Question 1

A reaction is found to have an activation energy of 38.0 kJ mol-1.If the rate constant for this reaction is 1.60 × 102 L mol-1 s-1 at 249 K,what is the rate constant at 436 K?

Accepted Answer

A)  2.38 × 105 L mol-1 s-1
B)  1.26 × 103 L mol-1 s-1
C)  7.94 × 104 L mol-1 s-1
D)  4.20 × 105 L mol-1 s-1
E)  3.80 × 104 L mol-1 s-1 D

Question 2

Given the following balanced equation,determine the rate of reaction with respect to [O3].If the rate of loss of O3 is 3.91 × 10-1 mol L-1 s-1,what is the rate of the formation of O2? 
2O3(g)→ 3O2(g)

Accepted Answer

A)  2.61 mol L-1 s-1
B)  0.937 mol L-1 s-1
C)  0.261 mol L-1 s-1
D)  0.587 mol L-1 s-1
E)  0.817 mol L-1 s-1 D

Question 3

What is the activation energy for a reaction that has a rate constant of 0.0883 L mol-1 s-1 at 333 K and 0.469 L mol-1 s-1 at 366 K?

Accepted Answer

A)  34.8 kJ mol-1
B)  28.0 kJ mol-1
C)  51.3 kJ mol-1
D)  39.1 kJ mol-1
E)  60.9 kJ mol-1 C

Question 4

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } 
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L }^{ - 1} \mathrm {~s} ^ { - 1 } \right) \
\hline 0.20 & 0.0050 \
0.40 & 0.020 \
0.80 & 0.080
\end{array}$$

Accepted Answer

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

Question 5

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl2 loss is 4.84 × 10-2 mol L-1 s-1,what is the rate of formation of NOCl? 
2NO(g)+ Cl2(g)→ 2NOCl(g)

Accepted Answer

A)  4.84 × 10-2 mol L-1 s-1
B)  2.42 × 10-2 mol L-1 s-1
C)  1.45 × 10-1 mol L-1 s-1
D)  9.68 × 10-2 mol L-1 s-1
E)  1.61 × 10-2 mol L-1 s-1

Question 6

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1.If the initial concentration of N2O is 10.9 mol L-1,what is the concentration of N2O after 9.6 s?

Accepted Answer

A)  7.4 × 10-3 mol L-1
B)  1.0 × 10-3 mol L-1
C)  1.4 × 10-3 mol L-1
D)  3.6 × 10-3 mol L-1
E)  8.7 × 10-3 mol L-1

Question 7

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? 
Rate = k [X]2[Y]3

Accepted Answer

A)  The rate of reaction will increase by a factor of 9.
B)  The rate of reaction will increase by a factor of 2.
C)  The rate of reaction will increase by a factor of 8.
D)  The rate of reaction will increase by a factor of 4.
E)  The rate of reaction will remain unchanged.

Question 8

Determine the missing initial rate for the following $\frac{1}{2}$ order reaction given the following information: $$\begin{array} { l | l } 
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L }^{ - 1 }\mathrm {~s} ^ { - 1 } \right) \
\hline 0.8456 & 0.0326 \
0.6843 & 0.0293 \
0.4321 & ?
\end{array}$$

Accepted Answer

A)  0.0352 mol L-1 s-1
B)  0.0301 mol L-1 s-1
C)  0.0215 mol L-1 s-1
D)  0.0233 mol L-1 s-1
E)  0.0280 mol L-1 s-1

Question 9

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } 
{ [ \mathrm { A } ] ( \mathrm { mol } \mathrm { L }^{ - 1 } )} & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \mathrm {~s} ^ { - 1 } \right) \
\hline 0.0143 & 3.00 \times 10 ^ { - 3 } \
0.0429 & 9.00 \times 10 ^ { - 3 } \
0.0715 & 1.5 \times 10 ^ { - 2 }
\end{array}$$

Accepted Answer

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

Question 10

Which of the following statements is FALSE?

Accepted Answer

A)  The average rate of a reaction decreases during a reaction.
B)  It is not possible to determine the rate of a reaction from its balanced equation.
C)  The rate of zero-order reactions is not dependent on concentration.
D)  The half-life of a first-order reaction is dependent on the initial concentration of reactant.
E)  None of the above statements is false.

Question 11

Calculate the frequency factor,A,for a reaction with a rate constant of 6.3 × 103 s-1 and an activation energy,Ea,of 74 kJ mol-1 at 315 K.

