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Chemistry 132 > Kinetics > Flashcards

Kinetics Flashcards

1
Q

What is the reaction rate?

A

The speed of a chemical reaction, used to measure how fast the reaction make products or uses reactants

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2
Q

What is rate?

A

How much a quantity changes in a given period of time

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3
Q

What is the average rate?

A

The change in measured concentrations over any particular time period

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4
Q

What is the instantaneous rate?

A

The change in [] over one specific time period

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5
Q

What are three common techniques used to monitor a reaction mixture?

A

Polarimetry, spectroscopy, and pressure measurement

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6
Q

What is rate law?

A

An equation relating concentration of reactants to rate when the reverse reaction is negligible

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7
Q

What is the order of the reaction?

A

The sum of the exponents on the reactants

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8
Q

If a reaction is zero order…

A

Doubling [a] will have no effect on the reaction rate

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9
Q

If a reaction is 1st order…

A

Doubling [a] will double the rate of the reaction, therefore it is directly proportional to the reactant [].

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10
Q

If a reaction is 2nd order…

A

Doubling [a] will quadruple the rate of the reaction because rate is directly proportional to the square of the reactant concentration

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11
Q

For a particular reaction in which A → products, a doubling of the concentration of A causes the reaction rate to double. What is the order of the reaction?

A

1st order

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12
Q

For a reaction

rate = k[A]m[B]n

what will the overall order be?

A

m+n

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13
Q

What are the units referring to each one of the reaction orders?

A

zero order = M/s

first order = 1/s or s-1

second order = 1/M.s or M-1s-1

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14
Q

In a forward reaction the concentration of the reactants is ___________ and of the products is ____________

A

Decreasing, increasing

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15
Q

In a graph of [] over time, the rate can be determined if ___________ by applying the ____________ of ___.

A

The [] of a substance is known at two distinct points in the reaction, by applying the slope formula of delta y/delta x.

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16
Q

The average rate is the more time specific one.

A

False, it is the instantaneous rate.

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17
Q

Reaction rate can be determined by the balanced reaction alone.

A

False, it cannot be determined by the balanced chemical equation alone.

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18
Q

What is the rate formula of a reaction?

A

Rate = k[A]m[B]n

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19
Q

Which formula can be used to solve for the constant “k”?

A

k = rate/[A]m

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20
Q

What is the integrated rate law?

A

It’s what identifies the relationship of the [] reactants vs time

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21
Q

What is the half-life of a reaction?

A

It is the time required for the concentration of a reactant to fall to 1/2 of its initial value.

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22
Q

What if the reaction mechanism?

A

A series of individual chemical steps by which an overall chemical reaction occurs.

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23
Q

At the beginning of the reaction, the [] of the product is always:

A

Zero

24
Q

The rate of a a chemical reaction speeds up as the reactants form products.

A

False, it slows down

25
Q

The rate law is determine by the coefficients of the balanced equation

A

False

26
Q

If the units of “k” were M/s, we are able to determine that the reaction is:

A

Zero order

27
Q

If the units of “k” were 1/M s, we would be able to determine that the reaction is:

A

Second order

28
Q

If we collect concentration and rate data that shows the rate remains the same with concentration changes, we can determine that the reaction is:

A

Zero order

29
Q

How do you selected which integrated rate law equation to use?

A

It is based upon the reaction order

30
Q

What is the general concept of Kinetics?

A

rate = -Δ[reactant]/ΔT = Δ[product]/ΔT

31
Q

For a particular reaction in which A → products, a doubling of the concentration of A causes the reaction rate to double. What is the order of the reaction?

A

1st order

32
Q

What does the slope (or curve) indicate in an integrated rate law graph?

A

The rate order

33
Q

How can we define dynamic equilibrium?

A

The rates of the forward and reverse reactions are equal and opposite

34
Q

Once equilibrium is stablished, the [] of the reactant and products double.

A

False, once they reach equilibrium the [] does not change

35
Q

What does it mean if K >> 1?

A

That the reaction favors product formation at equilibrium

36
Q

What does it mean if K << 1

A

That the reaction favors reactant formation at equilibrium

37
Q

What does it mean if K = 1?

A

That the neither product is favored at equilibrium and reaction proceeds to midway point

38
Q

What is the term for when rates of the forward and reverse reactions occur at the same rate?

A

Dynamic equilibrium

39
Q

K is not the result of the concentrations of the reactants and the products.

A

False, K is the result of the concentrations of the reactants and the products.

40
Q

The _________ of a reaction is the time required for the concentration of a reactant to fall to 1/2 of its initial value

A

Half-life

41
Q

What is the series of individual chemical steps by which an overall chemical reaction occurs?

A

Reaction Mechanism

42
Q

What is an elementary step?

A

A step that cannot be broken down into simpler steps

43
Q

What are the two requirements for a reaction mechanism?

A

The steps must sum to the overall reaction and the mechanism must predict an experimentally observed rate law

44
Q

What are molecules that can be canceled in a reaction mechanism?

A

Reaction intermeadiates (similar to spectator ions)

45
Q

The rate determining step is much faster than the others.

A

False, it is much slower than the others

46
Q

What is the reactio quotient (Qc)?

A

The ratio at any point in the reaction of the [] of the products raised to their stoichiometric coefficients divided by the [] of the reactants raised to their stoichiometric coefficients.

47
Q

What happens if Q < K?

A

The reaction goes to the right, towards the products

48
Q

What happens if Q> K?

A

The reaction goes to the left, towards the reactants

49
Q

What happens if Q = K?

A

The reaction is at equilibrium

50
Q

If your reaction reads:

2CO(g) CO2(g) + C(s)

What will your equilibrium equation be?

A

K = [CO2]/[CO]2

Because solids are not included in this type of reaction

51
Q

If your reaction reads:

CO2 (g) + H2O (l) H+(aq) + HCO3-(aq)

What will the equilibrium constant be?

A

K = [H+][HCO3-]/[CO2]

52
Q

This is straight forward. What types of substances would not be included in writing an equilibrium constant expression?

A

Solids and liquids

53
Q

When the reaction is reversed, the new K is the _____ of the original.

A

Inverse

54
Q

When the reaction is mulitiplied by a factor, the new K is the “original K” rasied to the power of the factor.

A

true

55
Q

When is it more likely for the x is small rule to be applied?

A

The x is small approximation is most likely to apply to a reaction with a small equilibrium constant and an initial concentration of reactant that is not too small

56
Q

Kc’s unit is grams

A

False, Kc is unitless but based upon concentration, is is measured in M

57
Q
A

Chemistry 132 (10 decks)

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