Question 1

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s-1 and an activation energy,Ea,of 68.4 kJ mol-1 at 305 K.

Accepted Answer

A)  4.1 × 103 s-1
B)  8.1 × 103 s-1
C)  8.1 × 1015 s-1
D)  4.1 × 1015 s-1
E)  1.0 × 104 s-1

Question 2

What is the activation energy for a reaction that has a rate constant of 1.087 L mol-1 s-1 at 273 and 12.99 L mol-1 s-1 at 373 K?

Accepted Answer

A)  48.6 kJ mol-1
B)  18.4 kJ mol-1
C)  37.9 kJ mol-1
D)  12.7 kJ mol-1
E)  21.0 kJ mol-1

Question 3

Derive an expression for a "1/4-life" for a first-order reaction.

Accepted Answer

A)    ln⁡[A]t[ A]0−k\frac { \ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } } { - k }−kln[ A]0​[A]t​​​ 
B)    0.347k\frac { 0.347 } { k }k0.347​ 
C)    ln⁡[A]t[ A]0−4k\frac { \ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } } { - 4 k }−4kln[ A]0​[A]t​​​ 
D)    4k\frac { 4 } { k }k4​ 
E)    1.386k\frac { 1.386 } { k }k1.386​

Question 4

The decomposition of  N2\mathrm { N } _ { 2 }N2​   O5\mathrm { O } _ { 5 }O5​  in solution in carbon tetrachloride proceeds via the reaction 
2N2O5 (soln) ?  4NO24 \mathrm { NO } _ { 2 }4NO2​  (soln) +  O2\mathrm { O } _ { 2 }O2​  (soln) 
The reaction is first order and has a rate constant of 4.82 ×  10−310 ^ { - 3 }10−3   s−1s ^ { - 1 }s−1  at 64 °C.If the reaction is initiated with 0.073 mol in a 1.00 L vessel,how many moles remain after 151 s?

Accepted Answer

A)  0.077 mol
B)  0.053 mol
C)  0.038 mol
D)  15 mol
E)  0.035 mol

Question 5

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g) → 4NO2(g) + O2(g) .
If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment,what is the rate of appearance of NO2 at that moment?

Accepted Answer

A)  0.800 mol min-1
B)  1.60 mol min-1
C)  3.20 mol min-1
D)  6.40 mol min-1

Question 6

Calculate the temperature if a reaction has a rate constant,k,of 1234 s-1,a frequency factor,A,of 1.34 × 1014 s-1,and an activation energy,Ea,of 79.6 kJ mol-1.

Accepted Answer

A)  298 K
B)  341 K
C)  377 K
D)  418 K
E)  447 K

Question 7

For a reaction,what generally happens if the temperature is increased?

Accepted Answer

A)  a decrease in k occurs,which results in a faster rate
B)  a decrease in k occurs,which results in a slower rate
C)  an increase in k occurs,which results in a faster rate
D)  an increase in k occurs,which results in a slower rate
E)  there is no change to either k or the rate

Question 8

Given the following balanced equation,determine the rate of reaction with respect to [O2]. 2O3(g) ? 3O2(g)

Accepted Answer

A)  Rate = -  2Δ[O2]Δt\frac { 2 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }Δt2Δ[O2​]​ 
B)  Rate = -  23\frac { 2 } { 3 }32​   Δ[O2]Δt\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }ΔtΔ[O2​]​ 
C)  Rate = +  13\frac { 1 } { 3 }31​   Δ[O2]Dt\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }DtΔ[O2​]​ 
D)  Rate = +  3Δ[O2]Δt\frac { 3 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }Δt3Δ[O2​]​ 
E)  It is not possible to determine the answer without more information.

Question 9

Given the following balanced equation,determine the rate of reaction with respect to [NH3]. N2(g) + 3H2(g) ? 2NH3(g)

Accepted Answer

A)  Rate = +  2Δ[NH3]Δt\frac { 2 \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }Δt2Δ[NH3​]​ 
B)  Rate = -  2Δ[NH3]Δt\frac { 2 \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }Δt2Δ[NH3​]​ 
C)  Rate = +  12\frac { 1 } { 2 }21​   Δ[NH3]Δt\frac { \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }ΔtΔ[NH3​]​ 
D)  Rate = -  12\frac { 1 } { 2 }21​   Δ[NH3]Δt\frac { \Delta \left[ \mathrm { NH } _ { 3 } \right] } { \Delta t }ΔtΔ[NH3​]​ 
E)  It is not possible to determine the answer without more information.

