Unit 3.5 - Chemical Kinetics Flashcards
1
Q
Equation for the rate of a reaction
A
Rate of reaction = change in concentration/unit time
2
Q
Unit of rate if measuring change in concentration over time
A
moldm-3s-1
3
Q
Unit of rate if measuring change in volume over time
A
cms-1
4
Q
Unit of rate if measuring change in mass over time
A
gs-1
5
Q
Relationship between concentration and rate
A
Directly proportional
6
Q
What does it mean that concentration is directly proportional to rate?
A
Double concentration = double rate
7
Q
Which word do we always use when explaining rates
A
Time
8
Q
How do we measure the rate of reaction for a change in concentration of reagent or product
A
By kinetic experiments
9
Q
The change in concentration of what do we measure for the rate of a reaction?
A
Concentration of reagents or reactants
10
Q
What’s the problem with measuring the rate of reaction through the change in concentration and what is done therefore?
A
Not always easy to follow the change in concentration
Usually another property that changes during the reaction is measured
11
Q
How can we measure the rate of reaction at any instant in a reaction?
A
If continuous results are recorded, or many results over time, a graph is drawn
Th rate at any instant is measured using a tangent and a gradient at that point
12
Q
What do we do to calculate the initial rate of a reaction?
A
Tangent at time = 0
13
Q
How do we calculate the instantaneous rate of a reaction?
A
Tangent at that specific time and gradient
14
Q
When is the rate of a reaction highest?
A
At the start of the reaction
15
Q
Why is the rate of a reaction highest at the start of the reaction?
A
This is when there are the most reactants available for collision
16
Q
List the things that he rate of a reaction is dependent on
A
Concentration
Pressure (for gas)
Temperature
Particle size
Catalysts
Light (sometimes)
17
Q
What is the state that an element has to be in for it to be affected by pressure changes?
A
Gaseous
18
Q
What does increasing the concentration or pressure (for a gas) do to the rate of reaction and why?
A
Increases the rate
Less distance between molecules in a given volume = increased number of collisions per unit time
19
Q
What does a different particle size do to the rate of reaction? Explain
A
Smaller = increased rate
Increased surface area = closer together = more collisions per unit time
20
Q
How do we measure the rate of a reaction?
A
We need to work out how much reactant has been used up or how much product has been produced
21
Q
What properties can change with time that we can use to measure the rate of reaction?
A
Concentration of reactants or products
Mass of reactant
Volume or pressure of gas produced
pH
Colour change (or other electromagnetic absorption)
22
Q
How do we work out the means of following a reaction?
A
Study the equation
23
Q
Means of following this reaction:
CaCO3 + 2HCl —> CaCl2 + H2O + CO2
A
- Gas syringe to measure the change in volume over time
- Measure change in mass over time with scales (CO2 is a heavy gas)
24
Q
What property about CO2 makes it useful for following the rate of a reaction? Explain
A
CO2 is a heavy gas
Can measure the change in mass over time with scales to measure the rate of the reaction
25
Means of following this reaction:
CH3CO2C2H5 + H2O —> CH3COOH + C2H5OH
1. Measure change in pH over time (ethanoic acid is involved)
2. Sampling and quenching
26
Means of following this reaction:
CH3COCH3 + I2 —> CH3COCH2 + HI
Measure change in colour over time using a colorimeter
(Brown solution of I2 disappears during the reaction)
27
Describe I2
Brown solution
28
Means of following this reaction:
2KI + H2O2 + 2H+ —> I2 + 2H2O
1. Monitor change in pH over time
2. Iodine-clock reaction - measure change in colour over time using a colorimeter
29
Example of a spectroscopic method to follow the rate of a reaction
NMR has been used to study the rates at which drugs act within the body
30
What type of method is using NMR to study the rate of a reaction?
Spectroscopic
31
When is the iodine-clock technique used to measure the rate of reaction?
In a reaction where iodine is produced
32
Give a description of the theory behind the iodine-clock reaction
Iodine ions can be oxidised to iodine at a measurable rate
Iodine gives a strongly coloured blue/black complex with starch solution
If a given amount of thiosulfate ion (with which iodine reacts very rapidly with to reform iodide ions) is added, the solution will be colourless until enough iodine has been formed to react with all of the thiosulfate
The time taken for this to occur acts like a clock to measure the rate of iodide ions being oxidised
33
What are iodide ions oxidised to at a measurable rate?
