Question 1

The aquation of tris(1,10-phenanthroline) iron(II) in acid solution takes place according to the equation:
Fe(phen) 32+ + 3 H3O+ + 3 H2O → Fe(H2O) 62+ + 3 phenH+.
If the activation energy,Ea,is 126 kJ/mol and the rate constant at 30°C is 9.8 × 10-3 min-1,what is the rate constant at 35°C?

Accepted Answer

A)  4) 4 × 10- 3 min-1
B)  2) 2 × 10- 2 min-1
C)  4) 5 × 101 min-1
D)  2) 3 × 102 min-1E) All of the above
F) C) and D)

Question 2

What is the minimum energy barrier that must be overcome for a chemical reaction to occur?

Accepted Answer

A)  activation energy
B)  net energy
C)  potential energy
D)  rate limiting energyE) None of the above
F) A) and D)

Question 3

The rate constant,k,for a first-order reaction is equal to 4.2 × 10-4 s-1.What is the half-life for the reaction?

Accepted Answer

A)  2) 9 × 10-4 s
B)  1) 2 × 103 s
C)  1) 7 × 103 s
D)  2) 4 × 103 sE) A) and B)
F) A) and C)

Question 4

The decay curve shown below approximates the decay of phosphorus-32.What is the approximate half-life of phosphorus-32?

Accepted Answer

A)  14 days
B)  27 days
C)  35 days
D)  37.5 daysE) B) and D)
F) A) and C)

Question 5

The first-order decomposition of hydrogen peroxide occurs according to the equation
2 H2O2(aq) → 2 H2O(l) + O2(g) 
Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Accepted Answer

A)  [H2O2] versus time
B)  [H2O2]2 versus time
C)  1/[H2O2] versus time
D)  ln[H2O2] versus timeE) B) and C)
F) A) and D)

Question 6

The decomposition of dinitrogen pentoxide is described by the chemical equation
2 N2O5(g) → 4 NO2(g) + O2(g) 
If the rate of disappearance of N2O5 is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO2 at that moment?

Accepted Answer

A)  0) 700 mol/min
B)  1) 40 mol/min
C)  2) 80 mol/min
D)  5) 60 mol/minE) B) and D)
F) A) and B)

Question 7

If the units for rate are M s-1,what are the units for the rate constant,k,if the overall order of the reaction is three?

Accepted Answer

A)  s-1
B)  M2 s-1
C)  M-1 s-1
D)  M-2 s-1E) A) and B)
F) A) and C)

Question 8

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. 
-Which equation best represents the reaction?

Accepted Answer

A)  4A(g) → B(g) + 2C(g) 
B)  4A(g) + B(g) → 2C(g) 
C)  2C(g) → 4A(g) + B(g) 
D)  2C(g) + B(g) → 4A(g) E) A) and B)
F) C) and D)

Question 9

In aqueous solution,hypobromite ion,BrO-,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation. -,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation.   A plot of 1/[BrO-] vs.time is linear and the slope is equal to 0.056 M-1s-1.If the initial concentration of BrO- is 0.80 M,how long will it take one-half of the BrO- ion to react? A) 4) 5 × 10-2 s B) 7) 1 s C) 12 s D) 22 s" class="answers-bank-image d-inline" rel="preload" >
A plot of 1/[BrO-] vs.time is linear and the slope is equal to 0.056 M-1s-1.If the initial concentration of BrO- is 0.80 M,how long will it take one-half of the BrO- ion to react?