Question 10

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

Accepted Answer

A)    ln⁡[A]t[ A]0=−kt\ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } = - k tln[ A]0​[A]t​​=−kt 
B)   1[ A]t−1[ A]0=kt\frac { 1 } { [ \mathrm {~A} ] _ { t } } - \frac { 1 } { [ \mathrm {~A} ] _ { 0 } } = k t[ A]t​1​−[ A]0​1​=kt 
C)  [A]t - [A]0 = -kt
D)  k = Ae(-Ea/RT) 
E)    ln⁡k2k1=EaR(1T) +ln⁡A\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right)  + \ln \mathrm { A }lnk1​k2​​=REa​​(T1​) +lnA

Question 11

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

Accepted Answer

A)   t1/2=1k[ A]0t 1 / 2 = \frac { 1 } { k [ \mathrm {~A} ] _ { 0 } }t1/2=k[ A]0​1​ 
B)   t1/2=0.693kt 1 / 2 = \frac { 0.693 } { k }t1/2=k0.693​ 
C)   t1/2=[A]02kt 1 / 2 = \frac { [ \mathrm { A } ] _ { 0 } } { 2 k }t1/2=2k[A]0​​ 
D)   t1/2=2k[ A]0t 1 / 2 = \frac { 2 k } { [ \mathrm {~A} ] _ { 0 } }t1/2=[ A]0​2k​ 
E)   t1/2=k[ A]0t 1 / 2 = \frac { k } { [ \mathrm {~A} ] _ { 0 } }t1/2=[ A]0​k​

Question 12

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration:  [A](molL−1)  Initial Rate (molL−1 s−1) 0.200.2500.400.5000.600.750\begin{array} { l | l } { [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } ight)  } & 	ext { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } ight)  \\hline 0.20 & 0.250 \0.40 & 0.500 \0.60 & 0.750\end{array}[A](molL−1) 0.200.400.60​ Initial Rate (molL−1 s−1) 0.2500.5000.750​​

Accepted Answer

A)  zero order
B)  first order
C)  second order
D)  third order
E)  impossible to determine

Question 13

Which of the following is 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.

Question 14

A reaction with an activation energy of 61.0 kJ mol-1 has a rate constant of 0.0345 L mol-1 s-1 at 301 K.What is the rate constant at 401 K?

Accepted Answer

A)  1.92 L mol-1 s-1
B)  7.90 × 10-5 L mol-1 s-1
C)  0.0445 L mol-1 s-1
D)  0.345 L mol-1 s-1
E)  15.1 L mol-1 s-1

Question 15

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

Accepted Answer

A)    ln⁡[A]t[ A]0=−kt\ln \frac { [ \mathrm { A } ] _ { t } } { [ \mathrm {~A} ] _ { 0 } } = - k tln[ A]0​[A]t​​=−kt 
B)   1[ A]t−1[ A]0=kt\frac { 1 } { [ \mathrm {~A} ] _ { t } } - \frac { 1 } { [ \mathrm {~A} ] _ { 0 } } = k t[ A]t​1​−[ A]0​1​=kt 
C)  [A]t - [A]0 = -kt
D)  k = Ae(-Ea/RT) 
E)   ln⁡k2k1=EaR(1T) +∣ln⁡A\ln \frac { k _ { 2 } } { k _ { 1 } } = \frac { E _ { \mathrm { a } } } { R } \left( \frac { 1 } { T } \right)  + \mid \ln \mathrm { A }lnk1​k2​​=REa​​(T1​) +∣lnA

Question 16

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1.If the initial concentration of N2O5 is 2.88 mol L-1,what is the concentration of N2O5 after 12.5 minutes?

Accepted Answer

A)  0.124 mol L-1
B)  0.805 mol L-1
C)  2.82 mol L-1
D)  0.355 mol L-1
E)  0.174 mol L-1

Question 17

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

Question 18

The rate constant for a zero-order reaction is 0.54 L mol-1 s-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?

Accepted Answer

A)  2.0 s
B)  5.0 s
C)  0.25 s
D)  6.9 s
E)  1.3 s

Question 19

What is the unit of k in a zero-order reaction?

Accepted Answer

A)  mol L-1 s-1
B)  mol L-1 s
C)  L mol-1 s-1
D)  M2 s-1
E)  s-1

Question 20

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 5.30 × 10 -6 L mol-1 s-1 at 298 K.At what temperature will the rate constant be 0.530 L mol-1 s-1?

Accepted Answer

A)  461 K
B)  410 K
C)  310 K
D)  495 K
E)  328 K

Exam 13: Chemical Kinetics

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2O₃(g) ? 3O₂(g)

Correct Answer
verified

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

Correct Answer
verified

A reaction with an activation energy of 61.0 kJ mol^-1 has a rate constant of 0.0345 L mol^-1 s^-1 at 301 K.What is the rate constant at 401 K?

Correct Answer
verified

Calculate the temperature if a reaction has a rate constant,k,of 1234 s^-1,a frequency factor,A,of 1.34 × 10¹⁴ s^-1,and an activation energy,E_a,of 79.6 kJ mol^-1.

Correct Answer
verified

Correct Answer
verified

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g) → 4NO₂(g) + O₂(g) . If the rate of disappearance of N₂O₅ is equal to 1.60 mol min^-1 at a particular moment,what is the rate of appearance of NO₂ at that moment?

Correct Answer
verified

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 2.88 mol L^-1,what is the concentration of N₂O₅ after 12.5 minutes?

