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ANACHEM > Chemical Kinetics > Flashcards

Chemical Kinetics Flashcards

1
Q

study that deals with how fast the reaction will proceed to completion

A

chemical kinetics

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2
Q

what is the formula for rate of reaction?

A

Rate = Δconc/Δt
or
Rate = Δ[A]/Δt

Δ = change; [ ] = conc. (in M usually); t = unit time; A = substance A

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3
Q

in a rxn, what do u call something that is consumed?

A

reactant

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4
Q

in a rxn, what is something that is formed?

A

product

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5
Q

If 4A → 2B, what is the rate expression?

rate expression = rate of disappearance = rate of formation

A

Rate = -1/4 Δ[A]/Δt = 1/2 Δ[B]/Δt

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6
Q

Accdg to the collision theory of reaction, atoms/molecules/ions must ____ for reactions to occur

A

collide

collision theory nga eh haha!

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7
Q

↑ or ↓ rxn rate?

more collisions

A

↑ reaction rate

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8
Q

in the transition state theory, what do you call the high energy intermediate that reactants must reach before falling into products?

A

transition state

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9
Q

in the transition state theory, what do you call the energy that reactants must acquire to reach the transition state?

A

activation energy

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10
Q

T or F

the rate of rxn is dependent on the reactants’ nature

A

True

same nature = ↑ rxn rate

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11
Q

↑ or ↓ rxn rate?

reactants have fewer and weaker bonds

A

↑ rxn rate

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12
Q

T or F?

reactions between molecules are slower than that of ions

A

True

mas mabilis ions kasi no bond-breaking is needed; can form bonds alr

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13
Q

↑ or ↓ rxn rate?

compounds by ionic bonds

A

↑ rxn rate

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14
Q

↑ or ↓ rxn rate?

the concentration of reactants is increased

A

↑ rxn rate

because collisions are more likely

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15
Q

↑ or ↓ rxn rate?

in gases, the pressure in a container is higher than normal

A

↑ rxn rate

↑P↓V lower volume = more compressed = more collisions

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16
Q

↑ or ↓ rxn rate?

in solids, the surface area is increased

A

↑ rxn rate

↑ surface area = breaking a solid reactant into smaller particles

breaking a solid reactant into smaller particles increases the number of particles available for collision

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17
Q

↑ or ↓ rxn rate?

in solids, the surface area is increased

A

↑ rxn rate

↑ surface area = breaking a solid reactant into smaller particles

breaking a solid reactant into smaller particles increases the number of particles available for collision

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18
Q

the average rate of a reaction ____ as the reaction proceeds

increases or decreases?

A

decreases

decreases kasi as the rxn proceeds, nababawasan conc. ng reactants

lower conc. of reactants leads to lower rxn rate

19
Q

enumerate the formula for rate law given the substance A

A

rate = k[A]x

k = rate constant; x = rxn order; [ ] = conc.; A = reactant A

rate is directly proportional to the concentration of reactant

20
Q

what law expresses the relationship of the rate of rxn to the rate constant and the conc. of the reactants raised to its rxn order

A

rate law

21
Q

what do you call the reaction by which the rate does not vary with the increase or decrease in the concentration of the reactants?

A

zero-order reaction

rate of rxn is independent of all reactant concentrations

22
Q

what reaction can be defined as a chemical reaction for which the reaction rate is entirely dependent on the concentration of only one reactant?

if conc. is doubled, the rxn rate is also doubled

A

first-order reaction

23
Q

what reaction is one whose rate is proportional to the square of the concentration of one reactant? It also has a reaction rate that is proportional to the product of the concentrations of two reactants

if conc. is doubled, the rxn rate is quadrupled

A

second-order reaction

24
Q

in the case of multiple reaction steps, in what step will the rate depend?

slow step or fast step?

A

slow step; the rxn rate will always depend sa slow step

25
Q

in a rxn, what do you call something that is consumed first then produced later on as a final product?

first appears as a reactant then as a product

A

catalyst

26
Q

in a rxn, what do you call something that is produced first then is consumed later on?

first appears as a product then as a reactant

A

intermediate

27
Q

what do you call the time it takes for a conc. of a reactant to decrease by half of its original amount?

time it takes for half of the reactant to be converted to product

A

half-life

28
Q

half-life formula for zero-order reaction

A

t1/2 = [A]i/2k

29
Q

half-life formula for first-order reaction

A

t1/2 = ln2/k

30
Q

half-life formula for second-order reaction

A

1/k[A]i

31
Q

T or F?

a half-life of a first-order reaction depends on initial concentration of a reactant

A

False; given the formula ln2/k, a first-order reaction does not depend on the initial conc. of a reactant

only first & second-order rxns are dependent on initial conc. (reactant)

32
Q

is half-life dependent on the rate constant for all reaction orders?

yes or no

A

yes; also, since rate constant k is found on the denominator of every formula for half-life, ↑K ↓t1/2

33
Q

rate constant k is dependent on where?

A

activation energy and temperature

34
Q

Integrated Rate Law formula for 0-order rxns

A

[A]f = -kt + [A]i

notice: k is negative, therefore slope is negative (➘)

35
Q

Integrated Rate Law formula for 1st-order rxns

A

ln[A]f = -kt + ln[A]i

notice: k is negative, therefore slope is negative (➘)

36
Q

Integrated Rate Law formula for 2nd-order rxns

A

1/[A]f = kt + 1/[A]i

notice: k is positive, therefore slope is positive (➚)

37
Q

↑ or ↓ rxn rate?

increase in temp

A

↑ rxn rate?

↑temp = ↑kinetic energy = ↑collision = ↑rxn rate

38
Q

enumerate arrhenius equation

(be familiar lang daw but no solving regarding this (hopefully))

A

ln(k) = -Ea/RT + ln(A)
or
k = Ae-Ea/RT
wherein: k = rate constant, A = collision frequency, -Ea = activation energy, R = gas constant (8.314 kJ/mol), T = abs temp, e = euler’s number

39
Q

what do you call the species not directly involved in a rxn, but speeds it up?

A

catalyst

40
Q

what increases the rate by lowering activation energy of the rxn by providing alternative pathways for the rxn?

A

catalyst

41
Q

there are 3 types of catalysts, what are they?

A
  1. heterogenous
  2. homogenous
  3. enzyme
42
Q

type of catalyst wherein the catalyst and reactants are of different phases

A

heterogenous catalyst

43
Q

type of catalyst wherein catalysts and reactants are of the same phase

faster since they r in the same phase

A

homogenous catalyst

44
Q

this type of catalyst involves enzymes that have active sites that specifically bind to substrates

A

enzyme

ANACHEM (4 decks)

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