Accepted Answer

A)  1.2 × 1016 s-1
B)  3.8 × 1016 s-1
C)  4.0 × 1016 s-1
D)  6.1 × 1016 s-1
E)  8.9 × 1016 s-1

Question 12

The isomerization of methylisonitrile to acetonitrile 
$\mathrm { CH } _ { 3 }$ NC(g)? $\mathrm { CH } _ { 3 }$ CN(g) 
is first order in $\mathrm { CH } _ { 3 }$ NC.The rate constant for the reaction is 5.26 × 10-3 $s ^ { - 1 }$ at 531 K.The $\text { half-life }$ of the reaction when the initial [ $\mathrm { CH } _ { 3 }$ NC] is 0.030 mol L-1 is ________ s.

Accepted Answer

A)  4.38 × 102
B)  2.85
C)  6.34 × 103
D)  7.59 × 10-3
E)  1.32 × 102

Question 13

The rate of disappearance of HBr in the gas phase reaction 
2HBr(g)? $\mathrm { H } _ { 2 }$ (g)+ $\mathrm { Br } _ { 2 }$ (g)
Is 0.190 mol L-1 $s ^ { - 1 }$ at 150 °C.The rate of reaction is ________ mol L-1 $s ^ { - 1 }$ .

Accepted Answer

A)  2.63
B)  0.0361
C)  0.436
D)  0.380
E)  0.0950

Question 14

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s-1)for the reaction?

Accepted Answer

A)  2.0 × 10-4 s-1
B)  9.6 × 10-4 s-1
C)  1.2 × 10-2 s-1
D)  5.8 × 10-2 s-1

Question 15

A reaction is found to have a rate constant of 3.36 × 104 L mol-1 s-1 at 344 K and a rate constant of 7.69 L mol-1 s-1 at 219 K.Determine the activation energy for this reaction.

Accepted Answer

A)  23.8 kJ mol-1
B)  42.0 kJ mol-1
C)  11.5 kJ mol-1
D)  12.5 kJ mol-1
E)  58.2 kJ mol-1

Question 16

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of NO loss is 1.68 × 10-2 mol L-1 s-1,what is the rate of formation of NOCl? 
2NO(g)+ Cl2(g)→ 2NOCl(g)

Accepted Answer

A)  1.68 × 10-2 mol L-1 s-1
B)  3.81 × 10-2 mol L-1 s-1
C)  5.05 × 10-2 mol L-1 s-1
D)  6.14 × 10-2 mol L-1 s-1
E)  1.45 × 10-2 mol L-1 s-1

Question 17

The aquation of tris (1,10-phenanthroline)iron(II)in acid solution takes place according to the equation: 
Fe(phen)32+ + 3H3O+ + 3H2O → Fe(H2O)62+ + 3phenH+.
If the activation energy,Ea,is 126 kJ mol-1 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-1

Question 18

Which of the following represents the equation for a first-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 19

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

The reaction that occurs in a Breathalyzer,a device used to determine the alcohol level in a person's bloodstream,is given below.If the rate of appearance of Cr2(SO4)3 is 1.64 mol min-1 at a particular moment,what is the rate of disappearance of C2H6O at that moment? 
2K2Cr2O7 + 8H2SO4 + 3C2H6O → 2Cr2(SO4)3 + 2K2SO4 + 11H2O

Accepted Answer

A)  0.547 mol min-1
B)  1.09 mol min-1
C)  2.46 mol min-1
D)  4.92 mol min-1

Exam 13: Chemical Kinetics

A reaction is found to have an activation energy of 38.0 kJ mol^-1.If the rate constant for this reaction is 1.60 × 10² L mol^-1s^-1 at 249 K,what is the rate constant at 436 K?

Given the following balanced equation,determine the rate of reaction with respect to [O₃].If the rate of loss of O₃ is 3.91 × 10^-1 mol L^-1 s^-1,what is the rate of the formation of O₂? 2O₃(g) → 3O₂(g)

What is the activation energy for a reaction that has a rate constant of 0.0883 L mol^-1 s^-1at 333 K and 0.469 L mol^-1 s^-1 at 366 K?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl₂ loss is 4.84 × 10^-2 mol L^-1 s^-1,what is the rate of formation of NOCl? 2NO(g) + Cl₂(g) → 2NOCl(g)

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1.If the initial concentration of N₂O is 10.9 mol L^-1,what is the concentration of N₂O after 9.6 s?

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X]²[Y]³

Which of the following statements is FALSE?

Calculate the frequency factor,A,for a reaction with a rate constant of 6.3 × 10³ s^-1 and an activation energy,E_a,of 74 kJ mol^-1 at 315 K.