Iodine
34
In what solution does iodine give a strongly coloured blue/black complex?
Starch solution
35
Colour of iodine in starch
Blue/black
36
Iodine indicator
Starch
37
What does iodine do with thiosulfate ions?
Reforms iodide ions
38
When is the solution colourless during the iodine clock reaction?
When the iodine is reacting rapidly with the thiosulfate ions to reform iodide ions - it’s colourless until enough iodine has been formed to react with all of the thiosulfate
39
The rate of what is essentially being measured during the iodine-clock reaction?
The rate of iodide ions being oxidised
40
When does the indicator remain colourless during the iodine clock reaction?
When the thiosulfate reacts with the iodine, the indicator remains colourless
41
At which point does the iodine in the reaction mixture and the starch turn blue black during the iodine clock reaction?
The instant the last thiosulfate ion has reacted, there is iodine in the reaction mixture and the starch turns blue/black
42
Thiosulfate ion
S2O32-
43
How could reaction rates be compared using the iodine clock reaction?
If the amount of thiosulfate is kept constant, can compare the times taken to change colour
44
Suitable example of the iodine clock reaction
Oxidising iodide ions by hydrogen peroxide in acid solution
45
Equation for oxidising iodine ions by hydrogen peroxide in acid solution
H2O2 (aq) + 2H+ (aq) + 2I- (aq) —> 2H2O (l) + I2 (aq)
46
Equation for iodine reforming iodide ions with thiosulfate ions
I2 (aq) + 2s2O32- (aq) —> 2I- (aq) + S4O62- (aq)
47
Why is measuring the time taken to produce excess iodine in the iodine clock reaction only an approximation for the rate as the reaction proceeds?
The reaction is faster at first (higher concentration of reactant)
The average rate is measured
48
When is a reaction fastest and why?
At the start
Higher concentration of reactant
49
What gives a measure of the initial rate of reaction in the iodide clock experiment?
The time taken from mixing the reactant to the formation of the dark blue starch solution
50
What does the time taken from mixing the reactant to the formation of the dark blue starch solution in the iodine clock reaction give a measure of?
The *initial* rate of reaction
51
Initial rate equation
Initial rate ∝ 1/t
52
What is proportional to the reciprocal of time (1/t)?
*initial* rate
53
When does the beginning of the concentration-time curve approximate to a straight line in the iodine clock reaction?
If the amount of sodium thiosulfate used is small and is equivalent to m moldm^3 of iodine
54
Describe the beginning of the concentration time curve of a concentration of iodine against time graph
Straight line
55
How can we measure the rate of reaction of the isomerisation of cyclopropane to propane?
Can measure concentration over time using gas chromatography at a constant temperature
56
Under which condition must gas chromatography be done?
Constant temperature
57
Sampling
A process involving removing small samples of the reaction mixture at regular time intervals
58
Quenching
Where samples are placed in ice water to lower the concentration of the reactants and to stop the reaction continuing
59
How can the samples be tested after sampling and quenching?
Using other techniques like titration
60
What is sampling and quenching used to measure?
Changes in concentration
61
Why do we use ice water when sampling and quenching?
Cools the sample
Slows down the motion of particles (significantly - don’t actually stop completely)
Can monitor the exact concentrations at that moment in time
62
What can we titrate CH3CO2C2H5 with and what is the indicator?
NaOH
Methyl orange
63
What happens to the concentration of the product during the sampling and quenching method?
Concentration increases throughout the reaction
Starts to flatline when the reaction is stopping
64
What do we plot on a graph after sampling and quenching?
Concentration against time
65
What is the ratio between the moles of NaOH (titrant) and ethanoic acid produced during a sampling and quenching reaction example?
1:1
66
Advantages of quenching
Accurate
Easy to perform
No need for sophisticated equipment
67
Disadvantages of quenching
Laborious process (involves 5 titrations)
68
Equation for the reaction between 1-bromobutane and sodium hydroxide
CH3CH2CH2CH2Br + OH- —> CHCH2CH2CH2OH + Br-
69
What type of reaction is the reaction between 1-bromobutane and sodium hydroxide?
