Question 1

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

Accepted Answer

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

Question 2

Calculate the temperature if a reaction has a rate constant, k, of 21.3 s-1, a frequency factor, A, of 7.98 × 1013 s-1, and an activation energy, Ea, of 102 kJ mol-1.

Accepted Answer

A) 316 K 
B) 273 K 
C) 381 K 
D) 298 K 
E) 424 K 
A) 316 K 
B) 273 K 
C) 381 K 
D) 298 K 
E) 424 K

Question 3

Which rate law is termolecular?

Accepted Answer

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

Question 4

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

Question 5

The following reaction is first order, C2H6 → 2CH3. If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

Accepted Answer

A) 4.5 min 
B) 17 min 
C) 53 min 
D) 65 min 
A) 4.5 min 
B) 17 min 
C) 53 min 
D) 65 min

Question 6

The isomerization reaction, CH3NC → CH3CN, is first order and the rate constant is equal to 0.46 s-1 at 600 K. What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 mol L-1?

Accepted Answer

A) 1.2 × 10-3 mol L-1 
B) 2.7 × 10-3 mol L-1 
C) 1.2 × 10-1 mol L-1 
D) 2.7 × 10-1 mol L-1 
A) 1.2 × 10-3 mol L-1 
B) 2.7 × 10-3 mol L-1 
C) 1.2 × 10-1 mol L-1 
D) 2.7 × 10-1 mol L-1

Question 7

The isomerization of methylisonitrile to acetonitrile CH3NC(g)→ CH3CN(g)
Is first order in CH3NC. The half-life of the reaction is 5.20 × 101 s at 545 K. The rate constant when the initial [CH3NC] is 0.030 mol L-1 is ________ s-1.

Accepted Answer

A) 75.1 
B) 0.641 
C) 0.0133 
D) 1.56 
E) 2.84 × 104 
A) 75.1 
B) 0.641 
C) 0.0133 
D) 1.56 
E) 2.84 × 104

Question 8

Calculate the frequency factor, A, for a reaction with a rate constant of 162.3 s-1 and an activation energy, Ea, of 68 kJ mol-1 at 298 K.

Accepted Answer

A) 2.1 × 102 s-1 
B) 2.5 × 103 s-1 
C)  2.6 × 10121 s-1 
D) 1.3 × 1014 s-1 
E) 3.8 × 1011 s-1 
A) 2.1 × 102 s-1 
B) 2.5 × 103 s-1 
C)  2.6 × 10121 s-1 
D) 1.3 × 1014 s-1 
E) 3.8 × 1011 s-1

Question 9

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 
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 10

What happens to the concentration of reactants and products during a chemical reaction?

Accepted Answer

The concentration of reactants

Question 11

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

Accepted Answer

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

Question 12

Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2 is 6.94 × 10-1 mol L-1 s-1, what is the rate of the loss of O3? 2O3(g)→ 3O2(g)

Accepted Answer

A) 0.463 mol L-1 s-1 
B) 1.04 mol L-1 s-1 
C) 2.08 mol L-1 s-1 
D) 0.231 mol L-1 s-1 
E) 4.16 mol L-1 s-1 
A) 0.463 mol L-1 s-1 
B) 1.04 mol L-1 s-1 
C) 2.08 mol L-1 s-1 
D) 0.231 mol L-1 s-1 
E) 4.16 mol L-1 s-1

Question 13

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g).
If the rate of appearance of NO2 is equal to 0.560 mol min-1 at a particular moment, what is the rate of appearance of O2 at that moment?

Accepted Answer

A) 0.140 mol min-1 
B) 0.280 mol min-1 
C) 1.12 mol min-1 
D) 2.24 mol min-1 
A) 0.140 mol min-1 
B) 0.280 mol min-1 
C) 1.12 mol min-1 
D) 2.24 mol min-1

Question 14

Which of the following is the characteristic of a first-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 15

Calculate the temperature if a reaction has a rate constant, k, of 841 s-1, a frequency factor, A, of 6.0 × 1012 s-1, and an activation energy, Ea, of 62 kJ mol-1.

Accepted Answer

A) 320 K 
B) 340 K 
C) 280 K 
D) 330 K 
E) 380 K 
A) 320 K 
B) 340 K 
C) 280 K 
D) 330 K 
E) 380 K

Question 16

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

Accepted Answer

A) 4.55 mol L-1 
B) 0.258 mol L-1 
C) 3.87 mol L-1 
D) 2.20 mol L-1 
E) 2.39 mol L-1 
A) 4.55 mol L-1 
B) 0.258 mol L-1 
C) 3.87 mol L-1 
D) 2.20 mol L-1 
E) 2.39 mol L-1

Question 17

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if Ea = 85.6 kJ mol-1?

