F.Sc. Part 1 Chemistry.Ch.11.Test (Malik Xufyan)

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Maliks Chemistry - F.Sc. l
Maliks Chemistry- F.Sc. ll
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Maliks Chemistry - F.Sc. l
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CHEMISTRYCHEMISTRYCHEMISTRY
Chapter-wise
Test Series
Malik Xufyan
JIAS ACADEMY
Malik
Jhang Ins tute for Advanced Studies
0313-7355727
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Malik Xufyan
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Chapter # Topic Page #
Basic concepts – Unsolved paper1
2
3
4
5
6
7
8
9
10
11
5
6
16
17
24
25
36
37
45
46
54
55
64
65
73
74
83
84
93
94
103
104
Experimental Techniques – Solved Paper
Gases – Unsolved Paper
Gases – Solved Paper
Liquid – Unsolved Paper
Liquid – Solved Paper
Atomic Structure – Unsolved Paper
Atomic Structure – Solved Paper
Chemical Bonding –Unsolved Paper
Chemical Bonding – Solved Paper
Thermochemistry – Unsolved Paper
Thermochemistry – Solved Paper
Chemical Equilibrium – Unsolved Paper
Chemical Equilibrium – Solved Paper
Solu on – Unsolved Paper
Solu on – Solved Paper
Electrochemistry – Unsolved Paper
Electrochemistry – Solved Paper
Chemical Kine cs – Unsolved Paper
Chemical Kine cs – Solved Paper
Basic concepts – Solved Paper
Experimental techniques – Unsolved Paper
INDEX

Chapter#11:Chemical Kinetics Malik Chemistry
Jhang Institute for Advanced Studeies104
Name : CH # Chemical Kinetics Class 11th
Chemistry Test # 11, CH # 11 (Complete) Marks : 85
Time : 2 & Half Hour Objective & Subjective JIAS Test System
Section-I= Objectives
1. Choose the correct answer 17x1=17
Sr # Statement A B C D
1. According to collision theory the rate of reaction is
equal to
Number of collisions Number of effective
collisions
Concentration of
products
Concentration of
reactants
2. The unit of the rate constant is the same as that of First order reaction 2nd
order reaction 3rd
order reaction Zero order
reaction
3. The energy of activation by using catalyst for a
reaction is
Increased Decreased No change Moderate
4. Rate of chemical reaction is characterized by Concentration Temperature Catalyst All
5. If the energy of the activated complex lies close to
the energy of reactants it means that reaction is
Slow Fast Exothermic Endothermic
6 Photochemical reactions are 1st
order 2nd
order 3rd
order Zero order
7. The chemical substances which increase the effect
of catalyst are
Promoters Inhibitors Both a and b speeder
8. In zero order reaction ,the rate is independent of Temperature of reaction Concentration of
reactants
Concentration of
products
None of these
9. The rate of reaction is defined as dc/dt dt/dc dc.dt (dc)2
/(dt)2
10. A substance that affects the rate of reaction but
remains unaltered at the end of reaction is called
Acid Base Catalyst Activator
11. With the increase of reaction ,the rate of reaction Increases greatly Does not increase Increases a little Decrease rapidly
12. Which method is used for those reactions which
involve small volume change in solutions
Spectrometry Conductrometry Dilatometry
method
Refractrometric
reaction
13. Half life period of 1st
order reaction is independent
of
Initial concentration of
reactants
Condition of
temperature
Presence of
catalyst
All
14. The change in concentration of reactants or products
per unit time is called
Rate law Rate equation Rate of reaction Rate constant
15. The reaction that involve gases ,the rate depends on Catalyst Temperature moles/dm3
Partial pressure
16. Larger the surface area of the reactant molecules Lower the rate of
reaction
Higher the rate of
reaction
Rate of reaction is
unaffected
Rate may increase
or decrease
17. Catalyst accelerates the reaction by Lowering activation
energy
Increasing activation
energy
Lowering kinetic
energy
Lowering enthalpy
change

