Question 1

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. 
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 2

Determine the rate law and the value of k for the following reaction using the data provided: CO(g) + Cl2(g) → COCl2(g) [CO]i (M) [Cl2]i (M) Initial Rate (M1 s-1)
0)25 0.40 0.696
0)25 0.80 1.97
0)50 0.80 3.94

Accepted Answer

A)  Rate = 11 M-3/2 s-1 [CO][Cl2]3/2 
B)  Rate = 36 M-1.8 s-1 [CO][Cl2]2.8 
C)  Rate = 17 M-2 s-1 [CO][Cl2]2 
D)  Rate = 4.4 M-1/2 s-1 [CO][Cl2]1/2 
E)  Rate = 18 M-3/2 s-1 [CO]2[Cl2]1/2 
A)  Rate = 11 M-3/2 s-1 [CO][Cl2]3/2 
B)  Rate = 36 M-1.8 s-1 [CO][Cl2]2.8 
C)  Rate = 17 M-2 s-1 [CO][Cl2]2 
D)  Rate = 4.4 M-1/2 s-1 [CO][Cl2]1/2 
E)  Rate = 18 M-3/2 s-1 [CO]2[Cl2]1/2

Question 3

A particular first-order reaction has a rate constant of 1.35 ×     at 25.0 °C. What is the magnitude of k at 75.0 °C if

Accepted Answer

A)  1.61 × 104 s-1 
B)  646 s-1 
C)  1.11 × 10117 s-1 
D)  6.19 × 10-5 s-1 
E)  1.36 × 102 s-1 
A)  1.61 × 104 s-1 
B)  646 s-1 
C)  1.11 × 10117 s-1 
D)  6.19 × 10-5 s-1 
E)  1.36 × 102 s-1

Question 4

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 5

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 6

What data should be plotted to show that experimental concentration data fit a first-order reaction?

Accepted Answer

A)    vs. time 
B)  [reactant] vs. time 
C)  ln[reactant] vs. time 
D)  ln(k) vs.   
E)  ln(k) vs. Ea 
A)    vs. time 
B)  [reactant] vs. time 
C)  ln[reactant] vs. time 
D)  ln(k) vs.   
E)  ln(k) vs. Ea

Question 7

Determine the missing initial rate for a reaction with an order of   given the following information:

Accepted Answer

A)  6.0 × 10-3 mol L-1 s-1 
B)  2.8 × 10-2 mol L-1 s-1 
C)  7.3 × 10-3 mol L-1 s-1 
D)  9.74 × 10-3 mol L-1 s-1 
E)  1.0 × 10-2 mol L-1 s-1 
A)  6.0 × 10-3 mol L-1 s-1 
B)  2.8 × 10-2 mol L-1 s-1 
C)  7.3 × 10-3 mol L-1 s-1 
D)  9.74 × 10-3 mol L-1 s-1 
E)  1.0 × 10-2 mol L-1 s-1

Question 8

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 
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

Question 9

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   order 
E)  0th order 
A)  1st order 
B)  2nd order 
C)  3rd order 
D)  1   order 
E)  0th order

Question 10

If a reaction carried out at 61 °C has an activation energy, Ea, of 67.3 kJ mol-1, a rate constant of 791 s-1, and a frequency factor, A, of 2.65 × 1013, what is the value of R? k = A

Accepted Answer

A)  0.08314 J mol-1 K-1 
B)  2.62 J mol-1 K-1 
C)  0.08206 J mol-1 K-1 
D)  9.51 J mol-1 K-1 
E)  8.314 J mol-1 K-1 
A)  0.08314 J mol-1 K-1 
B)  2.62 J mol-1 K-1 
C)  0.08206 J mol-1 K-1 
D)  9.51 J mol-1 K-1 
E)  8.314 J mol-1 K-1

Question 11

For a reaction that follows the general rate law Rate = k[A]0[B][C]2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 4, the concentration of B is increased by a factor of 2, and the concentration of C is increased by a factor 6?

Accepted Answer

A)  The rate will decrease by a factor of 1/72.00. 
B)  The rate will decrease by a factor of 1/48. 
C)  The rate will increase by a factor of 72. 
D)  The rate will increase by a factor of 48. 
A)  The rate will decrease by a factor of 1/72.00. 
B)  The rate will decrease by a factor of 1/48. 
C)  The rate will increase by a factor of 72. 
D)  The rate will increase by a factor of 48.

