Question 1

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 increase 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 increase 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 2

What is the overall order of the following reaction,given the rate law? 
NO(g)+ O3(g)→ NO2(g)+ O2(g)Rate = k[NO][O3]

Accepted Answer

A) 1st order 
B) 2nd order 
C) 3rd order 
D) 1 $\frac{1}{2}$ order 
E) 0th order 
A) 1st order 
B) 2nd order 
C) 3rd order 
D) 1 $\frac{1}{2}$ order 
E) 0th order

Question 3

If the activation energy for a given compound is found to be 42.0 kJ mol-1 with a frequency factor of 8.0 × 1010 s-1,what is the rate constant for this reaction at 298 K?

Accepted Answer

A) 2.9 × 10-4 s-1 
B) 7.4 × 10-4 s-1 
C) 1.4 × 109 s-1 
D) 4.6 × 10 5 s-1 
E) 3.5 × 103 s-1 
A) 2.9 × 10-4 s-1 
B) 7.4 × 10-4 s-1 
C) 1.4 × 109 s-1 
D) 4.6 × 10 5 s-1 
E) 3.5 × 103 s-1

Question 4

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g).
If the rate of appearance of O2 is equal to 3.00 mol min-1 at a particular moment,what is the rate of disappearance of N2O5 at that moment?

Accepted Answer

A) 0.750 mol min-1 
B) 1.50 mol min-1 
C) 6.00 mol min-1 
D) 12.0 mol min-1 
A) 0.750 mol min-1 
B) 1.50 mol min-1 
C) 6.00 mol min-1 
D) 12.0 mol min-1

Question 5

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Accepted Answer

A) 1 
B) 3 
C) 1.5 
D) 2.5 
E) 2 
A) 1 
B) 3 
C) 1.5 
D) 2.5 
E) 2

Question 6

Identify a homogeneous catalyst.

Accepted Answer

A) SO2 over vanadium (V)oxide 
B) Pd in H2 gas 
C) Pt with methane 
D) H2SO4 with concentrated HCl 
E) N2 and H2 catalyzed by Fe 
A) SO2 over vanadium (V)oxide 
B) Pd in H2 gas 
C) Pt with methane 
D) H2SO4 with concentrated HCl 
E) N2 and H2 catalyzed by Fe

Question 7

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

Accepted Answer

A) Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$ 
B) Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$ 
C) Rate = - $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$ 
D) Rate = + $\frac { 2 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$ 
E) It is not possible to determine the answer without more information. 
A) Rate = - $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$ 
B) Rate = + $\frac { 1 } { 2 }$ $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$ 
C) Rate = - $\frac { \Delta \left[ \mathrm { O } _ { 2 } \right] } { \mathrm { D } t }$ 
D) Rate = + $\frac { 2 \Delta \left[ \mathrm { O } _ { 2 } \right] } { \Delta t }$ 
E) It is not possible to determine the answer without more information.

Question 8

Carbon-14,which is present in all living tissue,radioactively decays via a first-order process.A one-gram sample of wood taken from a living tree gives a rate for carbon-14 decay of 13.6 counts per minute.If the half-life for carbon-14 is 5720 years,how old is a wood sample that gives a rate for carbon-14 decay of 11.9 counts per minute?

Accepted Answer

A) 5.3 × 102 yr 
B) 7.6 × 102 yr 
C) 1.1 × 103 yr 
D) 9.4 × 103 yr 
A) 5.3 × 102 yr 
B) 7.6 × 102 yr 
C) 1.1 × 103 yr 
D) 9.4 × 103 yr

Question 9

A reaction with an activation energy of 34.0 kJ mol-1 has a rate constant of 26.8 s-1 at 354 K.What is the rate constant at 314 K?

