Question 1

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? The rate will

Accepted Answer

A)  decrease by a factor of 1/9.00. 
B)  decrease by a factor of 1/3.00. 
C)  increase by a factor of 3.00. 
D)  increase by a factor of 9.00.

Question 2

The first-order reaction,2 N2O(g)→ 2 N2(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

Question 3

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 s

Question 4

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]

Question 5

Identify an 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

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 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/min

Question 7

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

Accepted Answer

A)  7 
B)  10 
C)  3 
D)  4 
E)  5

Question 8

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 9

Write a balanced reaction for which the following rate relationships are TRUE. Rate = -   =   =

Accepted Answer

A)  2 N2O5 → 4 NO2 + O2 
B)  4 NO2 + O2 → 2 N2O5 
C)  2 N2O5 → NO2 + 4 O2 
D)   NO2 + O2 →     N2O5 
E)   N2O5 →     NO2 + O2

Question 10

What are the units of k in the following rate law?
Rate = k[X]0[Y]0

Accepted Answer

A)   
B)  Ms 
C)  M-1s-1 
D)   
E)

Question 11

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

Question 12

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

Accepted Answer

A)  Rate = +  
B)  Rate = -   
C)  Rate = +   
D)  Rate = -  
E)  It is not possible to determine without more information.

Question 13

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

Accepted Answer

A)  4.55 M 
B)  0.258 M 
C)  3.87 M 
D)  2.20 M 
E)  2.39 M

Question 14

What are the units of k in the following rate law?
Rate = k[X]

Accepted Answer

A)   
B)  Ms 
C)   
D)   
E)

Question 15

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

Accepted Answer

A)  decrease by a factor of 1/25.0. 
B)  decrease by a factor of 1/5.00. 
C)  increase by a factor of 5.00. 
D)  increase by a factor of 25.0.

Question 16

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

Accepted Answer

A)  Rate = +  
B)  Rate = -   
C)  Rate = +   
D)  Rate = -   
E)  It is not possible to determine without more information.

Question 17

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 =

Question 18

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism?
1st step: A + B → 2C + D slow
2nd step: C → E fast
3rd step: D → 2F fast

Accepted Answer

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

Question 19

What is the overall order of the following reaction,given the rate law?
X + 2 Y → 4 Z Rate = k[X][Y]

Accepted Answer

A)  3rd order 
B)  5th order 
C)  2nd order 
D)  1st order 
E)  6th order

Question 20

A graph of 1/[A] vs.t gives a straight line.What are the units of k for this system?

Accepted Answer

A)  M s-1 
B)  s-1 
C)  M-1 s-1 
D)  M-2 s-1 
E)  M-3 s-1

Exam 15: Chemical Kinetics

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? The rate will

The first-order reaction,2 N₂O(g) → 2 N₂(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 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?

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

Identify an homogeneous catalyst.

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?

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

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?

Write a balanced reaction for which the following rate relationships are TRUE. Rate = - = =

What are the units of k in the following rate law? Rate = k[X]⁰[Y]⁰

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

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

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 M^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

What are the units of k in the following rate law? Rate = k[X]

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

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

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

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism? 1^st step: A + B → 2C + D slow 2^nd step: C → E fast 3^rd step: D → 2F fast

What is the overall order of the following reaction,given the rate law? X + 2 Y → 4 Z Rate = k[X][Y]

A graph of 1/[A] vs.t gives a straight line.What are the units of k for this system?

Exam 15: Chemical Kinetics

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? The rate will

The first-order reaction,2 N2O(g) → 2 N2(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 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?

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

Identify an homogeneous catalyst.

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?

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

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?

Write a balanced reaction for which the following rate relationships are TRUE. Rate = - = =

What are the units of k in the following rate law? Rate = k[X]0[Y]0

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

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

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

What are the units of k in the following rate law? Rate = k[X]

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

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

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

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism? 1st step: A + B → 2C + D slow 2nd step: C → E fast 3rd step: D → 2F fast

What is the overall order of the following reaction,given the rate law? X + 2 Y → 4 Z Rate = k[X][Y]

A graph of 1/[A] vs.t gives a straight line.What are the units of k for this system?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? The rate will

The first-order reaction,2 N₂O(g) → 2 N₂(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 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?

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

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?

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?

What are the units of k in the following rate law? Rate = k[X]⁰[Y]⁰

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

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 M^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will

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

A reaction occurs via the following sequence of elementary steps.What is the rate law based on this reaction mechanism? 1^st step: A + B → 2C + D slow 2^nd step: C → E fast 3^rd step: D → 2F fast