Accepted Answer

A)  4) 5 × 10-2 s
B)  7) 1 s
C)  12 s
D)  22 sE) All of the above
F) A) and D)

Question 10

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -5 M/s.Over the same time interval what is the rate of reaction with respect to B,Δ[B]/Δt? A) Δ[B]/Δt = Δ[A]/Δt = 3.7 × 10-5 M/s B) Δ[B]/Δt = (1/4) (Δ[A]/Δt) = (1/4) (3.7 × 10-5 M/s) = 9.2 × 10-6 M/s C) Δ[B]/Δt = (1/2) (Δ[A]/Δt) = (1/2) (3.7 × 10-5 M/s) = 1.8 × 10-5 M/s D) Δ[B]/Δt = -(1/2) (Δ[A]/Δt) = -(1/2) (3.7 × 10-5 M/s) = -1.8 × 10-5 M/s" class="answers-bank-image d-inline" rel="preload" >
-Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10-5 M/s.Over the same time interval what is the rate of reaction with respect to B,Δ[B]/Δt?

Accepted Answer

A)  Δ[B]/Δt = Δ[A]/Δt = 3.7 × 10-5 M/s
B)  Δ[B]/Δt = (1/4) (Δ[A]/Δt) = (1/4) (3.7 × 10-5 M/s) = 9.2 × 10-6 M/s
C)  Δ[B]/Δt = (1/2) (Δ[A]/Δt) = (1/2) (3.7 × 10-5 M/s) = 1.8 × 10-5 M/s
D)  Δ[B]/Δt = -(1/2) (Δ[A]/Δt) = -(1/2) (3.7 × 10-5 M/s) = -1.8 × 10-5 M/sE) A) and B)
F) C) and D)

Question 11

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 sE) A) and C)
F) C) and D)

Question 12

Consider a reaction that occurs by the following mechanism:
A + BC → AC + B
AC + D → A + CD
The potential energy profile for this reaction is shown below. 
-Transition states occur at which reaction stages?

Accepted Answer

A)  reaction stages 1 and 5
B)  reaction stages 2,3,and 4
C)  reaction stages 2 and 4
D)  reaction stage 3E) A) and B)
F) A) and C)

Question 13

The decomposition of dinitrogen pentoxide is described by the chemical equation
2 N2O5(g) → 4 NO2(g) + O2(g) 
If the rate of appearance of NO2 is equal to 0.560 mol/min at a particular moment,what is the rate of appearance of O2 at that moment?

Accepted Answer

A)  0) 140 mol/min
B)  0) 280 mol/min
C)  1) 12 mol/min
D)  2) 24 mol/minE) A) and B)
F) A) and C)

Question 14

Decays by electron capture to give If unshaded spheres represent  Atoms and shaded spheres represent Atoms,how many half-lives have passed in the following example?

Accepted Answer

A)  1 half-life
B)  2 half-lives
C)  3 half-lives
D)  4 half-livesE) A) and C)
F) B) and D)

Question 15

A common rule of thumb in organic chemistry is that increasing the temperature of a reaction at room temperature by 10°C doubles the rate.Calculate Ea for a reaction that follows this rule of thumb Assume room temperature is 25°C.

Accepted Answer

A)  0) 576 kJ
B)  12.2 kJ
C)  38.4 kJ
D)  52.9 kJE) B) and C)
F) A) and C)

Question 16

A gaseous reaction occurs by a two-step mechanism,shown below.
Step 1: AX +Y2 → AXY2
Step 2: AXY2 + AX → 2 AXY
If the rate law for this reaction is Rate = k[AX]2[Y2],the intermediate is ________,and step ________ is the rate-determining step.

Accepted Answer

Question 17

Given the following hypothetical reaction: 2 E(g) + F(g) + G(g) → products.
If the rate law is: Rate = k[E]2[F]-1,what is the overall order of reaction?

Accepted Answer

A)  zero
B)  first
C)  second
D)  thirdE) A) and B)
F) B) and C)

Question 18

The following reaction is first order in A and first order in B:
A + B → Products Rate = k[A][B]
What is the rate constant k of this reaction in vessel (b) relative to the rate constant k of this reaction in vessel (a) ? Each vessel has the same volume.Shaded spheres represent A molecules,and unshaded spheres represent B molecules.