Accepted Answer

A) 6.15 s-1 
B) 2.08 s-1 
C) 7.68 s-1 
D) 9.80 s-1 
E) 4.00 s-1 
A) 6.15 s-1 
B) 2.08 s-1 
C) 7.68 s-1 
D) 9.80 s-1 
E) 4.00 s-1

Question 10

Calculate the activation energy,Ea,for a reaction with a frequency factor,A,of 8.12 × 109 s-1 and a rate constant of 3.05 × 104 s-1 at 375 K.

Accepted Answer

A) 72.5 kJ mol-1 
B) 38.9 kJ mol-1 
C) 104 kJ mol-1 
D) 68.0 kJ mol-1 
E) 71.6 kJ mol-1 
A) 72.5 kJ mol-1 
B) 38.9 kJ mol-1 
C) 104 kJ mol-1 
D) 68.0 kJ mol-1 
E) 71.6 kJ mol-1

Question 11

The second-order reaction 2Mn(CO)5 → Mn2(CO)10 has a rate constant equal to 3.0 × 109 L mol-1 s-1 at 25 °C.If the initial concentration of Mn(CO)5 is 2.0 × 10-5 mol L-1,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 12

A reaction with an activation energy of 65.4 kJ mol-1 has a rate constant of 1.15 s-1 at 354 K.At what temperature will the rate constant be double?

Accepted Answer

A) 365 K 
B) 708 K 
C) 181 K 
D) 340 K 
E) 378 K 
A) 365 K 
B) 708 K 
C) 181 K 
D) 340 K 
E) 378 K

Question 13

Given the following balanced equation,determine the rate of reaction with respect to [SO3].If the rate of SO2 loss is 1.19 × 10-3 mol L-1 s-1,what is the rate of formation of SO3? 
2SO2(g)+ O2(g)→ 2SO3(g)

Accepted Answer

A) 3.56 × 10-3 mol L-1 s-1 
B) 1.19 × 10-3 mol L-1 s-1 
C) 1.78 × 10-3 mol L-1 s-1 
D) 1.42 × 10-2 mol L-1 s-1 
E) 7.12 × 10-3 mol L-1 s-1 
A) 3.56 × 10-3 mol L-1 s-1 
B) 1.19 × 10-3 mol L-1 s-1 
C) 1.78 × 10-3 mol L-1 s-1 
D) 1.42 × 10-2 mol L-1 s-1 
E) 7.12 × 10-3 mol L-1 s-1

Question 14

What is the overall reaction order for the reaction that has the rate law Rate = k[O2][NO]2?

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 15

A reaction is found to have an activation energy of 108 kJ mol-1.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 16

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 s 
A) 2.9 × 10-4 s 
B) 1.2 × 103 s 
C) 1.7 × 103 s 
D) 2.4 × 103 s

Question 17

The combustion of ethylene proceeds by the reaction 
$\mathrm { C } _ { 2 }$ $\mathrm { H } _ { 4 }$ (g)+ $3 \mathrm { O } _ { 2 }$ (g)? $2 \mathrm { CO } _ { 2 }$ (g)+ $2 \mathrm { H } _ { 2 }$ O(g) 
When the rate of disappearance of $\mathrm { O } _ { 2 }$ is 0.37 mol L-1 $s ^ { - 1 }$ ,the rate of appearance of $\mathrm { CO } _ { 2 }$ is ________ $\mathrm { mol } \mathrm { L } ^ { - 1 } \mathrm {~s} ^ { - 1 }$

Accepted Answer

A) 0.12 
B) 1.1 
C) 0.56 
D) 0.74 
E) 0.25 
A) 0.12 
B) 1.1 
C) 0.56 
D) 0.74 
E) 0.25

Question 18

The half-life for the decay of radium is 1620 years.What is the rate constant for this first-order process?

