Font size
S
M
L
XL
Worksheets5.0 Reaction Kinetics
Total questions: 125
Worksheet time: 1hrs 3mins
Name
Class
Date
1.
Rate of reaction
a)
Rate = ([initial concentration] - [final concentration]) ÷ time taken
= ∆ [concentration] ÷ ∆t
b)
Rate = ([final concentration] - [initial concentration]) ÷ time taken
= ∆ [concentration] ÷ ∆t
2.
graph rate of reaction
a)
change of concentration vs time
b)
change of concentration vs temperature
3.
graph of reactant
a)
concentration of reactants decreases with time (senyum)
b)
concentration of reactants increases with time (senyum)
4.
graph of product
a)
concentration of product increases with time
b)
concentration of product decreases with time
5.
instanteneous rates
a)
The RATE OF CHANGE at a particular moment. Same as the value of the derivative at a particular point. For a function, the instantaneous rate of change at a point is the same as the slope of the tangent line. That is, it's the slope of a curve.
b)
The CHANGE OF TEMPERATURE change of temperature at a particular moment. Same as the value of the derivative at a particular point. For a function, the instantaneous rate of change at a point is the same as the slope of the tangent line. That is, it's the slope of a curve.
6.
tangent of concentration/ time graph
a)
to get rate of REACTION at particular moment
b)
to get rate of CONSTANT at particular moment
7.
gradient of a tangent decrease with time
a)
shows rate of reaction DECREASE with time, because concentration of the reactant DECREASE with time.
b)
shows rate of reaction INCREASE with time, because concentration of the reactant INCREASE with time.
8.
initial rate
a)
maximum rate.
rate at time zero
b)
minimum rate.
rate at a particular time
9.
Calculate initial rate
a)
at time = 0
b)
at time when reactant concentration is zero
10.
Calculate rate at time 60s
a)
find tangent of gradient at time 60 sec.
b)
find tangent of gradient at time 0 sec.
11.
negative sign
a)
reactants
b)
product
12.
positive sign
a)
product
b)
reactants
13.
graph of reactant
a)
concentration of reactants decreases with time (senyum)
b)
concentration of product increases with time
14.
graph of product
a)
concentration of product increases with time
b)
concentration of reactants decreases with time (senyum)
15.
rate of dissappearance of reactants
a)
-∆[reactant]/∆t
b)
∆[product]/∆t
16.
rate of appearance/ formation of products
a)
∆[product]/∆t
b)
-∆[reactant]/∆t
17.
rate of dissappearance = rate of appearance
a)
-∆[reactant]/∆t = ∆[product]/∆t
b)
-∆[product]/∆t = ∆[reactant]/∆t
18.
X-> Y
a)
-∆[ X ]/∆t = ∆[ Y ]/∆t
b)
-∆[ Y ]/∆t = ∆[ X ]/∆t
19.
2X -> Y
a)
-∆[ X ]/∆t =2∆[ Y ]/∆t
b)
-∆[ Y ]/∆t =2∆[ X ]/∆t
20.
decomposes
a)
dissappearance
b)
appearance
21.
formation
a)
appearance
b)
dissappearance
22.
the collision theory of Arrhennius
a)
to explain how chemical reactions take place.
b)
to explain how reactants molecules approach one another.
23.
chemical reaction occur when...
a)
collisions between reacting particles
b)
repulsions between reacting particles
24.
ineffective collisions
a)
the reactants molecules approach one another, they experience REPULSIONS between their electron clouds.
Therefore, reactants must have sufficient energy to overcome this repulsions before electron clouds can penetrate one another.
b)
the reactants molecules approach one another, they experience ATTRACTIONS between their electron clouds.
Therefore, reactants must have sufficient energy to overcome this repulsions before electron clouds can penetrate one another.
25.
activation energy, Ea
a)
Minimum energy required
before a reaction can take place
b)
Maximum energy required
before a reaction can take place
26.
activation energy, Ea
a)
minimum energy that must be overcome by reactant molecules before a reaction can take place.
b)
maximum energy that must be overcome by reactant molecules before a reaction can take place.
