Question 1

Define half-life.

Accepted Answer

A half-life of a reaction is t

Question 2

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 O2 is 0.28 M s-1,the rate of appearance of CO2 is
________ M s-1.

Accepted Answer

A)  0.19 
B)  0.093 
C)  0.84 
D)  0.42 
E)  0.56 
A)  0.19 
B)  0.093 
C)  0.84 
D)  0.42 
E)  0.56

Question 3

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

Accepted Answer

A)  NOCl(g) + NOCl(g) → 2 NO(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) → 2 NO(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 4

The rate constant for a second-order reaction is 0.54 M-1s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Accepted Answer

A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s 
A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s

Question 5

What happens in the concentration of reactants and products during a chemical reaction?

Accepted Answer

The concentration of reactants

Question 6

Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g)→ 4 NO2(g)+ O2(g)[N2O5]i (M)Initial Rate (M-1s-1)
0)093 4.84 × 10-4
0)084 4.37 × 10-4
0)224 1.16 × 10-3

Accepted Answer

A)  Rate = 5.6 × 10-2 M-1s-1[N2O5]2 
B)  Rate = 6.0 × 10-1 M-2s-1[N2O5]3 
C)  Rate = 1.6 × 10-3 M1/2s-1[N2O5]1/2 
D)  Rate = 1.7 × 10-2 M-1/2s-1[N2O5]3/2 
E)  Rate = 5.2 × 10⁻3 s-1[N2O5] 
A)  Rate = 5.6 × 10-2 M-1s-1[N2O5]2 
B)  Rate = 6.0 × 10-1 M-2s-1[N2O5]3 
C)  Rate = 1.6 × 10-3 M1/2s-1[N2O5]1/2 
D)  Rate = 1.7 × 10-2 M-1/2s-1[N2O5]3/2 
E)  Rate = 5.2 × 10⁻3 s-1[N2O5]

Question 7

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A][B]2,what is the new rate if the concentration of [A] is increased to 0.200 M?

Accepted Answer

A)  0.0200 M/s 
B)  0.0400 M/s 
C)  0.0600 M/s 
D)  0.0800 M/s 
E)  0.100 M/s 
A)  0.0200 M/s 
B)  0.0400 M/s 
C)  0.0600 M/s 
D)  0.0800 M/s 
E)  0.100 M/s

Question 8

The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g)
If the rate of appearance of O2 is equal to 3.00 mol/min at a particular moment,what is the rate of disappearance of N2O5 at that moment?

Accepted Answer

A)  0.750 mol/min 
B)  1.50 mol/min 
C)  6.00 mol/min 
D)  12.0 mol/min 
A)  0.750 mol/min 
B)  1.50 mol/min 
C)  6.00 mol/min 
D)  12.0 mol/min

Question 9

What is a catalyst and what function does it serve?

Accepted Answer

A catalyst is a substance that is not us

Question 10

Which rate law is termolecular?

Accepted Answer

A)  rate = k[A]2[B]  
B)  rate = k [A] [B]3 
C)  rate = k [A]  
D)  rate = k [A][B][C][D] 
E)  rate = k [A]2 
A)  rate = k[A]2[B]  
B)  rate = k [A] [B]3 
C)  rate = k [A]  
D)  rate = k [A][B][C][D] 
E)  rate = k [A]2

Question 11

Which rate law has a molecularity of one?

Accepted Answer

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

Question 12

The elementary reaction 2 NO2(g)→ 2 NO(g)+ O2(g)
Is second order in NO2 and the rate constant at 501 K is 7.93 × 10-3 M-1s-1.The reaction half-life at this temperature when [NO2]0 = 0.45 M is ________ s.

Accepted Answer

A)  3.6 × 10-3 
B)  0.011 
C)  126 
D)  87 
E)  280 
A)  3.6 × 10-3 
B)  0.011 
C)  126 
D)  87 
E)  280

Question 13

A gas chromatograph can be used to determine the relative amounts of reactants and products by

Accepted Answer

A)  measuring the changes in pressure as the reaction proceeds. 
B)  analyzing the intensity of the transmitted light. 
C)  separating the components of the mixture, which results in an individual peak for each component and the peaks are quantified. 
D)  measuring the degree of the polarization of light. 
E)  measuring the change in temperature of the reaction. 
A)  measuring the changes in pressure as the reaction proceeds. 
B)  analyzing the intensity of the transmitted light. 
C)  separating the components of the mixture, which results in an individual peak for each component and the peaks are quantified. 
D)  measuring the degree of the polarization of light. 
E)  measuring the change in temperature of the reaction.

Question 14

The isomerization of methylisonitrile to acetonitrile CH3NC(g)→ CH3CN(g)
Is first order in CH3NC.The half-life of the reaction is 5.20 × 101 s at 545 K.The rate constant when the initial [CH3NC] is 0.030 M is ________ s-1.

Accepted Answer

A)  75.1 
B)  0.641 
C)  0.0133 
D)  1.56 
E)  2.84 × 104 
A)  75.1 
B)  0.641 
C)  0.0133 
D)  1.56 
E)  2.84 × 104

Question 15

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

Accepted Answer

A)  4.21 g 
B)  183 g 
C)  54.8 g 
D)  76.3 g 
E)  67.5 g 
A)  4.21 g 
B)  183 g 
C)  54.8 g 
D)  76.3 g 
E)  67.5 g

Question 16

What function do enzymes serve?

Accepted Answer

They are biological catalysts.They lower

Question 17

Which rate law is bimolecular?

Accepted Answer

A)  rate = k[A]5[B]3 
B)  rate = k[A][B] 
C)  rate = k[A]3 
D)  rate = k[A][B][C][D] 
E)  rate = k[A]2[B]4 
A)  rate = k[A]5[B]3 
B)  rate = k[A][B] 
C)  rate = k[A]3 
D)  rate = k[A][B][C][D] 
E)  rate = k[A]2[B]4

Question 18

Give the characteristic of a second-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 19

Which of the following represents the integrated rate law for a zeroth-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 20

Which of the following represents the equation for a second-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]o 
A)  t 1/2 =   
B)  t 1/2 =   
C)  t 1/2 =   
D)  t 1/2 =   
E)  t 1/2 = [A]o

Exam 14: Chemical Kinetics

Define half-life.

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 O2 is 0.28 M s-1,the rate of appearance of CO2 is ________ M s-1.

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

The rate constant for a second-order reaction is 0.54 M-1s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

What happens in the concentration of reactants and products during a chemical reaction?

Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g)→ 4 NO2(g)+ O2(g)[N2O5]i (M)Initial Rate (M-1s-1) 0)093 4.84 × 10-4 0)084 4.37 × 10-4 0)224 1.16 × 10-3

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A][B]2,what is the new rate if the concentration of [A] is increased to 0.200 M?

The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g) If the rate of appearance of O2 is equal to 3.00 mol/min at a particular moment,what is the rate of disappearance of N2O5 at that moment?

What is a catalyst and what function does it serve?

Which rate law is termolecular?

Which rate law has a molecularity of one?

The elementary reaction 2 NO2(g)→ 2 NO(g)+ O2(g) Is second order in NO2 and the rate constant at 501 K is 7.93 × 10-3 M-1s-1.The reaction half-life at this temperature when [NO2]0 = 0.45 M is ________ s.

A gas chromatograph can be used to determine the relative amounts of reactants and products by

The isomerization of methylisonitrile to acetonitrile CH3NC(g)→ CH3CN(g) Is first order in CH3NC.The half-life of the reaction is 5.20 × 101 s at 545 K.The rate constant when the initial [CH3NC] is 0.030 M is ________ s-1.

The first-order decay of radon has a half-life of 3.823 days.How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

What function do enzymes serve?

Which rate law is bimolecular?

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

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

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

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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 O₂ is 0.28 M s^-1,the rate of appearance of CO₂ is ________ M s^-1.

The rate constant for a second-order reaction is 0.54 M^-1s^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Determine the rate law and the value of k for the following reaction using the data provided. 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g)[N₂O₅]_i (M)Initial Rate (M^-1s^-1) 0)093 4.84 × 10^-4 0)084 4.37 × 10^-4 0)224 1.16 × 10^-3

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A][B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g) If the rate of appearance of O₂ is equal to 3.00 mol/min at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

The elementary reaction 2 NO₂(g)→ 2 NO(g)+ O₂(g) Is second order in NO₂ and the rate constant at 501 K is 7.93 × 10^-3 M^-1s^-1.The reaction half-life at this temperature when [NO₂]₀ = 0.45 M is ________ s.

The isomerization of methylisonitrile to acetonitrile CH₃NC(g)→ CH₃CN(g) Is first order in CH₃NC.The half-life of the reaction is 5.20 × 10¹ s at 545 K.The rate constant when the initial [CH₃NC] is 0.030 M is ________ s^-1.