The rate of disappearance of HBr in the gas phase reaction 2HBr(g) ? $\mathrm { H } _ { 2 }$ (g) + $\mathrm { Br } _ { 2 }$ (g) Is 0.190 mol L^-1 $s ^ { - 1 }$ at 150 °C.The rate of reaction is ________ mol L^-1 $s ^ { - 1 }$ .

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s^-1) for the reaction?

A reaction is found to have a rate constant of 3.36 × 10⁴ L mol^-1s^-1 at 344 K and a rate constant of 7.69 L mol^-1s^-1 at 219 K.Determine the activation energy for this reaction.

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of NO loss is 1.68 × 10^-2 mol L^-1 s^-1,what is the rate of formation of NOCl? 2NO(g) + Cl₂(g) → 2NOCl(g)

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

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

Exam 13: Chemical Kinetics

A reaction is found to have an activation energy of 38.0 kJ mol-1.If the rate constant for this reaction is 1.60 × 102 L mol-1 s-1 at 249 K,what is the rate constant at 436 K?

Given the following balanced equation,determine the rate of reaction with respect to [O3].If the rate of loss of O3 is 3.91 × 10-1 mol L-1 s-1,what is the rate of the formation of O2? 2O3(g) → 3O2(g)

What is the activation energy for a reaction that has a rate constant of 0.0883 L mol-1 s-1 at 333 K and 0.469 L mol-1 s-1 at 366 K?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl2 loss is 4.84 × 10-2 mol L-1 s-1,what is the rate of formation of NOCl? 2NO(g) + Cl2(g) → 2NOCl(g)

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1.If the initial concentration of N2O is 10.9 mol L-1,what is the concentration of N2O after 9.6 s?

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X]2[Y]3

Which of the following statements is FALSE?

Calculate the frequency factor,A,for a reaction with a rate constant of 6.3 × 103 s-1 and an activation energy,Ea,of 74 kJ mol-1 at 315 K.

The rate of disappearance of HBr in the gas phase reaction 2HBr(g) ? H2\mathrm { H } _ { 2 }H2​ (g) + Br2\mathrm { Br } _ { 2 }Br2​ (g) Is 0.190 mol L-1 s−1s ^ { - 1 }s−1 at 150 °C.The rate of reaction is ________ mol L-1 s−1s ^ { - 1 }s−1 .

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s-1) for the reaction?

A reaction is found to have a rate constant of 3.36 × 104 L mol-1 s-1 at 344 K and a rate constant of 7.69 L mol-1 s-1 at 219 K.Determine the activation energy for this reaction.

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of NO loss is 1.68 × 10-2 mol L-1 s-1,what is the rate of formation of NOCl? 2NO(g) + Cl2(g) → 2NOCl(g)

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

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

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

A reaction is found to have an activation energy of 38.0 kJ mol^-1.If the rate constant for this reaction is 1.60 × 10² L mol^-1s^-1 at 249 K,what is the rate constant at 436 K?

Given the following balanced equation,determine the rate of reaction with respect to [O₃].If the rate of loss of O₃ is 3.91 × 10^-1 mol L^-1 s^-1,what is the rate of the formation of O₂? 2O₃(g) → 3O₂(g)

What is the activation energy for a reaction that has a rate constant of 0.0883 L mol^-1 s^-1at 333 K and 0.469 L mol^-1 s^-1 at 366 K?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl₂ loss is 4.84 × 10^-2 mol L^-1 s^-1,what is the rate of formation of NOCl? 2NO(g) + Cl₂(g) → 2NOCl(g)

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1.If the initial concentration of N₂O is 10.9 mol L^-1,what is the concentration of N₂O after 9.6 s?

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X]²[Y]³

Calculate the frequency factor,A,for a reaction with a rate constant of 6.3 × 10³ s^-1 and an activation energy,E_a,of 74 kJ mol^-1 at 315 K.

The rate of disappearance of HBr in the gas phase reaction 2HBr(g) ? $\mathrm { H } _ { 2 }$ (g) + $\mathrm { Br } _ { 2 }$ (g) Is 0.190 mol L^-1 $s ^ { - 1 }$ at 150 °C.The rate of reaction is ________ mol L^-1 $s ^ { - 1 }$ .

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s^-1) for the reaction?

A reaction is found to have a rate constant of 3.36 × 10⁴ L mol^-1s^-1 at 344 K and a rate constant of 7.69 L mol^-1s^-1 at 219 K.Determine the activation energy for this reaction.

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of NO loss is 1.68 × 10^-2 mol L^-1 s^-1,what is the rate of formation of NOCl? 2NO(g) + Cl₂(g) → 2NOCl(g)