Nucleophillic substitution reaction
70
What does the fact that rate ∝ [OH-] in a reaction mean?
The rate of reaction depends on the concentration of OH-
If the concentration of OH- were doubled, the rate of reaction would double
71
Decomposition of hydrogen peroxide equation
2H2O2 —> 2H2O + O2
72
What is rate proportional to in the decomposition of hydrogen perioxide?
The concentration of the hydrogen peroxide
73
How can we form a rate equation?
By changing the proportionality sign for an equal sign and adding k, the rate constant
74
Rate equation for the decomposition of hydrogen peroxide
Rate = k[H2O2]
75
What does a rate equation give?
The dependence of the rate of the reaction on the concentration of the species in the rate equation
76
What is k in rate equations?
The rate constant
77
What is k (in rate equations) unique for?
Every set of chemical reactions
78
What is k (rate constant) independent of?
Concentration and time
79
What is the only thing that affects the value of k (rate constant)?
Temperature
80
What does the value of k (rate constant) depend on?
The reaction being studied
The temperature
81
What odes a higher k value mean?
Faster reaction
82
Example of a reaction with a high k value
Fireworks
83
Example of a reaction with a low k value
Rusting
84
How can the rate equations deduced?
From kinetic experiments
85
How can rate equations *not* be deduced?
From chemical equations
86
What does it mean if a reaction is first order with respect to something?
The rate of reaction depends on the concentration of that thing to the power one
87
What is the reaction 2H2O2 —> 2H2O + O2’s order with respect to hydrogen peroxide?
First order
88
How is the order of reaction found?
By experiment
89
How is the order of a reaction *not* found?
By chemical equations
90
General rate equation for a reaction whose rate depends on the concentration of reagents A and B
Rate = k[A]^x[B]^y
91
In Rate = k[A]^x[B]^y
What is x?
The order of the reaction with respect to A
92
In Rate = k[A]^x[B]^y
What is y?
The order of the reaction with respect to B
93
Order of reaction
The power to which the concentration term must be raised to fit the rate equation - is the exponent
94
What values do the order of a reaction usually have?
0, 1 or 2 for each reagent
95
What does it mean if something has an order of zero?
It doesn’t affect the rate
96
How do we work out the overall order of a reaction?
Is equal to the sum of the powers of the concentration terms in the rate equation
97
Can the overall rate of a reaction be more than 2?
Yes
98
The concentrations of what do we show in a rate equation?
The reactants
99
How do we know if something is to the power of one in orders of reaction?
If something is to the power of 1, it isn’t usually shown
100
Can the rate equation be deduced from the chemical equation?
No
101
How can we find orders?
Perform experiments
102
Why can’t we deduce rate equations from chemical equations?
Chemical reactions may be a one step process or may involve a number of steps
103
Rate determining step
The slowest step in a reaction
104
What is the slowest step of a reaction known as?
The rate determining step
105
Which step determines the rate equation? Explain
Chemical reactions may be a one step process or may involve a number of steps
In any reaction, one step will e slower than all the other steps and it is this step which determines the rate equation
106
How do you determine the rate of any clock reaction?
Measure time taken for the colour change to occur
rate = 1/time
107
Effect of an increased temperature on a rate equation + explain
No effect
Rate equation is independent on temperature
108
Catalyst of the decomposition of ammonia
Platinum
109
Decomposition of ammonia equation
2NH3 —> N2 + 3H2
110
If the decomposition of ammonia is zero order with respect to ammonia, what does this mean?
The rate is independent on the concentration of ammonia
111
Rate equation for zeroth order reactions
Rate = k
112
Units of k in zeroth order reactions
moldm^-3s^-1
113
What happens to the rate of reaction when the concentration of ammonia is doubled in the decomposition of ammonia? Why?
The rate of reaction is unchanged
The reaction is zero order with respect to the ammonia
114
What is the relationship between the concentration of the reagent and the rate of reaction in zeroth order reactions and what does this mean?