Jhang Institute for Advanced Studeies 105
Section l: Short Questions
2. Attempt only EIGHT questions. 8 x 2 = 16
i. What is reaction kinetics?
ii. How rate of reaction can be shown diagram-
matically?
iii. What is the importance of rate of reaction?
iv. Rate of reaction is an ever changing parameter.
Explain
v. Differentiate between rate of reaction and rate
constant?
vi. The sum of co-effitiants of a balanced equation
is not necessarily important to give order of re-
action. Justify
vii. The order of reaction is obtained from the rate
expression but the rate expression is obtained
from experiment. Justify
viii.Differentiate between fast step and rate deter-
mining step.
ix. 50 % of hypothetical 1st
order reaction com-
pletes in one hour .the remaining 50 percent
needs more than that one hour to complete.
x. The radioactive decay is always a 1st
order reac-
tion. Why?
xi. Differentiate between enthalpy change of reac-
tion and energy of activation of the reaction?
xii. Differentiate between homogeneous and het-
erogeneous reactions?
3. Attempt only 8 questions 8 X 2 = 16
i. What is activation of catalyst?
ii. Differentiate between negative catalyst and au-
to-catalyst?
iii. Write four characteristic of enzyme catalysis?
iv. Write four characteristics of a catalyst?
v. What is energy of activation?
vi. Draw Arrhenius plot to calculate the energy of
activation.
vii. Name the factors which affect the rate of chem-
ical reaction.
viii.What is the effect of concentration of reactants
on the rate of reaction?
ix. How order of reaction can be found?
x. Explain method of large excess?
xi. Differentiate between exothermic and endo-
thermic reaction
xii. What are the physical methods to determine the
rate of reaction?
4. Attept any 6 questions 6 x 2 = 12
i. What is psedudo 1st
order reaction? Give exam-
ple?
ii. How can you define order of reaction?
iii. What is zero order rection? Give example
iv. What is dilatometric method?
v. What is optical rotation method?
vi. What is catalytic poisning?
vii. How temperature affects the role of catalyst?
viii. What is a catalyst .what are its types?
ix. Differentiate between activation energy and ki-
netic energy?
Section-ll: Long Questions.
Attempt any three questions. 8 x 3 = 24
5) a) Write a detailed note on energy of activation.
b) A plot of Arrhenius equation for the thermal
decomposition of N2
O5
when slope is found to
be at -5400K. Calculate the energy of activation
of this reaction.
6) a) What is order of reaction .Write detail the
types of order of reaction with examples.
b) How the rate of reaction can be measured
graphically?
7) a) Write in detail the effect of temperature on
the rate of reaction
b) What is half life method? Find the different or-
der of reaction with this method?
8) a) Explain Arrhenius equation in detail.
b) Define catalyst. Write its types and describe the
characteristics of catalysts.
9) a) What factors are affected on the rate of reac-
tions?
b) What is determination of the rate of reaction in
detail?

Section l: Short Questions
2. Attempt only EIGHT questions 8 x 2 = 16
i. What is reaction kinetics?
The branch of chemistry, which deals with the study of reaction rates and the factors, which affect these
rates, is known as reaction kinetics.
ii. How rate of reaction can be shown diagrammatically?
iii. What is the importance of rate of reaction?
Having a slow rate of reaction means that more time is spend on manufacturing the product, whereas
having a fast rate of reaction, there is less time spent on manufacturing the product. Manufacturers are
always aiming to make a profit so they increase the rate of the chemical reaction which leads to spend-
ing less money and time.
iv. Rate of reaction is an ever changing parameter. Explain.
According to the law of mass action, rate of a chemical reaction is directly proportional to the concen-
tration of reactants.
When the reaction starts, the concentration of reactants is high, therefore, rate of reaction is fast. As the
concentration of reactants is decreased, the rate of a reaction is also decreased. At the end of reaction,
the reaction becomes very slow. Hence, rate of a chemical reaction is an ever changing parameter.
v. Differentiate between rate of reaction and rate constant?
Sr # Rate of reaction Rate constant of a reaction
1 It is the change in concentration of reactants
or products divided by the time taken for
the change.
It is the rate of a reaction when the concentration
of reactants is unity.
2 It changes with time. It does not change with time.
3 It depends upon the concentration of
reactants.
It is independent of the concentration of reactants.
4 It is variable quantity. It is constant quantity.
5 Its units are moldm-3
s-1
. Its units depend upon the order of reaction.
vi. The sum of co-effiticients of a balanced equation is not necessarily important to give order of reac-
tion. Justify.
The sum of the exponents to which the concentration terms in the rate law are raised to express the
observed rate of reaction is called the order of reaction. Thus, rate law, i.e., the order of reaction is
determined experimentally. The sum of the exponents in the rate law equation may or may not be the
same as in a balanced chemical equation. Therefore, the sum of the co-efficient of a balanced equation