Accepted Answer

A) 3.47 × 104 s-1 
B) 1.92 × 104 s-1 
C) 670 s-1 
D) 3.85 × 106 s-1 
E) 1.36 × 102 s-1 
A) 3.47 × 104 s-1 
B) 1.92 × 104 s-1 
C) 670 s-1 
D) 3.85 × 106 s-1 
E) 1.36 × 102 s-1

Question 18

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 
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 19

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→ 2CO2(g)+ 2H2O(g)
When the rate of disappearance of O2 is 0.28 mol L-1 s-1, the rate of appearance of CO2 is ________
Mol L-1 s-1.

Accepted Answer

A) 0.19 
B) 0.093 
C) 0.84 
D) 0.42 
E) 0.56 
A) 0.19 
B) 0.093 
C) 0.84 
D) 0.42 
E) 0.56

Question 20

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

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Exam 13: Chemical Kinetics

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

Calculate the temperature if a reaction has a rate constant, k, of 21.3 s-1, a frequency factor, A, of 7.98 × 1013 s-1, and an activation energy, Ea, of 102 kJ mol-1.

Which rate law is termolecular?

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?

The following reaction is first order, C2H6 → 2CH3. If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

The isomerization reaction, CH3NC → CH3CN, is first order and the rate constant is equal to 0.46 s-1 at 600 K. What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.30 mol L-1?

The isomerization of methylisonitrile to acetonitrile CH3NC(g)→ CH3CN(g) Is first order in CH3NC. The half-life of the reaction is 5.20 × 101 s at 545 K. The rate constant when the initial [CH3NC] is 0.030 mol L-1 is ________ s-1.

Calculate the frequency factor, A, for a reaction with a rate constant of 162.3 s-1 and an activation energy, Ea, of 68 kJ mol-1 at 298 K.

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

What happens to the concentration of reactants and products during a chemical reaction?

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

Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2 is 6.94 × 10-1 mol L-1 s-1, what is the rate of the loss of O3? 2O3(g)→ 3O2(g)

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g)→ 4NO2(g)+ O2(g). If the rate of appearance of NO2 is equal to 0.560 mol min-1 at a particular moment, what is the rate of appearance of O2 at that moment?

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

Calculate the temperature if a reaction has a rate constant, k, of 841 s-1, a frequency factor, A, of 6.0 × 1012 s-1, and an activation energy, Ea, of 62 kJ mol-1.

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

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if Ea = 85.6 kJ mol-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?

The combustion of ethylene proceeds by the reaction C2H4(g)+ 3O2(g)→ 2CO2(g)+ 2H2O(g) When the rate of disappearance of O2 is 0.28 mol L-1 s-1, the rate of appearance of CO2 is ________ Mol L-1 s-1.

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

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Calculate the temperature if a reaction has a rate constant, k, of 21.3 s^-1, a frequency factor, A, of 7.98 × 10¹³ s^-1, and an activation energy, E_a, of 102 kJ mol^-1.

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?

The following reaction is first order, C₂H₆ → 2CH₃. If the rate constant is equal to 5.5 × 10^-4 s^-1 at 1000 K, how long will it take for 0.35 mol of C₂H₆ in a 1.00 L container to decrease to 0.20 mol in the same container?

The isomerization reaction, CH₃NC → CH₃CN, is first order and the rate constant is equal to 0.46 s^-1 at 600 K. What is the concentration of CH₃NC after 0.20 minutes if the initial concentration is 0.30 mol L^-1?

The isomerization of methylisonitrile to acetonitrile CH₃NC(g)→ CH₃CN(g) Is first order in CH₃NC. The half-life of the reaction is 5.20 × 10¹ s at 545 K. The rate constant when the initial [CH₃NC] is 0.030 mol L^-1 is ________ s^-1.

Calculate the frequency factor, A, for a reaction with a rate constant of 162.3 s^-1 and an activation energy, E_a, of 68 kJ mol^-1 at 298 K.

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. If the rate of formation of O₂ is 6.94 × 10^-1 mol L^-1 s^-1, what is the rate of the loss of O₃? 2O₃(g)→ 3O₂(g)

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g)→ 4NO₂(g)+ O₂(g). If the rate of appearance of NO₂ is equal to 0.560 mol min^-1 at a particular moment, what is the rate of appearance of O₂ at that moment?

Calculate the temperature if a reaction has a rate constant, k, of 841 s^-1, a frequency factor, A, of 6.0 × 10¹² s^-1, and an activation energy, E_a, of 62 kJ mol^-1.

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

A particular first-order reaction has a rate constant of 1.35 × 10² s^-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if E_a = 85.6 kJ mol^-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?

The combustion of ethylene proceeds by the reaction C₂H₄(g)+ 3O₂(g)→ 2CO₂(g)+ 2H₂O(g) When the rate of disappearance of O₂ is 0.28 mol L^-1 s^-1, the rate of appearance of CO₂ is ________ Mol L^-1 s^-1.