Question 1

The rate constant for a zero-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

Question 2

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

Accepted Answer

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

Question 3

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

Accepted Answer

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

Question 4

The elementary reaction 2NO2(g)→ 2NO(g)+ O2(g)
Is second order in NO2 and the rate constant at 501 K is 7.93 × 10-3 L mol-1 s-1. The reaction half-life at this temperature when [NO2]0 = 0.45 mol L-1 is ________ s.

Accepted Answer

A) 3.6 × 10-3 
B) 0.011 
C) 126 
D) 87 
E) 280 
A) 3.6 × 10-3 
B) 0.011 
C) 126 
D) 87 
E) 280

Question 5

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Accepted Answer

A) 0.143 hr 
B) 2.28 hr 
C) 6.99 hr 
D) 22.7 hr 
A) 0.143 hr 
B) 2.28 hr 
C) 6.99 hr 
D) 22.7 hr

Question 6

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 7

In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3-, and bromide ion, Br-, according to the following chemical equation: 3BrO-(aq)→ BrO3-(aq)+ 2BR-(aq)
A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 L mol-1 s-1. If the initial concentration of BrO- is 0.80 mol L-1, how long will it take one-half of the BrO- ion to react?

Accepted Answer

A) 4.5 × 10-2 s 
B) 7.1 s 
C) 12 s 
D) 22 s 
A) 4.5 × 10-2 s 
B) 7.1 s 
C) 12 s 
D) 22 s

Question 8

Which rate law is bimolecular?

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][A][B] 
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][A][B]

Question 9

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

Accepted Answer

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

Question 10

Which of the following reactions would you predict to have the largest orientation factor?

Accepted Answer

A) NOF(g)+ NOF(g)→ 2NO(g)+ F2(g) 
B) Br2(g)+ H2C=CH2(g)→ H2BrC-CBrH2(g) 
C) NH3(g)+ BCl3(g)→ H3N-BCl3(g) 
D) H(g)+ Cl(g)→ HCl(g) 
E) All of these reactions should have nearly identical orientation factors. 
A) NOF(g)+ NOF(g)→ 2NO(g)+ F2(g) 
B) Br2(g)+ H2C=CH2(g)→ H2BrC-CBrH2(g) 
C) NH3(g)+ BCl3(g)→ H3N-BCl3(g) 
D) H(g)+ Cl(g)→ HCl(g) 
E) All of these reactions should have nearly identical orientation factors.

Question 11

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 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 rate constant for a first-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

Question 14

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 15

Define half-life.

Accepted Answer

A half-life of a reaction is t

Question 16

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

Accepted Answer

A) 1.00% 
B) 37.8% 
C) 40.2% 
D) 62.2% 
A) 1.00% 
B) 37.8% 
C) 40.2% 
D) 62.2%

Question 17

The rate of disappearance of HBr in the gas phase reaction 2HBr(g)→ H2 (g)+ Br2 (g)
Is 0.130 mol L-1 s-1 at 150 °C. The rate of reaction is ________ mol L-1 s-1.

Accepted Answer

A) 3.85 
B) 0.0650 
C) 0.0169 
D) 0.260 
E) 0.0860 
A) 3.85 
B) 0.0650 
C) 0.0169 
D) 0.260 
E) 0.0860

Question 18

What are the units of k in a first-order reaction?

Accepted Answer

A) mol L-1 s-1 
B) mol L-1 s 
C) L mol-1 s-1 
D) M2 s-1 
E) s-1 
A) mol L-1 s-1 
B) mol L-1 s 
C) L mol-1 s-1 
D) M2 s-1 
E) s-1

Question 19

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

Accepted Answer

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

Question 20

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

Accepted Answer

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

Exam 13: Chemical Kinetics

The rate constant for a zero-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?

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

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

The elementary reaction 2NO2(g)→ 2NO(g)+ O2(g) Is second order in NO2 and the rate constant at 501 K is 7.93 × 10-3 L mol-1 s-1. The reaction half-life at this temperature when [NO2]0 = 0.45 mol L-1 is ________ s.

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

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.

Which rate law is bimolecular?

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

Which of the following reactions would you predict to have the largest orientation factor?

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?

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

The rate constant for a first-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?

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

Define half-life.

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

The rate of disappearance of HBr in the gas phase reaction 2HBr(g)→ H2 (g)+ Br2 (g) Is 0.130 mol L-1 s-1 at 150 °C. The rate of reaction is ________ mol L-1 s-1.

What are the units of k in a first-order reaction?

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

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

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The rate constant for a zero-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?

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

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

The elementary reaction 2NO₂(g)→ 2NO(g)+ O₂(g) Is second order in NO₂ and the rate constant at 501 K is 7.93 × 10^-3 L mol^-1 s^-1. The reaction half-life at this temperature when [NO₂]₀ = 0.45 mol L^-1 is ________ s.

The first-order reaction, SO₂Cl₂ → SO₂ + Cl₂, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

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.

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?

The rate constant for a first-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?

The first-order reaction, SO₂Cl₂ → SO₂ + Cl₂, has a rate constant equal to 2.20 × 10^-5 s^-1 at 593 K. What percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours?

The rate of disappearance of HBr in the gas phase reaction 2HBr(g)→ H₂ (g)+ Br₂ (g) Is 0.130 mol L^-1 s^-1 at 150 °C. The rate of reaction is ________ mol L^-1 s^-1.

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