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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?


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

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The rate constant for the first-order decomposition of N2O is 3.40 s-1.What is the half-life of the decomposition?


A) 0.491 s
B) 0.204 s
C) 0.236 s
D) 0.424 s
E) 0.294 s

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B

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M.What is the rate constant for this reaction?


A) 1.0 × 10-2 M-1s-1
B) 4.5 × 10-2 M-1s-1
C) 9.7 × 10-2 M-1s-1
D) 2.2 × 10-2 M-1s-1
E) 3.8 × 10-2 M-1s-1

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The rate constant for a zero-order reaction is 0.54 s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?


A) 0.089 s
B) 1.8 s
C) 0.31 s
D) 5.6 s
E) 1.3 s

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Derive an expression for a "1/3-life" for a first-order reaction.


A)
Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
B)
Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
C)
Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
D)
Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)
E)
Derive an expression for a 1/3-life for a first-order reaction. A) B) C) D) E)

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Identify the CFC with the shortest atmospheric lifetime.


A) CFC-113
B) CFC-12
C) CFC-114
D) CFC-11
E) CFC-115

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D

Write a balanced reaction for which the following rate relationships are true. Rate = Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O = Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O = - Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O


A) Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O N2 + O2 →

Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O N2O
B) 2 N2O → 2 N2 + O2
C) N2O → N2 + 2 O2
D) Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O N2O →
Write a balanced reaction for which the following rate relationships are true. Rate = = = - A) N<sub>2</sub> + O<sub>2 </sub>→<sub> </sub> <sub> </sub> N<sub>2</sub>O B) 2 N<sub>2</sub>O → 2 N<sub>2</sub> + O<sub>2</sub> C) N<sub>2</sub>O → N<sub>2</sub> + 2 O<sub>2</sub> D) N<sub>2</sub>O → N<sub>2</sub> + O<sub>2</sub> E) 2 N<sub>2</sub> + O<sub>2 </sub>→ 2 N<sub>2</sub>O N2 + O2
E) 2 N2 + O2 → 2 N2O

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Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation. 2 NO2(g) → 2 NO(g) + O2(g) . A sample of NO2(g) is initially placed in a 2.50-L reaction vessel at 300°C.If the half-life and the rate constant at 300°C are 11 seconds and 0.54 M-1 s-1,respectively,how many moles of NO2 were in the original sample?


A) 0.17 mol
B) 0.42 mol
C) 5.9 mol
D) 15 mol

Correct Answer

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


A) What are the units of k in the following rate law? Rate = k[X] A) B) M<sup> </sup>s<sup>2</sup> C) D) E)
B) M s2
C) What are the units of k in the following rate law? Rate = k[X] A) B) M<sup> </sup>s<sup>2</sup> C) D) E)
D) What are the units of k in the following rate law? Rate = k[X] A) B) M<sup> </sup>s<sup>2</sup> C) D) E)
E) What are the units of k in the following rate law? Rate = k[X] A) B) M<sup> </sup>s<sup>2</sup> C) D) E)

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The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1.If the initial concentration of cyclopropane is 1.33 M,what is the concentration of cyclopropane after 644 s?


A) 0.43 M
B) 0.15 M
C) 0.94 M
D) 0.86 M
E) 0.67 M

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Which rate law has a molecularity of two?


A) Rate = k[A]0
B) Rate = k[A][B]
C) Rate = k[A][B][C]
D) Rate = k[A]
E) Rate = k[A]3

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How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?


A) 3
B) 2
C) 2.5
D) 2.75
E) 8

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Which of the following represents the integrated rate law for a second-order reaction?


A) Which of the following represents the integrated rate law for a second-order reaction? A) = - kt B) - = kt C) [A]<sub>o</sub> - [A]<sub>t</sub> = - kt D) k = Ae<sup>(Ea/RT) </sup> E) = - lnA = - kt
B) Which of the following represents the integrated rate law for a second-order reaction? A) = - kt B) - = kt C) [A]<sub>o</sub> - [A]<sub>t</sub> = - kt D) k = Ae<sup>(Ea/RT) </sup> E) = - lnA -
Which of the following represents the integrated rate law for a second-order reaction? A) = - kt B) - = kt C) [A]<sub>o</sub> - [A]<sub>t</sub> = - kt D) k = Ae<sup>(Ea/RT) </sup> E) = - lnA = kt
C) [A]o - [A]t = - kt
D) k = Ae(Ea/RT)
E) Which of the following represents the integrated rate law for a second-order reaction? A) = - kt B) - = kt C) [A]<sub>o</sub> - [A]<sub>t</sub> = - kt D) k = Ae<sup>(Ea/RT) </sup> E) = - lnA =
Which of the following represents the integrated rate law for a second-order reaction? A) = - kt B) - = kt C) [A]<sub>o</sub> - [A]<sub>t</sub> = - kt D) k = Ae<sup>(Ea/RT) </sup> E) = - lnA
Which of the following represents the integrated rate law for a second-order reaction? A) = - kt B) - = kt C) [A]<sub>o</sub> - [A]<sub>t</sub> = - kt D) k = Ae<sup>(Ea/RT) </sup> E) = - lnA - lnA

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


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

Correct Answer

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


A) Rate = - Given the following balanced equation,determine the rate of reaction with respect to [SO<sub>3</sub>]. 2 SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = + D) Rate = - E) It is not possible to determine without more information.
Given the following balanced equation,determine the rate of reaction with respect to [SO<sub>3</sub>]. 2 SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = + D) Rate = - E) It is not possible to determine without more information.
B) Rate = + Given the following balanced equation,determine the rate of reaction with respect to [SO<sub>3</sub>]. 2 SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = + D) Rate = - E) It is not possible to determine without more information.
Given the following balanced equation,determine the rate of reaction with respect to [SO<sub>3</sub>]. 2 SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = + D) Rate = - E) It is not possible to determine without more information.
C) Rate = + Given the following balanced equation,determine the rate of reaction with respect to [SO<sub>3</sub>]. 2 SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = + D) Rate = - E) It is not possible to determine without more information.
D) Rate = - Given the following balanced equation,determine the rate of reaction with respect to [SO<sub>3</sub>]. 2 SO<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 SO<sub>3</sub>(g) A) Rate = - B) Rate = + C) Rate = + D) Rate = - E) It is not possible to determine without more information.
E) It is not possible to determine without more information.

Correct Answer

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Given the following proposed mechanism,predict the rate law for the overall reaction. A2 + 2 B → 2 AB (overall reaction) Mechanism A2 ⇌ 2 A fast A + B → AB slow


A) Rate = k[A]1/2[B]2
B) Rate = k[A2][B]
C) Rate = k[A2]2[B]1/2
D) Rate = k[A2]1/2
E) Rate = k[A2]1/2[B]

Correct Answer

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


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

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What is the overall order of the following reaction,given the rate law? 2 NO(g) + H2(g) → N2(g) + 2 H2O(g) Rate = k[NO]2[H2]


A) 1st order
B) 2nd order
C) 3rd order
D) 4th order
E) 0th order

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C

What are the units of k in the following rate law? Rate = k[X]2[Y]


A) What are the units of k in the following rate law? Rate = k[X]<sup>2</sup>[Y]<sup> </sup> A) B) C) M<sup>2</sup>s<sup>2</sup> D) E)
B) What are the units of k in the following rate law? Rate = k[X]<sup>2</sup>[Y]<sup> </sup> A) B) C) M<sup>2</sup>s<sup>2</sup> D) E)
C) M2s2
D) What are the units of k in the following rate law? Rate = k[X]<sup>2</sup>[Y]<sup> </sup> A) B) C) M<sup>2</sup>s<sup>2</sup> D) E)
E) What are the units of k in the following rate law? Rate = k[X]<sup>2</sup>[Y]<sup> </sup> A) B) C) M<sup>2</sup>s<sup>2</sup> D) E)

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Biological catalysts that increase the rates of biochemical reactions are known as


A) substrates.
B) inhibitors.
C) enzymes.
D) binders.
E) trumanettes.

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