Chapter 13 Flashcards

1
Q

Rate of Reaction

A

A measure of how fast the reaction occurs.

Rate = -(1/a)∙[ ∆[A] / ∆t ]

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2
Q

Instantaneous Rate of Reaction

A

The rate at any one point in time

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3
Q

Rate Law

A

Relationship between the rate of a reaction and the concentration of the reactants.

Rate = k[A]n

Rate = k[A]m[B]n

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4
Q

Overall order of Reaction

A

Sum of the exponents

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5
Q

Half Life

A

The time required for the concentration of a reactant to fall to one-half of its initial value.

  • First-Order Reaction: half-life is independent of initial concentration.
  • Zero-Order and Second-Order half-lives depend on the initial concentration.
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6
Q

Arrhenius Equation

A

k = Ae-Ea/RT

  • Relates the rate constant of a reaction to the temperature, activation energy, and frequency factor.
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7
Q

Reaction Mechanism

A
  • Series of individual chemical steps by which an overall chemical reaction occurs.
  • Each step is an elementary step - cannot be broken down into simpler steps
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8
Q

Molecularity

A

The number of reactant particles involved in an elementary step.

  • A -> products : Unimolecular
  • A+A -> products : Bimolecular
  • A+B -> products : Bimolecular
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9
Q

Termolecular Steps

A

Elementary steps in which three reactant particles collide.

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10
Q

Rate-Determining Step

A
  • Limits the overall rate of the reaction thus determining the rate law for the overall reaction.
  • Slower than other elementary steps.
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11
Q

Homogeneous Catalysis

A

Catalysis in which the catalyst exists in the same phase (or state) as the reactants.

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12
Q

Heterogeneous Catalysis

A

Catalysis in which the catalyst and the reactants exist in different phases.

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13
Q

Frequency Factor (A)

A

The number of times that the reactants approach the activation barrier per unit time.

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14
Q

Exponential Factor (e)

A
  • The fraction of approaches that are successful in surmounting the activation barrier and forming products.
  • Increases with increasing temperature but decreases with increasing activation energy.
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15
Q

Activation Energy

A

Energy barrier in a chemical reaction that must be overcome for the reactants to be converted into products.

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16
Q

Arrhenius Equation - Linear Form

A

ln(k) = ln(A) - (Ea/R) x (1/T)

17
Q

Arrhenius Equation - Two Point Form

A

ln (k2/k1) = (Ea/R) x [(1/T1) - (1/T2)]

18
Q

Integrated Rate Law - Zero Order

A
  • [A]t = [A]o- kt
  • Units of K: M∙s-1
19
Q

Integrated Rate Law - First Order

A
  • ln[A]t = ln[A]o- kt
  • Units of k: s-1
20
Q

Integrated Rate Law - Second Order

A
  • 1/[A]t = kt + 1/[A]o
  • Units of k: M-1∙s-1
21
Q

Half-Life, Zero Order

A

t1/2 = [A]o/2k

22
Q

Half-Life, First Order

A

t1/2 = 0.693/k

23
Q

Half-Life, Second Order

A

t1/2 = 1/k[A]o

24
Q

Rate Law - Zero Order Reaction

A
  • n=0
  • rate is independent of the concentration of A.
25
Q

Rate Law - First Order Reaction

A
  • n=1
  • rate is directly proportional to the concentration of A
26
Q

Rate Law- Second Order Reaction

A
  • n=2
  • rate is proportional to the square of the concentration of A.