27.
effective collisions
a)
particle (small fraction) have enough energy to react
b)
Direction of collision should facilitates formation of new bonds.
28.
correct orientation
a)
Direction of collision should facilitates formation of new bonds.
b)
particle (small fraction) have enough energy to react
29.
effect of concentration on the rate of a reaction
a)
Increase concentration of reactants
Increase number of particles per unit volume.
Increase rate of collision.
Increase rate reaction.
b)
Increase concentration of reactants
Decrease number of particles per unit volume.
Decrease rate of collision.
Decrease rate reaction.
30.
effect of pressure on the rate of a reaction. Pressure only affect reaction system containing gases: because the volume occupied by gas depends on the pressure on the gas.
a)
Pressure increase,
Molecules pushed closer to one another.
Causes concentration gas increase.
More collision, increase rate reaction.
b)
Pressure increase,
Molecules pushed far away to one another.
Causes concentration gas decrease.
less collision, decrease rate reaction.
31.
effect of temperature on the rate of a reaction.
a)
increase temperature,
average kinetic energy molecule increases,
more collisions per unit time,
number of molecules having energy equal ot greater than Ea activation energy also increases.
b)
increase temperature,
average kinetic energy molecule decreases,
less collisions per unit time,
number of molecules having energy equal or greater than Ea activation energy decreases.
32.
effect of temperature on the rate of a reaction. Illystrated by Maxwell-Boltzmann distribution curve. rate reaction increase exponentially. Two times of area triangle Ea.
a)
Correct
b)
Incorrect
33.
Biological reactions
a)
involving enzymes
b)
involving catalyst
34.
optimum temperature. Rate reaction increase with temperature until optimum temperature.
Beyond the limit…
a)
rate decreases as enzymes get denatured because protein molecules.
b)
rate increases as enzymes get activated because protein molecules.
35.
Kinetic theory related kinetic energy (K.E) to absolute temperature (T)
a)
K.E of a particle directly proportional to its absolute temperature.
K.E = 1/2 mv²
1/2 mv² = T
v² = T
v..² /v.² = T../ T.
b)
K.E of a particle inversely proportional to its absolute temperature.
K.E = 1/2 mv²
1/2 mv² = T
v² = T
v..² /v.² = T../ T.
36.
Rate equation
a)
Expression of dependence rate reaction on [ ]
b)
k = rate constant.
37.
Rate equation
a)
Power of general equation: aA + bB -> cC + dD
Rate= k[A] ^x [B]^y
xy order of reaction obtain through experiment only. Not same as stoichimetry.
b)
Power of general equation: aA + bB -> cC + dD
Rate= k[A] ^a [B]^b [C] ^c [D]^d
xy order of reaction obtain through experiment only. Not same as stoichimetry.
38.
stoichiometric equation
a)
shows reacting mole ratios of the reactants and products
b)
Expression of dependence rate reaction on [ ]
39.
Order of reaction
a)
power of [reactants] is raised (experimentally determined).
b)
sum of powers of reactants is raised (experimentally determined).
40.
Overall order of reaction
a)
sum of powers of reactants is raised (experimentally determined).
b)
power of [reactants] is raised (experimentally determined).
41.
CO (g) + NO2 (g) -> CO2 (g) + NO (g). if doubling [NO2] increase rate reaction by 2² or 4 times.
if halved, rate would decrease to (½)² or ¼ of its original volume.
a)
second order for NO2
b)
zero order for NO2
42.
CO (g) + NO2 (g) -> CO2 (g) + NO (g). Changing [CO] has no effect on rate but CO must present for reaction occur.
a)
zero order for CO
b)
second order for CO
43.
First order
a)
when [substance] change x times. Rate would change by x¹ times.
b)
when [substance] change x times, rate would change by x² times
44.