Accepted Answer

A)  rate constant k in vessel (b) /rate constant k in vessel (a) = 1:2
B)  rate constant k in vessel (b) /rate constant k in vessel (a) = 1:1
C)  rate constant k in vessel (b) /rate constant k in vessel (a) = 2:1
D)  rate constant k in vessel (b) /rate constant k in vessel (a) = 4:1E) A) and D)
F) B) and C)

Question 19

Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume.How will the rate of decomposition in vessel (a) be affected if the volume of the vessel is decreased by a factor of 2?

Accepted Answer

A)  decrease by 1/2
B)  increase by 2
C)  increase by 4
D)  stay the sameE) A) and C)
F) All of the above

Question 20

The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

Accepted Answer

A)  H2,homogeneous
B)  N2,homogeneous
C)  NH3,homogeneous
D)  metal surface,heterogeneousE) A) and B)
F) A) and C)

Exam 12: Chemical Kinetics

A common rule of thumb in organic chemistry is that increasing the temperature of a reaction at room temperature by 10°C doubles the rate.Calculate E_a for a reaction that follows this rule of thumb Assume room temperature is 25°C.

Correct Answer
verified

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Which equation best represents the reaction?

Correct Answer
verified

Consider a reaction that occurs by the following mechanism: A + BC → AC + B AC + D → A + CD The potential energy profile for this reaction is shown below. -Transition states occur at which reaction stages?

Correct Answer
verified

The rate constant,k,for a first-order reaction is equal to 4.2 × 10^-4 s^-1.What is the half-life for the reaction?

Correct Answer
verified

What is the minimum energy barrier that must be overcome for a chemical reaction to occur?

Correct Answer
verified

A gaseous reaction occurs by a two-step mechanism,shown below. Step 1: AX +Y₂ → AXY₂ Step 2: AXY₂ + AX → 2 AXY If the rate law for this reaction is Rate = k[AX]²[Y₂],the intermediate is ,and step is the rate-determining step.

Correct Answer
verified

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) If the rate of appearance of NO₂ is equal to 0.560 mol/min at a particular moment,what is the rate of appearance of O₂ at that moment?

Correct Answer
verified

Correct Answer
verified

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) If the rate of disappearance of N₂O₅ is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO₂ at that moment?

Correct Answer
verified

Correct Answer
verified

Given the following hypothetical reaction: 2 E(g) + F(g) + G(g) → products. If the rate law is: Rate = k[E]²[F]^-1,what is the overall order of reaction?

Correct Answer
verified

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?

Correct Answer
verified

The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Correct Answer
verified

If the units for rate are M s^-1,what are the units for the rate constant,k,if the overall order of the reaction is three?

Correct Answer
verified

Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume.How will the rate of decomposition in vessel (a) be affected if the volume of the vessel is decreased by a factor of 2?

Correct Answer
verified

The decay curve shown below approximates the decay of phosphorus-32.What is the approximate half-life of phosphorus-32?

Correct Answer
verified

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10^-5 M/s.Over the same time interval what is the rate of reaction with respect to B,Δ[B]/Δt?

Correct Answer
verified

The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

Correct Answer
verified

Decays by electron capture to give If unshaded spheres represent Atoms and shaded spheres represent Atoms,how many half-lives have passed in the following example?

Correct Answer
verified

Correct Answer
verified

Exam 12: Chemical Kinetics

A common rule of thumb in organic chemistry is that increasing the temperature of a reaction at room temperature by 10°C doubles the rate.Calculate Ea for a reaction that follows this rule of thumb Assume room temperature is 25°C.

Correct AnswerverifiedShow Answer

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Which equation best represents the reaction?

Correct AnswerverifiedShow Answer

Consider a reaction that occurs by the following mechanism: A + BC → AC + B AC + D → A + CD The potential energy profile for this reaction is shown below. -Transition states occur at which reaction stages?

Correct AnswerverifiedShow Answer

The rate constant,k,for a first-order reaction is equal to 4.2 × 10-4 s-1.What is the half-life for the reaction?

Correct AnswerverifiedShow Answer

What is the minimum energy barrier that must be overcome for a chemical reaction to occur?