The rate of reaction is independent of the concentration of the reagent - rate stays the same as the concentration changes
115
Describe the line on a rate v.s concentration graph for a zeroth order reaction
Horizontal straight line
116
Give 2 examples of first order reactions
Decomposition reactions
Radioactive decay
117
Rate equation for first order reactions (e.g - decomposition of dinitrogen perioxide)
Rate = k[N2O5]
118
What order is the dinitrogen perioxide in its decomposition reaction?
First order
119
Units of k in first order reactions
s^-1
120
How do we know that the units are s^-1 with first order reactions?
k = rate/[N2O5] = moldm-3s-1/moldm-3 = s-1
121
Relationship between rate and concentration in first order reactions
Directly proportional
122
What happens when the concentrate of dinitrogen perioxide is doubled in its decomposition reaction and why?
Reaction is first order with respect to dinitrogen peroxide
As concentration is doubled, rate is doubled
123
Decomposition of ninitrogen peroxide
2N2O5 —> 4NO2 + O2
124
Explain the graph of rate v.s concentration for first order reactions
Straight line through the origin (as rate is zero when concentration is zero)
125
Why is the line through zero on rate v.s concentration graphs?
Rate is zero when concentration is zero
126
Half life of first order reactions
Constant
127
2 ways to show that a reaction is first order
1. Tangent at 0.1 and tangent at 0.05, and compare rates
2. Work out the half life and check that it’s constant
128
Decomposition of nitrogen dioxide
2NO2 —> 2NO + O2
129
What order is the decomposition of nitrogen dioxide?
3rd order with respect to the nitrogen dioxide
130
Rate equation for 2nd order reactions (e.g - the decomposition of nitrogen dioxide)
Rate = k[NO2]^2
131
Units of k in second order reactions
mol-1dm3s-1
132
Why is the unit of k mol-1dm3s-1 in 2nd order reactions?
k = rate/concentration
k = moldm-3s-1/(moldm-3)2
= 1/moldm-3 x s-1
=mol-1dm3s-1
133
What is rate proportional to in second order reactions?
Concentration^2
134
In the decomposition of nitrogen dioxide (a 2nd order reaction), if the concentration of nitrogen dioxide is doubled, what happens to the rate of reaction?
Is quadrupled, increased fourfold
135
Describe the curve on a concentration v.s rate graph of a 2nd order reaction
A curved line starting at the origin as rate is zero when concentration is zero
136
What will happen to the rate of a first order reaction if the concentration is increased by a factor of 3?
The rate will increase by a factor of 3 too
137
What happens to the rate of a 2nd order reaction if the concentration is increased by a factor of 3? Explain
3^2
= increases by a factor of 9
138
Describe the half life of second order reactions
Isn’t constant
Half life increases as the concentration decreases (exponential decay curve)
139
Describe the curve of rate v.s concentration for a second order reaction
Exponential decay curve
140
If we’re asked to work out he order of reaction with respect to a specific element, what do we need to do?
Choose the experiments where the concentration of the other reactant is constant
141
Equation to work out k (and where does this come from?)
k = rate/concentration
Rearranged rate = k[concentration]
142
What do we need to do with a rate-based question where we’re given pH values?
Should work out [H+]
143
Equation to work out [H+]
[H+] = 10^pH
144
How many steps do chemical reactions involve?
May involve one stop or a number of steps
145
Which step determines the rate equation?
The slowest step - the rate determining step
146
What does the rate determining step determine?
The rate equation
147
How can we identify the rate determining step of a chemical reaction?
It’s the slowest step
148
What does the rate determining step tell us?
Which particles are reacting in the reaction
149
Which species specifically is a rate dependent on?
The species in the rate determining step
150
What is dependent on the species in the rate determining step?
The rate
151
What information do we obtain about the rate determining step?
According to collision theory:
1.) the reacting particles must collide
2.) the particles must have sufficient energy for reaction (the activation energy)
152
What must colliding particles have in order to reacti?
Sufficient energy - the activation energy
153
How much energy is sufficient for a reaction to occur?
An amount of energy equivalent to the activation energy of a reaction
154
If something is first order with respect to something, what does it mean?
That only this element is involved in the rate determining step
155
How do we know if only one element is involved in a rate determining step?
If the rate equation shows only that element with first order respect to it
156
What does a rate equation tell us (relating to the rate determining step)?