is not necessarily important to give the order of reaction.
vii. The order of reaction is obtained from the rate expression but the rate expression is obtained from
experiment .justify.
There is no simple relationship b/w the overall reaction and the rate law expression. A reaction may
consist of several elementary steps(reactions) and the rate law expression is the combined result of
these steps. That is why, we cannot predict the rate law expression by looking at the overall equation.
Therefore, the rate law expression must be determined experimentally.
viii. Differentiate between fast step and rate determining step.
Sr # Fast step Rate determining step
1 An elementary reaction that is fast in the
reaction mechanism is called fast step.
The slowest step in the reaction mechanism is called
rate determining step.
2 It does not control the rate of reaction. It controls the rate of reaction.
ix. 50% of hypothetical 1st
order reaction completes in one hour .the remaining 50 percent needs
more than that one hour to complete.
The half life for the first order reaction is the time required to convert 50% of the reactants to products.
This occurs at 1 hour, so, t1/2
= 1 hour. It means in one half-life (1 hour) the concentration decreases
50% and 50% of reactants will be left behind. At the end of second half life, which occurs at 2 hours, the
concentration decreases by one-half again from 50% tp ½ × 50% = 25%. It means 75% of the reactants
are completed in two hours and 25% would be left behind and so on. Thus the remaining 50% needs
more than 1 hour to complete reaction.
x. The radioactive decay is always a 1st
order reaction. Why?
The half-life of a radioactive substance is the time required for disintegration of half of the element into
daughter elements. The half life of a radioactive substance is independent of the amount of the sample.
For the first order reaction, the half life is also independent of the initial concentration of the reactant.
Therefore, the radioactive decay is always the 1st
order of reaction.
xi. Differentiate between enthalpy change of reaction and energy of activation of the reaction?
Sr # Enthalpy change of a reaction Energy of activation of reaction
1. Enthalpy change equals the heat of
reaction at constant pressure.
The minimum amount of energy in addition to
average K.E which the particles must have for the
effective collisions is called activation energy.
2. ∆H = qp
Ea
= -2.303 R × slope
3. Enthalpy change depends on the initial
and final state of the reaction.
Activation energy depends upon the slope.
xii. Differentiate between homogeneous and heterogeneous catalysis?
Sr # Homogeneous catalysis Heterogeneous catalysis
1 In this catalysis, reactants and catalyst are
in the same phase.
In this catalysis, reactants and catalyst are in
different phase.
2 In this, the system remains homogeneous
during the reaction.
In this, the system remains heterogeneous during
the reaction.
3 Mostly liquids and gases are used as
homogenous catalysts.
Mostly solid are used as heterogeneous catalysts.
4 Example:
2SO2(g) + O2(g)
NO
2SO3(g)
NO is a homogeneous catalyst.
Example:
2SO2(g) + O2(g)
V2O5
2SO3(g)
V2
O5
is heterogeneous catalyst.