Correct AnswerverifiedShow Answer

A gaseous reaction occurs by a two-step mechanism,shown below. Step 1: AX +Y2 → AXY2 Step 2: AXY2 + AX → 2 AXY If the rate law for this reaction is Rate = k[AX]2[Y2],the intermediate is ________,and step ________ is the rate-determining step.

Correct AnswerverifiedShow Answer

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g) If the rate of appearance of NO2 is equal to 0.560 mol/min at a particular moment,what is the rate of appearance of O2 at that moment?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g) → 4 NO2(g) + O2(g) If the rate of disappearance of N2O5 is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO2 at that moment?

Correct AnswerverifiedShow Answer

The aquation of tris(1,10-phenanthroline) iron(II) in acid solution takes place according to the equation: Fe(phen) 32+ + 3 H3O+ + 3 H2O → Fe(H2O) 62+ + 3 phenH+. If the activation energy,Ea,is 126 kJ/mol and the rate constant at 30°C is 9.8 × 10-3 min-1,what is the rate constant at 35°C?

Correct AnswerverifiedShow Answer

Given the following hypothetical reaction: 2 E(g) + F(g) + G(g) → products. If the rate law is: Rate = k[E]2[F]-1,what is the overall order of reaction?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H2O2(aq) → 2 H2O(l) + O2(g) Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Correct AnswerverifiedShow Answer

If the units for rate are M s-1,what are the units for the rate constant,k,if the overall order of the reaction is three?

Correct AnswerverifiedShow Answer

Consider the first-order decomposition of A molecules (shaded spheres) in two vessels of equal volume.How will the rate of decomposition in vessel (a) be affected if the volume of the vessel is decreased by a factor of 2?

Correct AnswerverifiedShow Answer

The decay curve shown below approximates the decay of phosphorus-32.What is the approximate half-life of phosphorus-32?

Correct AnswerverifiedShow Answer

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10-5 M/s.Over the same time interval what is the rate of reaction with respect to B,Δ[B]/Δt?

Correct AnswerverifiedShow Answer

The Haber process is the synthesis of ammonia gas from hydrogen and nitrogen on a hot metal surface.What is the catalyst and what type of catalysis is occurring?

Correct AnswerverifiedShow Answer

Decays by electron capture to give If unshaded spheres represent Atoms and shaded spheres represent Atoms,how many half-lives have passed in the following example?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A common rule of thumb in organic chemistry is that increasing the temperature of a reaction at room temperature by 10°C doubles the rate.Calculate E_a for a reaction that follows this rule of thumb Assume room temperature is 25°C.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The rate constant,k,for a first-order reaction is equal to 4.2 × 10^-4 s^-1.What is the half-life for the reaction?

Correct Answer
verified

Correct Answer
verified

A gaseous reaction occurs by a two-step mechanism,shown below. Step 1: AX +Y₂ → AXY₂ Step 2: AXY₂ + AX → 2 AXY If the rate law for this reaction is Rate = k[AX]²[Y₂],the intermediate is ,and step is the rate-determining step.

Correct Answer
verified

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) If the rate of appearance of NO₂ is equal to 0.560 mol/min at a particular moment,what is the rate of appearance of O₂ at that moment?

Correct Answer
verified

Correct Answer
verified

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g) → 4 NO₂(g) + O₂(g) If the rate of disappearance of N₂O₅ is equal to 1.40 mol/min at a particular moment,what is the rate of appearance of NO₂ at that moment?

Correct Answer
verified

Correct Answer
verified

Given the following hypothetical reaction: 2 E(g) + F(g) + G(g) → products. If the rate law is: Rate = k[E]²[F]^-1,what is the overall order of reaction?

Correct Answer
verified

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?

Correct Answer
verified

The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Correct Answer
verified

If the units for rate are M s^-1,what are the units for the rate constant,k,if the overall order of the reaction is three?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10^-5 M/s.Over the same time interval what is the rate of reaction with respect to B,Δ[B]/Δt?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified