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Chemistry > Chemical Kinetics Concepts > Flashcards

Chemical Kinetics Concepts Flashcards

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1
Q

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

A

Chemical kinetics

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2
Q

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

A

change in the concentrations of reactants and products with time

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3
Q

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

A

Balanced chemical equation

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4
Q

balanced chemical equation for a reaction describes the quantitative
relationships between

A

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

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5
Q

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

A

False

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6
Q

Factors that affect reaction rates

A

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

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7
Q

Two substances cannot possibly react with each other unless _______

A

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

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8
Q

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

A

zero

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9
Q

the more particles collide per unit time, the __________.

A

the more a reaction between them
can occur.

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10
Q

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

A

increases

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11
Q

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

A

True

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12
Q

the more particles collide per unit time, _________________.

A

the more a reaction between them
can occur.

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13
Q

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

A

increases

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14
Q

Relationship between temperature and average kinetic energy

A

Directly proportional

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15
Q

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

A

Increases

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16
Q

What happens when the average kinetic energy increases

A

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

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17
Q

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

A

decreasing

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18
Q

Example of where temperature affects rate of reaction

A

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

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19
Q

True or False: Catalysts affect net chemical change itself

A

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

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20
Q

a substance that participates in a chemical reaction

A

Catalysts

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21
Q

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

A

Increasing

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22
Q

If the surface area of a reactant is increased:

A

✓ 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.

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23
Q

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

A

exposed

24
Q

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

A

The rate of reaction also increases

25
Q

What happens when the pressure of gaseous reactants is increased

A

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

26
Q

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

A

Faster

27
Q

If the pressure of gaseous reactants is increased

A

there are more reactant
particles for a given volume.

28
Q

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

A

Higher

29
Q

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

A

Reaction rate

30
Q

units for reaction rate

A

moles per liter per unit time

31
Q

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

A

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

32
Q

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

A

reaction rate

33
Q

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

A

True

34
Q

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

A

Diethyl ether

35
Q

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

A

ethylene

36
Q

Square brackets indicate _______

A

Molar concentration

37
Q

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

A

change in

38
Q

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).

A

Average reaction time

39
Q

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

A

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).

40
Q

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

A

rate law

41
Q

Rate law formula

A

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

42
Q

Reaction order: rate multiplied by 1

A

0

43
Q

Reaction order: rate multiplied by 2

A

1st order

44
Q

Reaction order: rate multiplied by 4

A

2nd order

45
Q

Reaction order: rate multiplied by 1/2

A

-1

46
Q

Rate constant: rate multiplied by 1

A

k

47
Q

Rate constant: rate multiplied by 2

A

k[A]

48
Q

Rate constant: rate multiplied by 4

A

k[A]^2

49
Q

is simply the sum of orders for each
reactant.

A

overall reaction order

50
Q

describe the mathematical
dependence of the rate on reactant concentrations.

A

reaction order

51
Q

The reaction orders in a rate law describe the

A

mathematical
dependence of the rate on reactant concentrations.

52
Q

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

A

initial rate

53
Q

units on k if overall reaction order is 0

A

M/s

54
Q

units on k if overall reaction order is 1

A

1/s

55
Q

units on k if overall reaction order is 2

A

1/(M*s)

56
Q

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;

A

Integrated rate laws

Chemistry (29 decks)

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