Chem Lesson 2: 12.4 - 12.6 Flashcards

1
Q

Integrated Rate Laws

A

Let’s us see the concentration of a reactant at any given time.

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2
Q

Integrated Rate Law (Zero Order Equation)

A

[A]f = [A]o - kt

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3
Q

Integrated Rate Law (First Order Equation)

A

ln[A] = ln[A]o - kt

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4
Q

Integrated Rate Law (Second Order Equation)

A

1/[A] = 1/[A]o + kt

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5
Q

K Unit for Zero Order

A

M^1t^-1

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6
Q

K Unit for First Order

A

t^-1

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7
Q

K Unit for Second Order

A

M^-1t^-1

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8
Q

Yes or No - Does the half life of a first order reaction depend on the initial concentration.

A

No

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9
Q

Half Life - Zero Order Reaction

A

[Ao] / 2k

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10
Q

Half Life - First Order Reaction (Mysterio)

A

ln*2 / k
0.693 / k

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11
Q

Half Life - Second Order Reaction

A

1 / (k * [Ao])

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12
Q

K Unit for Third Order

A

M^-2 t^-1

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13
Q

Decaying Order

A

First Order

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14
Q

How to cancel Ln out?

A

Raise both sides to the e^ power.

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15
Q

100% in Integer form

A

100

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16
Q

100% in Fraction form

A

1

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17
Q

Collision Theory

A

Requirements that need to take place for a chemical reaction to occur:
1. Collision (must collide).
2. Proper orientation.
3. Sufficient energy (to get over activation barrier).

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18
Q

Arrhenius Equation (def)

A

Relates activation energy and the rate constant (k).

19
Q

Arrhenius Equation (Exponential equation - before two point)

A

k = Ae^-Ea/RT

20
Q

Arrhenius Equation (Y = mx + b)

A

ln(k) = - Ea/R(1/T) + lnA

21
Q

Frequency Factor (A) - Arrhenius Equation (Definition for A)

A

Fraction of molecules that have the proper orientation when they collide.

22
Q

R (energy constant value for rate law)

A

8.314 J/mol * k

23
Q

Transition states

A

Short lived molecules formed in between reactants turning into products.

(Forms when E,a is met - top point of graph).

24
Q

(e^-Ea/RT) def in Arrenius Equation

A

Fraction of molecules that have enough energy to get over the activation energy barrier.

25
Q

Activation Energy (E,a)

A

Minimum amount of energy needed to make products during a collision.

26
Q

E,a (graphical method slope equation)

A

ea = -(slope)(R)

27
Q

Two Point Arrhenius Formula (two temps &/or two Rate Constants)

A

ln(k1/k2) = Ea/R * (1/T^2 - 1/T^1)

28
Q

Ea Unit

A

J mol^-1
or
J/mol

29
Q

C —> K

A

C + 273.15

30
Q

Frequency Factor (A Equation) - Find K

A

k = Ae^-Ea/RT

31
Q

Frequency Factor (A) Unit

A

Same as K values

32
Q

Reaction Mechanism

A

Provides precise details of the step-by-step process by which a reaction occurs.

33
Q

Elementary reaction

A

Each step in a reaction mechanism.

34
Q

Intermediate

A

Species that are produced in one step and used up in another step. (Appears on product side first then cancels out).

35
Q

Molecularity (Elementary Reaction)

A

Number of reactant entities (atoms, molecules, ions).

36
Q

Unimolecular Reaction

A

Reactions involving a single reactant entity to produce one or more products.

Usually happens when one reactant breaks up into two or more products.

A —-> Products
rate = k[A]

37
Q

Biomolecular Reaction

A

Reaction involving two reactants to produce one or more products.

A + B —-> Products
rate = k[A][B]

2A ——-> Products
rate = k[A]^2

38
Q

Termolecular Reaction

A

Reaction involving the simultaneous collision of three entities.
*Rare
2NO + O –> 2No,2
rate = k[NO]^2[O,2]

39
Q

Rate Limiting Step (Role Determining Step)

A

Slowest step in an elementary reaction.
*Slowest step is the first used in a rate law. If slowest step is after fast step must solve differently.

40
Q

Overall Reaction

A

Sum of all the elementary steps of the reaction.

41
Q

Intermediate vs. Catalyst

A

Intermediate appears on the products side first then cancels out. Catalyst appears on the reactant side first then cancels out.

42
Q

k,1 Elementary Reactions

A

The forward reaction

43
Q

Enthalpy

A

The internal energy of a system plus the P*V

44
Q

Arrenihus Equation (Def)

A

Describes the relationship between the reaction rate and temperature for chemical reactions.