Chemical Kinetics Concepts

Question 1

The study of reaction rates defined by the change in the concentrations of
reactants and products with time.

Answer 1

Chemical kinetics

Question 2

Chemical kinetics is the study of reactions rates defined by the ______

Answer 2

change in the concentrations of reactants and products with time

Question 3

describes the quantitative
relationships between the amounts of reactants present and the amounts of products
that can be formed,

Answer 3

Balanced chemical equation

Question 4

balanced chemical equation for a reaction describes the quantitative
relationships between

Answer 4

the amount of reactants present and the amount of products that can be formed

Question 5

True or False: Balanced chemical equations can sometimes indicate how fast a reaction will occur

Answer 5

False

Question 6

Factors that affect reaction rates

Answer 6

Molecular orientation
Concentration
temperature
catalyst
pressure
surface area
reactant state of matter

Question 7

Two substances cannot possibly react with each other unless _______

Answer 7

their
individual particles (molecules, atoms, or ions) come into contact.

Question 8

If
there is no contact, the reaction rate will be ________

Answer 8

zero

Question 9

the more particles collide per unit time, the __________.

Answer 9

the more a reaction between them
can occur.

Question 10

the reaction rate usually ________ as the concentration of the
reactants increases.

Answer 10

increases

Question 11

True or False: The more the reactant particles moving together, the more the molecules collide.

Answer 11

True

Question 12

the more particles collide per unit time, _________________.

Answer 12

the more a reaction between them
can occur.

Question 13

Consequently, the reaction rate usually _________ as the concentration of the
reactants increases.

Answer 13

increases

Question 14

Relationship between temperature and average kinetic energy

Answer 14

Directly proportional

Question 15

Increasing the temperature of a system ________ the average kinetic energy of its
individual particles.

Answer 15

Increases

Question 16

What happens when the average kinetic energy increases

Answer 16

the particles move faster
and collide more frequently per unit time and possess greater energy when they collide.

Question 17

the reaction rate of virtually all reactions decreases
with ________ temperature.

Answer 17

decreasing

Question 18

Example of where temperature affects rate of reaction

Answer 18

refrigeration retards the rate of growth of bacteria
in foods by decreasing the reaction rates of biochemical
reactions that enable bacteria to reproduce.

Question 19

True or False: Catalysts affect net chemical change itself

Answer 19

False: Catalysts increases the reaction rate without undergoing a net chemical change itself.

Question 20

a substance that participates in a chemical reaction

Answer 20

Catalysts

Question 21

The rate of a chemical reaction can be raised by
_______ the surface area of a solid reactant.

Answer 21

Increasing

Question 22

If the surface area of a reactant is increased:

Answer 22

✓ more particles are exposed to the other reactant;

✓ the rate of reaction increases;

✓ there is a greater chance of particles colliding, which leads to more
successful collisions per second.

Question 23

If the surface area is increased, more particles are _____ to the other reactant

Answer 23

exposed

Question 24

What happens to the rate of reaction when there is an increase in the surface area

Answer 24

The rate of reaction also increases

Question 25

What happens when the pressure of gaseous reactants is increased

Answer 25

the particles of the reactant for a given volume also increases.

Question 26

The higher the pressure of reactants, the ___________ the rate of a reaction will be.

Answer 26

Faster

Question 27

If the pressure of gaseous reactants is increased

Answer 27

there are more reactant particles for a given volume.

Question 28

The _________ the pressure of reactants, the faster the rate of a reaction will be.

Answer 28

Higher

Question 29

Expressed as the concentration of reactant consumed or the concentration of product formed per unit time.

Answer 29

Reaction rate

Question 30

units for reaction rate

Answer 30

moles per liter per unit time

Question 31

The units are moles per liter per unit time, written as

Answer 31

M/s, M/min, or M/h.

Question 32

is the change in the concentration of either the reactant or the product over a period of time.

Answer 32

reaction rate

Question 33

true or False: In systems where more than one reaction is possible, the same reactants can produce different products under different reaction conditions.

Answer 33

True

Question 34

in the presence of dilute sulfuric acid and at temperatures around 100°C, ethanol is converted to ___________:

Answer 34

Diethyl ether

Question 35

At 180°C, however, a completely different reaction occurs, which produces _______ as the major product:

Answer 35

ethylene

Question 36

Square brackets indicate _______

Answer 36

Molar concentration

Question 37

the capital Greek delta (Δ) means “___________”.

Answer 37

change in

Question 38

can be calculated from the concentrations of either the reactant or one of the products at thebeginning of the interval (time = t0) and at the end of the interval (t1).

Answer 38

Average reaction time

Question 39

The average reaction rate for a given time interval can be calculated

Answer 39

from the concentrations of either the reactant or one of the products at the beginning of the interval (time = t0) and at the end of the interval (t1).

Question 40

Mathematical relationship between the chemical reaction and the concentration of its reactants.

Answer 40

rate law

Question 41

Rate law formula

Answer 41

RATE LAW = k [A]x[B]y

Question 42

Reaction order: rate multiplied by 1

Answer 42

0

Question 43

Reaction order: rate multiplied by 2

Answer 43

1st order

Question 44

Reaction order: rate multiplied by 4

Answer 44

2nd order

Question 45

Reaction order: rate multiplied by 1/2

Answer 45

-1

Question 46

Rate constant: rate multiplied by 1

Answer 46

k

Question 47

Rate constant: rate multiplied by 2

Answer 47

k[A]

Question 48

Rate constant: rate multiplied by 4

Answer 48

k[A]^2

Question 49

is simply the sum of orders for each reactant.

Answer 49

overall reaction order

Question 50

describe the mathematical dependence of the rate on reactant concentrations.

Answer 50

reaction order

Question 51

The reaction orders in a rate law describe the

Answer 51

mathematical dependence of the rate on reactant concentrations.

Question 52

is the instantaneous rate at the start of the reaction (when t = 0).

Answer 52

initial rate

Question 53

units on k if overall reaction order is 0

Answer 53

M/s

Question 54

units on k if overall reaction order is 1

Answer 54

1/s

Question 55

units on k if overall reaction order is 2

Answer 55

1/(M*s)

Question 56

express the reaction rate as a function of the initial concentration and a measured (actual) concentration of one or more reactants after a specific amount of time (t) has passed;

Answer 56

Integrated rate laws