Question 12

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

Accepted Answer

A)    N2 + O2 →      N2O 
B)  2N2O → 2N2 + O2 
C)  N2O → N2 + 2O2 
D)    N2O →   N2 + O2 
E)  2N2 + O2 → 2N2O 
A)    N2 + O2 →      N2O 
B)  2N2O → 2N2 + O2 
C)  N2O → N2 + 2O2 
D)    N2O →   N2 + O2 
E)  2N2 + O2 → 2N2O

Question 13

The decomposition of     in solution in carbon tetrachloride proceeds via the reaction 2     (soln) →   (soln) +   (soln)
The reaction is first order and has a rate constant of 4.82 ×     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 
A)  0.077 mol 
B)  0.053 mol 
C)  0.038 mol 
D)  15 mol 
E)  0.035 mol

Question 14

What function do enzymes serve?

Accepted Answer

They are biological catalysts. They lowe

Question 15

Define activation energy.

Accepted Answer

The activation energ

Question 16

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.

Accepted Answer

A)  160. kJ mol-1 
B)  240. kJ mol-1 
C)  417 kJ mol-1 
D)  127 kJ mol-1 
E)  338 kJ mol-1 
A)  160. kJ mol-1 
B)  240. kJ mol-1 
C)  417 kJ mol-1 
D)  127 kJ mol-1 
E)  338 kJ mol-1

Question 17

If the activation energy for a given compound is found to be 103 kJ mol-1 with a frequency factor of 4.0 × 1013 s-1, what is the rate constant for this reaction at 398 K?

Accepted Answer

A)  1.2 s-1 
B)  8.2 s-1 
C)  3.9 × 1010 s-1 
D)  1.7 × 1010 s-1 
E)  2.5 × 107 s-1 
A)  1.2 s-1 
B)  8.2 s-1 
C)  3.9 × 1010 s-1 
D)  1.7 × 1010 s-1 
E)  2.5 × 107 s-1

Question 18

What is the overall order of the following reaction, given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]1[Y]2

Accepted Answer

A)  3rd order 
B)  5th order 
C)  2nd order 
D)  1st order 
E)  0th order 
A)  3rd order 
B)  5th order 
C)  2nd order 
D)  1st order 
E)  0th order

Question 19

Which of the following is the characteristic of a second-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. 
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 20

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 
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

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]2[Y]3

Determine the rate law and the value of k for the following reaction using the data provided: CO(g) + Cl2(g) → COCl2(g) [CO]i (M) [Cl2]i (M) Initial Rate (M1 s-1) 0)25 0.40 0.696 0)25 0.80 1.97 0)50 0.80 3.94

A particular first-order reaction has a rate constant of 1.35 × at 25.0 °C. What is the magnitude of k at 75.0 °C if

Identify a homogeneous catalyst.

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?

What data should be plotted to show that experimental concentration data fit a first-order reaction?

Determine the missing initial rate for a reaction with an order of given the following information:

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?

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 a reaction carried out at 61 °C has an activation energy, Ea, of 67.3 kJ mol-1, a rate constant of 791 s-1, and a frequency factor, A, of 2.65 × 1013, what is the value of R? k = A

For a reaction that follows the general rate law Rate = k[A]0[B][C]2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 4, the concentration of B is increased by a factor of 2, and the concentration of C is increased by a factor 6?

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

The decomposition of in solution in carbon tetrachloride proceeds via the reaction 2 (soln) → (soln) + (soln) The reaction is first order and has a rate constant of 4.82 × 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?

What function do enzymes serve?

Define activation energy.

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.

If the activation energy for a given compound is found to be 103 kJ mol-1 with a frequency factor of 4.0 × 1013 s-1, what is the rate constant for this reaction at 398 K?

What is the overall order of the following reaction, given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]1[Y]2

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

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?

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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

Determine the rate law and the value of k for the following reaction using the data provided: CO(g) + Cl₂(g) → COCl₂(g) [CO]_i(M) [Cl₂]_i (M) Initial Rate (M¹s^-1) 0)25 0.40 0.696 0)25 0.80 1.97 0)50 0.80 3.94

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?

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?

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 a reaction carried out at 61 °C has an activation energy, E_a, of 67.3 kJ mol^-1, a rate constant of 791 s^-1, and a frequency factor, A, of 2.65 × 10¹³, what is the value of R? k = A

For a reaction that follows the general rate law Rate = k[A]⁰[B][C]², what will happen to the rate of reaction if the concentration of A is increased by a factor of 4, the concentration of B is increased by a factor of 2, and the concentration of C is increased by a factor 6?

The first-order rearrangement of CH₃NC is measured to have a rate constant of 3.61 × 10^-15 s^-1 at 298 K and a rate constant of 8.66 × 10^-7 s^-1 at 425 K. Determine the activation energy for this reaction.

If the activation energy for a given compound is found to be 103 kJ mol^-1 with a frequency factor of 4.0 × 10¹³ s^-1, what is the rate constant for this reaction at 398 K?

What is the overall order of the following reaction, given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]¹[Y]²

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?