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CHM135 > Unit 6 Kinetics > Flashcards

Unit 6 Kinetics Flashcards

1
Q

how can rates of reactions be monitored?

A

finding the change in either the reactants or products

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1
Q

what is the formula to find the rate of production? what is the rate of production of b?

A

rate=change in concentration over the change in time

e.g rate of B= -(change of concentration of B)/the change in time

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2
Q

what is the rate of consumption formula of A?

A

rate of consumption of A= -change in concentration of A/t2-t1

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3
Q

what is the sign for the average rate of consumption?why?

A

negative because the reactants are decreasing as a function of time

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4
Q

what is the rate law formula defintion?

A

an equation showing how the reaction rate depends on the concentration (moles) of each reactant

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5
Q

what is an example equation of a rate law? what do the numbers to the left and right of the concentrations represent?

A

rate law=k[A]^m[B]^n

[A] and [B] are the concentrations in M

m is the exponent for A

n is the exponent for B

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6
Q

do the exponents equal the coefficients of each concentration?

A

no

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7
Q

how must the reaction law be determined?

A

experimentally

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8
Q

units of rate

A

M/s

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9
Q

What is the reaction rate?

A

a measure of how fast the reaction is going

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10
Q

what are integrated rate laws?

A

mathematical functions that give the concentrations over the change in time

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11
Q

what is half-life?

A

the time it takes the reactants to reach 50% of its original values

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12
Q

what do reaction mechanisms do?

A

connect microscopic molecular processes to the overall rate

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12
Q

what does Arrhenius equations decribe?

A

describes how the rate changes with temperature

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13
Q

what can kinetics reveal about a reaction

A

how a reaction occurs

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14
Q

what is the graphical method of the rate law? what does the shape of the line reveal

A

monitor the reaction over time

plot the data

shape of the graph line reveals the order of the reaction

15
Q

what is the zeroth order formula? does rate depend on concentration?

A

Rate=k

Rate does not depend on concentration because there is no concentration

16
Q

What are the conditions of the zeroth order in terms of the graph?

A

If the graph is linear and going downwards, the reaction is zero order

17
Q

What is the equation of a straight line for zeroth order (integrated rate law)?

A

[At]=-kt+[A]o

18
Q

What is the first-order formula for rates? Does rate depend on concentration?

A

Rate=k[A]

Rate does depend on the concentration

19
Q

What is the second order formula for Rate?

A

Rate=k[A]^2

20
Q

What happens to the concentration when you double the rate of a second order reaction?

A
  1. Apply the exponent to the rate side with the base 2

The reaction will quadruple

21
Q

What does the half-life depend on? what happens to the half-life in terms of amount?

A

Dependent on intial concentration

Gets shorter over the course of the reaction

22
Q

what is the Integrated Rate law for first-order reactions?

A

Ln[A]=-kt+1/[Ao]

23
Q

what is the Integrated Rate law for second-order reactions?

A

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

24
Q

What is the equation for half-life for the first-order reaction?

A

t1/2=ln2/k

25
Q

What does it mean if the graph is linear and goes down

A

The reaction is first order

26
Q

What does it mean if the graph is linear and going up?

A

The reaction is second order

27
Q

What is the half life formula of the second order reaction

A

t1/2=1/k[A]o

28
Q

What are the conditions of the half-life second-order reaction?

A

t1/2 depends on the intial concentration

t1/2 gets longer over the course of the reaction

29
Q

what is the half-life formula for a zero-order reaction?

A

t1/2=[A]o/2k

CHM135 (15 decks)

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