Second order
a)
when [substance] change x times, rate would change by x² times
b)
when [substance] change x times. Rate would change by x¹ times.
45.
Zero order
a)
when [substance] change x times, rate would change by x° (which is = 1) times. Rate independent of [substance].
b)
when [substance] change x times. Rate would change by x¹ times.
46.
Arrhenius equation
a)
k = Ae^(-Ea/RT)
b)
kt = Ae^(-Ea/RT)
47.
2 frequency factors
a)
1. Probability (correct orientation)
2. Collision (no. Of collision / time)
b)
1. Probability (correct orientation)
2. Ea
48.
e^(-Ea)/RT
a)
Fraction of particles with energy => Ea.
b)
Fraction of particles with energy <= Ea.
49.
Rate constant increase when...
a)
1. Ea decrease (add catalyst)
2. T increase
b)
1. Ea increase (add catalyst)
2. T increase
50.
The role of catalyst in reactions, Catalyst
a)
Substance increase rate chemical rxn without itself consumed.
b)
Substance increase rate chemical rxn with itself consumed.
51.
The role of catalyst in reactions, Regenerated
a)
Catalyst react with reactant to form intermediate but regenerate at the end. Might change but unchanged chemically at end.
b)
Catalyst react with reactant to form intermediate but regenerate at the end. Might changed chemically at end.
52.
Catalyst alters
a)
1. Rate rxn
2. Mechanism
3. Order
4. Ea
b)
1. Rate rxn
2. Mechanism
3. Ea
53.
Catalyst does not affect
a)
1. Yield
2. Overall stoichiometry
3. ∆H
b)
1. Yield
2. Overall stoichiometry
54.
Rate of reaction & amount of catalyst used.
a)
Directly proportional.
b)
Unchanged
55.
Why use catalyst in small quantity?
a)
Regenerated, small & expensive.
b)
Regenerated & small.
56.
How catalyst action?
a)
Alter rate rxn.
Prepare alternative pathway with lower Ea. So, more particles have enough E to overcome lower Ea, increase no. Of effective collision/time.
b)
Alter rate constant of rxn.
Prepare alternative pathway with higher Ea. So, more particles have enough E to overcome higher Ea, increase no. Of effective collision/time.
57.
Very specific
a)
Catalyst one rxn might not catalyst another.
b)
Catalyst would use as many reaction.
58.
Homogeneous catalyst
a)
Catalyst same physical states as reactant.
b)
Catalyst not same physical states as reactant.
59.
Intermediate product theory
a)
Reaction intermediate. A reaction intermediate or an intermediate is a molecular entity that is formed from the reactants (or preceding intermediates) and reacts further to give the directly observed products of a chemical reaction.
b)
To explain action of heterogeneous catalyst occur only on the surface of a substance.
60.
1889 Svante Arrhenius defined Activation energy, Ea as
a)
the least possible amount of energy (minimum) which is required to start a reaction or the amount of energy available in a chemical system for a reaction to take place.
b)
the maximum possible amount of energy (minimum) which is required to start a reaction or the amount of energy available in a chemical system for a reaction to take place.
61.
Heterogeneous catalyst
a)
Catalyst not same physical states as reactant.
b)
Catalyst same physical states as reactant.
62.
Adsorption theory
a)
To explain action of heterogeneous catalyst occur only on the surface of a substance.
b)
Reaction intermediate. A reaction intermediate or an intermediate is a molecular entity that is formed from the reactants (or preceding intermediates) and reacts further to give the directly observed products of a chemical reaction.
63.
Adsorption
a)
Occur only on the surface of a substance.
b)
Occurs in the body of a substance.
64.
Absorption
a)
Occurs in the body of a substance.
b)
Occur only on the surface of a substance.
65.
important purposes Adsorption and Absorption
a)
1. Brings the reactants closer to one another.
2. Weakens the covalent bonds in reactants molecules.
3. Hold reactant in right orientation for new bonds formed.
b)
1. Brings the reactants closer to one another.
2. Weakens the covalent bonds in reactants molecules.
66.