Accepted Answer

A) 4.28 × 10-4 yr-1 
B) 1.12 × 10-4 yr-1 
C) 2.33 × 10-4 yr-1 
D) 8.91 × 10-4 yr-1 
E) 6.17 × 10-4 yr-1 
A) 4.28 × 10-4 yr-1 
B) 1.12 × 10-4 yr-1 
C) 2.33 × 10-4 yr-1 
D) 8.91 × 10-4 yr-1 
E) 6.17 × 10-4 yr-1

Question 19

The first-order reaction,2N2O(g)→ 2N2(g)+ O2(g),has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

Accepted Answer

A) 0.62 s 
B) 2.8 s 
C) 6.3 s 
D) 8.4 s 
A) 0.62 s 
B) 2.8 s 
C) 6.3 s 
D) 8.4 s

Question 20

The rate constant for a second-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 
A) 2.0 s 
B) 5.0 s 
C) 0.25 s 
D) 6.9 s 
E) 1.3 s

Exam 13: Chemical Kinetics

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

What is the overall order of the following reaction,given the rate law? NO(g)+ O3(g)→ NO2(g)+ O2(g)Rate = k[NO][O3]

If the activation energy for a given compound is found to be 42.0 kJ mol-1 with a frequency factor of 8.0 × 1010 s-1,what is the rate constant for this reaction at 298 K?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g). If the rate of appearance of O2 is equal to 3.00 mol min-1 at a particular moment,what is the rate of disappearance of N2O5 at that moment?

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Identify a homogeneous catalyst.

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

A reaction with an activation energy of 34.0 kJ mol-1 has a rate constant of 26.8 s-1 at 354 K.What is the rate constant at 314 K?

Calculate the activation energy,Ea,for a reaction with a frequency factor,A,of 8.12 × 109 s-1 and a rate constant of 3.05 × 104 s-1 at 375 K.

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

A reaction with an activation energy of 65.4 kJ mol-1 has a rate constant of 1.15 s-1 at 354 K.At what temperature will the rate constant be double?

Given the following balanced equation,determine the rate of reaction with respect to [SO3].If the rate of SO2 loss is 1.19 × 10-3 mol L-1 s-1,what is the rate of formation of SO3? 2SO2(g)+ O2(g)→ 2SO3(g)

What is the overall reaction order for the reaction that has the rate law Rate = k[O2][NO]2?

A reaction is found to have an activation energy of 108 kJ mol-1.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?

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?

The half-life for the decay of radium is 1620 years.What is the rate constant for this first-order process?

The first-order reaction,2N2O(g)→ 2N2(g)+ O2(g),has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

The rate constant for a second-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?

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Filters

What is the overall order of the following reaction,given the rate law? NO(g)+ O₃(g)→ NO₂(g)+ O₂(g)Rate = k[NO][O₃]

If the activation energy for a given compound is found to be 42.0 kJ mol^-1 with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g)→ 4NO₂(g)+ O₂(g). If the rate of appearance of O₂ is equal to 3.00 mol min^-1 at a particular moment,what is the rate of disappearance of N₂O₅ at that moment?

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

A reaction with an activation energy of 34.0 kJ mol^-1 has a rate constant of 26.8 s^-1 at 354 K.What is the rate constant at 314 K?

Calculate the activation energy,E_a,for a reaction with a frequency factor,A,of 8.12 × 10⁹ s^-1 and a rate constant of 3.05 × 10⁴ s^-1 at 375 K.

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

A reaction with an activation energy of 65.4 kJ mol^-1 has a rate constant of 1.15 s^-1 at 354 K.At what temperature will the rate constant be double?

Given the following balanced equation,determine the rate of reaction with respect to [SO₃].If the rate of SO₂ loss is 1.19 × 10^-3 mol L^-1 s^-¹,what is the rate of formation of SO₃? 2SO₂(g)+ O₂(g)→ 2SO₃(g)

What is the overall reaction order for the reaction that has the rate law Rate = k[O₂][NO]²?

A reaction is found to have an activation energy of 108 kJ mol^-1.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?

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?

The first-order reaction,2N₂O(g)→ 2N₂(g)+ O₂(g),has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

The rate constant for a second-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?