled? Rate = k[X][Y]3

If the activation energy for a given compound is found to be 103 kJ/mol,with a frequency factor of 4.0 × 1013 s-1,what is the rate constant for this reaction at 398 K?

What is the overall reaction order for the reaction that has the rate law: Rate = k[F2]2[NO]?

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of Cl2 loss is 4.24 × 10-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K.Determine the activation energy for this reaction.

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

Carbon-14 has a half-life of 5720 years and this is a first-order reaction.If a piece of wood has converted 75% of the carbon-14,then how old is it?

What is the overall order of the following reaction,given the rate law? X + 2Y → 4Z Rate = k[X][Y]

Give the characteristic of a zero-order reaction having only one reactant.

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k[X][Y]

Given the following balanced equation,determine the rate of reaction with respect to [HCl]. H2(g)+ Cl2(g)→ 2 HCl(g)

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Given the following proposed mechanism,predict the rate law for the overall reaction. 2 NO₂ + Cl₂ → 2 NO₂Cl (overall reaction) Mechanism NO₂ + Cl₂ → NO₂Cl + Cl slow NO₂ + Cl → NO₂Cl fast

The second-order reaction 2 Mn(CO)₅ → Mn₂(CO)₁₀,has a rate constant equal to 3.0 × 10⁹ M^-1 s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 2.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

A reaction is found to have an activation energy of 108 kJ/mol.If the rate constant for this reaction is 4.60 × 10^-6s^-1 at 275 K,what is the rate constant at 366 K?

Given the following balanced equation,determine the rate of reaction with respect to [SO₂]. 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)

Given the following rate law,how does the rate of reaction change if the concentration of X is doubled? Rate = k[X][Y]³

If the activation energy for a given compound is found to be 103 kJ/mol,with a frequency factor of 4.0 × 10¹³ s^-1,what is the rate constant for this reaction at 398 K?

What is the overall reaction order for the reaction that has the rate law: Rate = k[F₂]²[NO]?

Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of Cl₂ loss is 4.24 × 10^-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15s^-1 at 298 K and a rate constant of 8.66 × 10^-7s^-1 at 425 K.Determine the activation energy for this reaction.

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

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

Given the following balanced equation,determine the rate of reaction with respect to [HCl]. H₂(g)+ Cl₂(g)→ 2 HCl(g)