How many particles must collide in the rate determining step
157
How many particles collide in 2nd order reactions?
2
158
How many particles collide in 3rd order reactions?
3
159
How many particles in the rate determining step of first order reactions?
1
160
When is there only 1 particle in the rate determining step?
1st order reactions
161
How many particles in the rate determining step for 1st order reactions?
1
162
Write a possible mechanism by which explains the rate equation of
Rate = k[A]
For the reaction
A + B —> C + D
A —> A* slow
A* + B —> C + D fast
163
What does the rate determining step of a reaction determine?
The rate of a reaction
164
When is something not involved in the rate equation?
If it’s not involved in the rate determining step
165
What is an element also not included in if it’s not included in the rate determining step?
The rate equation
166
What does a species have to be present for a reaction to be dependent on it?
in the rate equation
167
What will the rate determining step and the rate equation include for a one-step process?
Both reagents
168
When will the rate determining step and the rate equation include both reagents?
One step processes
169
Equation for the hydrolysis of 1-bromobutane by aqueous sodium hydroxide
CH3CH2CH2CH2Br + OH- —> CH3CH2CH2CH2OH + Br-
170
What type of process is the hydrolysis of 1-bromobutane by aqueous sodium hydroxide?
One step reaction
171
Give the rate equation for the following one step reaction
CH3CH2CH2CH2Br + OH- —> CH3CH2CH2CH2OH + Br-
Rate = k[CH3(CH2)3Br][OH-]
172
When can the rate equation be deduced from a single step?
If that step is a rate determining step
173
If the single step of a one step reaction is the rate determining step, what an be deduced?
The rate equation
174
What can’t be determined from a chemical equation?
Rate equations
175
What can’t rate equations be deduced from?
Chemical equations
176
If the rate equation is
Rate = k[CH3COOCH3][H+]^2
What are the reactants of the rate determining step?
CH3COOCH3 + 2H+ —> products
177
Is it possible to identify conclusively the product of the rate determining step in every case?
No
178
What can we do as we can’t always conclusively identify the products of a rate-determining step?
Can suggest products
179
What must we do when suggesting products for a rate determining step?
Make sure that the equation balances just like any other
180
Suggest products for the following rate determining step
C3H7I + Br- ——> C3H7Br + I-
181
What must combine to form the overall equation of a reaction?
All of the steps in the mechanism, including the rate determining step
182
If a rate determining step has the following reactants:
CH3COOCH3 + 2H+ —> products
What will the rate equation be?
Rate = k[CH3COOCH3][H+]^2
183
How can we prove or disprove a reaction mechanism?
Can use the information derived from the kinetics of a reaction
184
What can we prove or disprove from the kinetics of a reaction?
A reaction mechanism
185
How can we actually work out what the reactants are for a rate determining step?
By looking at the kinetics of a reaction
186
What can we work out using kinetics?
The reactants for the rate determining step of a reaction
187
How do we know if a proposed mechanism for a reaction is correct?
If our proposed mechanism does not have a step with the reactants for the rate determining step, it cannot be the correct mechanism
188
Which reactants is it vital that a mechanism has in it for it to be correct?
The reactants for the rate determining step
189
What do the coefficients in a chemical reaction show?
All of the reactants in all steps, including those not in the rate equation
190
Which species do orders show?
Only those present in the rate determining step
191
Explain why the orders of reaction in a rate equation do not always correspond to the coefficients in a chemical equation
Coefficients —> all reactants in all steps, including those not in the rate equation
Orders —> species present in the rate determining step
192
When considering the reaction
BrO3- + 6H+ + 6Br- —> 3Br2 + 3H2O
With rate equation
Rate = k[BrO3-][Br-][H+}^2
How can you tell that this reaction involves more than one step?
Coefficients of equation don’t match up with the orders of the rate equation
13 species in chemical equation (LHS), 4 in rate equation
193
Which side of a reaction do we look at the coefficients to compare to them with the orders of the rate equation?
Left
194
What’s the only thing we need to remember to consider when writing out possible mechanisms for reactions using rate equations?
Make sure that the equation balances
195
Consider the following reaction:
NO2 + CO —> NO + CO2
Rate equation:
Rate = k[NO2]^2
Suggest a likely rate determining step for the reaction and hence suggest a two-step mechanism for this reaction. Explain.
NO2 + NO2 —> NO + NO3 slow step (rate determining)
NO3 + CO—> NO + CO2
or
NO2 + NO2 —> intermediates
Intermediates —> NO + CO2
We needed to make sure that the reactants had 2 NO2’s since it’s squared in the rate equation
196
If something is squared in a rate equation, what do we need to ensure we do for the rate determining step reaction?
Include it twice
197
What does this rate equation show?
Rate = k[A][B]^2
It shows how the rate is affected by the concentrations of the reactants [A] and [B]
198
What does the rate constant actually show in a rate equation?
How other variables other than the concentration of the reactants affect the rate
199
What effects the value of k (rate constant)?
Change in temperature
Addition of catalyst
200
How is k expressed mathematically?
Using the Arrhenius equation
201
What is the Arrhenius equation for?
Expressing k mathematically
202
Arrhenius equation
k = Ae^-(Ea/RT)
203
What does the whole of e^-(Ea/RT) represent in the Arrhenius equation?
The fraction of the molecules in a gas which have energies equal to or greater than the activation energy at a stated temperature
204
What does the frequency factor A in the Arrhenius equation include?
Factors like the frequency of collisions and their orientation
205
What includes factors like the frequency of collisions and their orientations in the Arrhenius equation?
A, the frequency factor
206
What does A, the frequency factor, vary with and to what extent?
It varies slightly with temperature, although not much and is taken as constant across small temperature ranges
207
When is A, the frequency factor, taken as constant?
Across small temperature ranges
208
What is the only thing that A, the frequency factor, is effected by?
Large temperature changes
209
Name for this equation
k = Ae^-(Ea/RT)
The Arrhenius equation
210
Units of k (rate constant)
Depends on the overall order
211
Units of T in Arrhenius equation
K
212
R in the Arrhenius equation
Gas constant
213
Ea in Arrhenius equation and unit
Activation energy
Jmol-1
214
e in Arrhenius equation
Mathematical constant
215
How do we obtain “e” for the Arrhenius equation?
Shift ln
216
A in Arrhenius equation and units
Frequency factor
No units
217
What is the frequency factor related to?
The frequency of collisions between particles
218
When do we treat the frequency factor as a constant?
Over a limited range of temperatures
219
When can a frequency factor vary?
If temperatures change significantly
220
What type of term is ln?
Logarithmic
(Loge not log10)
221
Write the Arrhenius equation in logarithmic terms
ln A = ln k + Ea/RT
222
What is the only bit we put in brackets when putting in Arrhenius equation calculations into a calculator?
Multiplying R and T
223
What do we do with the R and T when typing in Arrhenius equation calculations into a calculator?
Use brackets
224
How would we rearrange the Arrhenius equation to find temperature?
T = Ea/(lnA-lnK) x R
225
What happen when we take the natural log when rearranging the Arrhenius equation?
It cancels out e
226
How do we rearrange the Arrhenius equation to work out the activation energy?
Ea = RT(lnA - lnK)
227
How do we rearrange the Arrhenius equation to find A?
A = k/e^-Ea/RT
228
How do we use a graphical method with the Arrhenius equation?
Convert and re-arrange the equation int the straight line formula, y = mx + c
229
Put the Arrhenius equation into the straight line formula and explain what each feature now means
ln (k) = (Ea/R) 1/T + ln A
Y = mx + c
Y-axis = plot ln K
X-axis = plot 1/T
Gradient (m) = gives - (Ea/R)
Y-intercept (c) = gives ln A
230
How do we work out the activation energy of a reaction using the Arrhenius equation in graphical form? Explain
Arrhenius equation in the equation of a straight line
ln (k) = (Ea/R) 1/T + ln A
y = mx + c
Gradient = Ea/R
So Ea must be gradient x R
231
Do we use the big numbers from the equation when working out rate constants?
No - ignore them
232
Another word for frequency factor in the Arrhenius equation
Arrhenius constant
233
Why do we need to work out the concentration of hydrogen ions if we’re given pH in a determination of the rate equation question?
To work out whether [H+] needs to be included in the rate equation
234
Order of a reaction
The power to which the concentration is raised