Desorption
a)
Product released from the Nickel surface providing a new surface for adsorption of the reactants molecules.
b)
Occurs in the body of a substance.
67.
Enzymes, substance that:
a)
1. Catalyse biological reaction in living organism.
2. Protein molecules.
3. Very specific in action.
4. Very sensitive to change of T and pH.
5. Very efficient than inorganic catalyst.
b)
1. Catalyse biological reaction in living organism.
2. Protein molecules.
3. Very specific in action.
4. Very sensitive to change of T and pH.
68.
Enzyme catalase lower the Ea for the decomposition of H2O2 from
a)
85 - 20 kJ mol-1.
b)
85 - 55 kJ mol-1.
69.
Optimum pH for Pepsin
a)
2
b)
9
70.
Optimum pH for Lipase
a)
9
b)
2
71.
Denature
a)
If temperature too high, or
pH too high/ low.
Becomes ineffective.
b)
If temperature too high and too low, or
pH too high/ low.
Becomes ineffective.
72.
Importants
a)
without enzymes, the biological reactions in our body will be too slow to sustain life.
b)
without enzymes, the biological reactions in our body will be too fast to sustain life.
73.
Initial rate of concentration vs time graph
a)
Tangent at rate rxn at time 0, [reactant] is maximum
b)
Tangent at rate rxn at time when product is maximum
74.
How to determine the order of substance
Kalau constant kita boleh abaikan
A= A
B= B
a)
Determine order of A- keep [B] constant, varying [A].
Determine order of B- keep [A] constant, varying [B].
Whatever changes in rates due to A not B vise versa.
b)
Determine order of A- keep [B] constant, varying [B].
Determine order of B- keep [A] constant, varying [A].
Whatever changes in rates due to A not B vise versa.
75.
Rate = k[A]^x[B]^y
a)
Experiment yang sama [reactant] boleh diabaikan. Bahagikan exp nilai rate rxn besar ÷ exp nilai rate rxn kecil = order untuk reactant yang vary.
b)
Experiment yang sama [reactant] boleh diabaikan. Bahagikan exp nilai rate rxn kecil ÷ exp nilai rate rxn besar = order untuk reactant yang vary.
76.
rate constant
a)
k
b)
rate = k [A] [B]²
77.
First order reaction, Half-life
a)
time taken for initial amount ([ ], mass, moles etc) of a reactant to decrease to half its value.
b)
time taken for initial amount ([ ], mass, moles etc) of a product to decrease to half its value.
78.
First order reaction, t1/2
a)
ln2/ k
b)
ln2 x k
79.
Half-life of first order
a)
independent of initial amount of reactant.
b)
dependent of initial amount of reactant.
80.
First half-life for first order reaction
a)
example 1.0M. from 1.0 to 0.5
b)
example 1.0M. from 0.5 to 0.25
81.
Second half-life for first order reaction
a)
example 1.0M. from 0.5 to 0.25
b)
example 1.0M. from 0.25 to 0.125
82.
Third half-life for first order reaction
a)
example 1.0M. from 0.25 to 0.125
b)
example 1.0M. from 0.5 to 0.25
83.
Differential equation of zero order reaction
a)
A-> products
Rate = k[A]°
Or rate = k
-dC/dt = k
-dC = k dt
b)
A-> products
Rate = k[A]¹
-dC/dt = kC
C = [A] at time t
-dC/C = kdt
84.
Differential equation of dirst order reaction
a)
A-> products
Rate = k[A]¹
-dC/dt = kC
C = [A] at time t
-dC/C = kdt
b)
A -> products
Rate = k[A]²
-dC/dt = kC²
-dC/C² = kdt
85.
Differential equation of second order reaction
a)
A -> products
Rate = k[A]²
-dC/dt = kC²
-dC/C² = kdt
b)
A-> products
Rate = k[A]¹
-dC/dt = kC
C = [A] at time t
-dC/C = kdt
86.
Intergrating the equation of zero order reaction
a)
C° to C dC = -° to t (kdt)
C-Co = kt
So, C = - kt + Co
b)
C0 to C (dC/C) = - 0 to t (kt)
ln C - ln Co = -kt
Co = [A] at time 0.
So, ln C = -kt + ln Co
87.
Intergrating the equation first order reaction
a)
C0 to C (dC/C) = - 0 to t (kt)
ln C - ln Co = -kt
Co = [A] at time 0.
So, ln C = -kt + ln Co
b)
C° to C dC = -° to t (kdt)
C-Co = kt
So, C = - kt + Co
88.
Intergrating the equation of second order reaction
a)
Co to C (dC/C²) = - o to t (k dt)
-1/C + 1/Co = -kt
So, 1/C = kt + 1/Co
b)
C0 to C (dC/C) = - 0 to t (kt)
ln C - ln Co = -kt
Co = [A] at time 0.
So, ln C = -kt + ln Co
89.
Graph of second order reaction
a)
1/C vs t give directly proportional straight line with slope = k
b)
1/C vs t give inversely proportional straight line with slope = k
90.
To determine the rate constant of second order reaction
a)
gradient of the graph. 1/[A] ÷ t
b)
gradient of the graph. [A] ÷ t
91.
t½ of zero order reaction
a)
Co/2k
b)
1/kCo
92.
t½ of first order reaction
a)
ln2/k
b)
Co/2k
93.
t½ of second order reaction
a)
1/kCo
b)
ln2/k
94.
Summarises the rate equation in order of zero, first, second order…
a)
Rate= k, k[A], k[A]²
b)
Rate= k[A]², k[A], k
95.
Summarises the Integrated rate equation in order of zero, first, second order…
a)
C= -kt + Co
ln C = -kt + ln Co, lnCo/C = kt,
1/C = kt + 1/Co
b)
1/C = kt + 1/Co,
ln C = -kt + ln Co, lnCo/C = kt,
C= -kt + Co,
96.
Summarises the Half-life, t½ in order of zero, first, second order…
a)
Co/2k, ln2/k, 1/kCo.
b)
1/kCo, ln2/k, Co/2k,
97.
Graph [ ] vs time of zero order reaction
a)
inversely proportional linear graph
b)
directly proportional linear graph
98.
First order reaction, Graph
a)
ln C vs t give inversely proportional straight line with slope = -k. (if log will ÷2.303)
b)
ln C vs t give directly proportional straight line with slope = -k. (if log will ÷2.303)
99.
Rate/ concentration graph of zero order reaction
a)
Rate vs [A] constant stagnant. K = 0
b)
Rate vs [A] increase. gradient = k
100.
Rate/ concentration graph of first order reaction
a)
Rate vs [A] increase. gradient = k
b)
Rate vs [A] constant stagnant. K = 0
101.
Rate/ concentration graph of second order reaction
a)
Rate vs [A]², gradient = k
b)
Rate vs [A] increase. gradient = k
102.
Elementary reaction
a)
One-step reactions
b)
Two-step reactions
103.
Reaction mechanism
a)
Most rxn take place in several steps (reaction mechanism= from experimental results, rate equation). Sequence of steps lead to formation product.
b)
One of the steps will be slowest, has highest Ea, forms bottle neck of reaction, overall rate rxn dependent, rate equation contain only this species.
104.
Overall stoichiometric equation
a)
Total individual steps
b)
Intermediate
105.
Rate-determining step. A + B (slow) -> X
X + C (fast) -> products
Overall rate rxn depends only,
Rate = k[A][B]
If increase [C] does not affect rate rxn because C cannot take part until X is formed.
a)
One of the steps will be slowest, has highest Ea, forms bottle neck of reaction, overall rate rxn dependent, rate equation contain only this species.
b)
One of the steps will be fastest, has highest Ea, forms bottle neck of reaction, overall rate rxn dependent, rate equation contain only this species.
106.
Alkaline hydrolysis of 2-methyl-2-iodopropane
a)
(SN1) first + zero order
Mechanism= first step require high Ea because involves the breaking of covalent bonds. = second step is fast as involves combination of opposite charged particles. Graf dua bonggol, bonggol pertama lebih tinggi daripada bonggol kedua.
b)
(SN2) first + first.
Only one step, form an intermediate (or an activated complex, in process of C....O forming, C....i breaking).
107.
Alkaline hydrolysis of 1-iodobutane
a)
(SN2) first + first.
Only one step, form an intermediate (or an activated complex, in process of C....O forming, C....i breaking).
b)
(SN1) first + zero order
Mechanism= first step require high Ea because involves the breaking of covalent bonds. = second step is fast as involves combination of opposite charged particles. Graf dua bonggol, bonggol pertama lebih tinggi daripada bonggol kedua.
108.
Activated complex
a)
Intermediate
b)
Total individual steps
109.
SN1 mechanism
a)
Alkaline hydrolysis of 2-methyl-2-iodopropane
b)
Alkaline hydrolysis of 1-iodobutane
110.
SN2 mechanism
a)
Alkaline hydrolysis of 1-iodobutane
b)
Alkaline hydrolysis of 2-methyl-2-iodopropane
111.
Slow and fast. Which one is correct?
a)
2NO (g) + Cl2 (g) -> 2NOCl (g)
NO + Cl2 (slow) -> NOCl2
NOCl2 + NO (fast) -> 2NOCl
Rate = k[NO] [Cl2]
b)
2NO (g) + Cl2 (g) -> 2NOCl (g)
NO + Cl2 (fast) -> NOCl2
NOCl2 + NO (slow) -> 2NOCl
Rate = k[NO] [Cl2]
112.
Rate of reaction
a)
rate change of [substance] with time.
b)
rate constant change of [substance] with time.
113.
Instantaneous rate
a)
Obtained drawing tangents to the [ ] / time graph at particular time.
b)
Obtained drawing tangents to the log [ ] / time graph at particular time.
114.
Effective collision
a)
Collision have enough E to overcome Ea and also in correct orientation.
b)
Collision have enough E to overcome Ea.
115.
Factors affected rates of reactions
a)
[ ]
T
P
Cat
b)
[ ]
T
P
116.
Increasing temperature
a)
Increase the number of fraction of particles having E => Ea.
b)
Decrease the number of fraction of particles having E => Ea.
117.
Catalyst
a)
Increase rate rxn by providing an alternative pathway, with lower Ea for rxn to occur.
b)
Rxn one products formed can act as a catlyst for rxn.
118.
Autocatalyst
a)
Rxn one products formed can act as a catlyst for rxn.
b)
Increase rate rxn by providing an alternative pathway, with lower Ea for rxn to occur.
119.
Enzymes
a)
Catalyst that catalyses biological rxn in living organism.
b)
Catalyst that catalyses biological rxn in non living organism.
120.
Order of reaction
a)
Power of molar [reactant] raised in experimentally determined rate equation.
b)
Time taken for amount of reactant to decrease to half of its original quantity.
121.
Half-life
a)
Time taken for amount of reactant to decrease to half of its original quantity.
b)
Time taken for amount of reactant to decrease to double of its original quantity.
122.
Arrhennius equation
a)
k = Ae^ (-Ea/RT).
b)
kt = Ae^ (-Ea/RT).
123.
When increasing temperature...
a)
Rate constant increases.
b)
Rate constant decreases.
124.
Rate constant dependent on
a)
1. T and
2. presence of catalyst
b)
T only
125.
Rate determining step
a)
Step with highest Ea, slowest step in rxn mechanism, rate equation dependence.
b)
Step with lowest Ea, fastest step in rxn mechanism, rate equation dependence.
Reset