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [NH₃]. N₂(g) + 3H₂(g) ? 2NH₃(g)

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

Derive an expression for a "1/4-life" for a first-order reaction.

Correct Answer
verified

What is the activation energy for a reaction that has a rate constant of 1.087 L mol^-1 s^-1at 273 and 12.99 L mol^-1 s^-1 at 373 K?

Correct Answer
verified

Correct Answer
verified

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s^-1 and an activation energy,E_a,of 68.4 kJ mol^-1 at 305 K.

Correct Answer
verified

Which of the following is the characteristic of a zero-order reaction having only one reactant?

Correct Answer
verified

The rate constant for a zero-order reaction is 0.54 L mol^-1s^-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?

Correct Answer
verified

What is the unit of k in a zero-order reaction?

Correct Answer
verified

A reaction with an activation energy of 71.6 kJ mol^-1 has a rate constant of 5.30 × 10 ^-6 L mol^-¹ s^-1 at 298 K.At what temperature will the rate constant be 0.530 L mol^-1 s^-1?

Correct Answer
verified

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

Correct Answer
verified

For a reaction,what generally happens if the temperature is increased?

Correct Answer
verified

Exam 13: Chemical Kinetics

Given the following balanced equation,determine the rate of reaction with respect to [O2]. 2O3(g) ? 3O2(g)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A reaction with an activation energy of 61.0 kJ mol-1 has a rate constant of 0.0345 L mol-1 s-1 at 301 K.What is the rate constant at 401 K?

Correct AnswerverifiedShow Answer

Calculate the temperature if a reaction has a rate constant,k,of 1234 s-1,a frequency factor,A,of 1.34 × 1014 s-1,and an activation energy,Ea,of 79.6 kJ mol-1.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g) → 4NO2(g) + O2(g) . If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment,what is the rate of appearance of NO2 at that moment?

Correct AnswerverifiedShow Answer

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1.If the initial concentration of N2O5 is 2.88 mol L-1,what is the concentration of N2O5 after 12.5 minutes?

Correct AnswerverifiedShow Answer

Given the following balanced equation,determine the rate of reaction with respect to [NH3]. N2(g) + 3H2(g) ? 2NH3(g)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Derive an expression for a "1/4-life" for a first-order reaction.

Correct AnswerverifiedShow Answer

What is the activation energy for a reaction that has a rate constant of 1.087 L mol-1 s-1 at 273 and 12.99 L mol-1 s-1 at 373 K?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s-1 and an activation energy,Ea,of 68.4 kJ mol-1 at 305 K.

Correct AnswerverifiedShow Answer

Which of the following is the characteristic of a zero-order reaction having only one reactant?

Correct AnswerverifiedShow Answer

The rate constant for a zero-order reaction is 0.54 L mol-1 s-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?

Correct AnswerverifiedShow Answer

What is the unit of k in a zero-order reaction?

Correct AnswerverifiedShow Answer

A reaction with an activation energy of 71.6 kJ mol-1 has a rate constant of 5.30 × 10 -6 L mol-1 s-1 at 298 K.At what temperature will the rate constant be 0.530 L mol-1 s-1?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

For a reaction,what generally happens if the temperature is increased?

Correct AnswerverifiedShow Answer

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2O₃(g) ? 3O₂(g)

Correct Answer
verified

Correct Answer
verified

A reaction with an activation energy of 61.0 kJ mol^-1 has a rate constant of 0.0345 L mol^-1 s^-1 at 301 K.What is the rate constant at 401 K?

Correct Answer
verified

Calculate the temperature if a reaction has a rate constant,k,of 1234 s^-1,a frequency factor,A,of 1.34 × 10¹⁴ s^-1,and an activation energy,E_a,of 79.6 kJ mol^-1.

Correct Answer
verified

Correct Answer
verified

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g) → 4NO₂(g) + O₂(g) . If the rate of disappearance of N₂O₅ is equal to 1.60 mol min^-1 at a particular moment,what is the rate of appearance of NO₂ at that moment?

Correct Answer
verified

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 2.88 mol L^-1,what is the concentration of N₂O₅ after 12.5 minutes?

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [NH₃]. N₂(g) + 3H₂(g) ? 2NH₃(g)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the activation energy for a reaction that has a rate constant of 1.087 L mol^-1 s^-1at 273 and 12.99 L mol^-1 s^-1 at 373 K?

Correct Answer
verified

Correct Answer
verified

Calculate the frequency factor,A,for a reaction with a rate constant of 7834 s^-1 and an activation energy,E_a,of 68.4 kJ mol^-1 at 305 K.

Correct Answer
verified

Correct Answer
verified

The rate constant for a zero-order reaction is 0.54 L mol^-1s^-1.What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?

Correct Answer
verified

Correct Answer
verified

A reaction with an activation energy of 71.6 kJ mol^-1 has a rate constant of 5.30 × 10 ^-6 L mol^-¹ s^-1 at 298 K.At what temperature will the rate constant be 0.530 L mol^-1 s^-1?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified