Chem Lesson 2: 12.4 - 12.6

Question 1

Integrated Rate Laws

Answer 1

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

Question 2

Integrated Rate Law (Zero Order Equation)

Answer 2

[A]f = [A]o - kt

Question 3

Integrated Rate Law (First Order Equation)

Answer 3

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

Question 4

Integrated Rate Law (Second Order Equation)

Answer 4

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

Question 5

K Unit for Zero Order

Answer 5

M^1t^-1

Question 6

K Unit for First Order

Answer 6

t^-1

Question 7

K Unit for Second Order

Answer 7

M^-1t^-1

Question 8

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

Answer 8

No

Question 9

Half Life - Zero Order Reaction

Answer 9

[Ao] / 2k

Question 10

Half Life - First Order Reaction (Mysterio)

Answer 10

ln*2 / k
0.693 / k

Question 11

Half Life - Second Order Reaction

Answer 11

1 / (k * [Ao])

Question 12

K Unit for Third Order

Answer 12

M^-2 t^-1

Question 13

Decaying Order

Answer 13

First Order

Question 14

How to cancel Ln out?

Answer 14

Raise both sides to the e^ power.

Question 15

100% in Integer form

Answer 15

100

Question 16

100% in Fraction form

Answer 16

1

Question 17

Collision Theory

Answer 17

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).

Question 18

Arrhenius Equation (def)

Answer 18

Relates activation energy and the rate constant (k).

Question 19

Arrhenius Equation (Exponential equation - before two point)

Answer 19

k = Ae^-Ea/RT

Question 20

Arrhenius Equation (Y = mx + b)

Answer 20

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

Question 21

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

Answer 21

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

Question 22

R (energy constant value for rate law)

Answer 22

8.314 J/mol * k

Question 23

Transition states

Answer 23

Short lived molecules formed in between reactants turning into products.

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

Question 24

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

Answer 24

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

Question 25

Activation Energy (E,a)

Answer 25

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

Question 26

E,a (graphical method slope equation)

Answer 26

ea = -(slope)(R)

Question 27

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

Answer 27

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

Question 28

Ea Unit

Answer 28

J mol^-1 or J/mol

Question 29

C ---> K

Answer 29

C + 273.15

Question 30

Frequency Factor (A Equation) - Find K

Answer 30

k = Ae^-Ea/RT

Question 31

Frequency Factor (A) Unit

Answer 31

Same as K values

Question 32

Reaction Mechanism

Answer 32

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

Question 33

Elementary reaction

Answer 33

Each step in a reaction mechanism.

Question 34

Intermediate

Answer 34

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

Question 35

Molecularity (Elementary Reaction)

Answer 35

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

Question 36

Unimolecular Reaction

Answer 36

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]

Question 37

Biomolecular Reaction

Answer 37

Reaction involving two reactants to produce one or more products. A + B ----> Products rate = k[A][B] 2A -------> Products rate = k[A]^2

Question 38

Termolecular Reaction

Answer 38

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

Question 39

Rate Limiting Step (Role Determining Step)

Answer 39

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.

Question 40

Overall Reaction

Answer 40

Sum of all the elementary steps of the reaction.

Question 41

Intermediate vs. Catalyst

Answer 41

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

Question 42

k,1 Elementary Reactions

Answer 42

The forward reaction

Question 43

Enthalpy

Answer 43

The internal energy of a system plus the P*V

Question 44

Arrenihus Equation (Def)

Answer 44

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