3. Attempt only 8 questions 8 X 2 = 16
i. What is activation of catalyst?
Activation of catalyst:
A substance which promotes the activity of a catalyst is called a promoter or activator or activation of
catalyst.
Example:
Hydrogenation of vegetable oil is carried out by Ni. The catalytic activity of Ni can be increased by
using Cu and tellurium.
ii. Differentiate between negative catalyst and auto-catalyst?
Sr # Negative catalyst Auto catalyst
1 A substance which retards the rate of a
reaction is called a negative catalyst. And
this phenomenon is called negative catalysis.
In some reactions, a product formed acts as
catalyst. And this phenomenon is called auto
catalysis.
iii. Write four characteristic of enzyme catalysis?
Characteristic of enzyme catalysis:
1) Enzymes are the most efficient catalysts known and they lower the energy of activation of a reaction.
2) Enzymes catalysis are highly specific. E.g., Urease catalyses the hydrolysis of urea only and it cannot
hydrolyze any other amide even methyl urea.
3) Enzyme catalytic reactions have maximum rates at an optimum temperature.
4) The pH of the medium also controls the rates of enzyme catalytic reactions. Each enzyme has an opti-
mum pH.
iv. Write four characteristics of a catalyst?
Characteristics of a catalyst:
1) A catalyst cannot affect the equilibrium constant of a reaction. It only decreases the time to reach equi-
librium.
2) A catalyst is specific in its reaction. A particular catalyst works for one reaction. It may not work for any
other reaction.
3) The mechanism of a catalyzed reaction is different from that of an uncatalysed reaction.
4) A catalyst cannot start a reaction, which is not thermodynamically feasible.
v. What is energy of activation?
Activation energy:
The minimum amount of energy in addition to average K.E which the particles must have for the ef-
fective collisions is called activation energy.
Ea
= -2.303 R × slope
Activation energy provides information about the path a reaction occurs.
vi. Draw Arrhenius plot to calculate the energy of activation.
See the topic of Arrhenius equation.
vii. Name the factors which affect the rate of chemical reaction.
Following factors affect the rate of reaction.
• Nature of a reactant.
• Concentration of reactants.
• Surface area.
• Light.
• Temperature.
• Catalyst.
viii. What is the effect of concentration of reactants on the rate of reaction?

Rate of a reaction is affected by increasing or decreasing the concentration of reactants.
According to the Law of Mass Action:
“the rate at which a substance reacts, is directly proportional to its active mass, and the rate of reaction
is directly proportional to the product of active masses of reacting substances”
Thus, by increasing the conc. of any reactant, rate of reaction is increased and by decreasing the conc.
rate of reaction is decreased. The frequency of collisions b/ w molecules depend upon concentrations.
The more crowded the molecules, the more chance of collision. Hence, rate of reaction increases. Ex-
ample: combustion in normal air (with 21% O2
) becomes faster in pure O2
.
ix. How order of reaction can be found?
Many methods are used to determine the order of reaction.
• Hit and trial method.
• Graphical method.
• Differential method.
• Half life method.
• Method of large excess.
x. Explain method of large excess?
In this method, one of the reactants is taken in small amount while others are atken in large amounts.
Since conc. of reactants present in large amount is almost constant. Therefore, rate does not depend on
their concentrations.
Hence, rate only depends upon the conc. of reactant taken in small amount. It is because small changes
in its amount greatly affect the rate. Thus order of reaction with respect to this reactant is determined.
Similarly, this process is repeated with all the reactants by taking them in small amounts.
Thus, order of reaction with respect to reactant is determined.
Hence, overall order of reaction is the sum of the order with respect to each reactant.
xi. Differentiate between exothermic and endothermic reaction.
Sr# Endothermic reactions: Exothermic reaction
1. The chemical reactions which are
accompanied by absorption of heat, are
called endothermic reaction.
The chemical reactions which are accompanied
by the evolution of heat, are called exothermic
reactions.
xii. What are the physical methods to determine the rate of reaction?
Most commonly used physical methods to determine the rate of reaction are:
• Spectrometry
• Conductometery
• Dilatometric method
• Refractrometry
• Optical rotation method (Poliarimetery)
4. Attempt any 6 questions. 6 x 2 =12
i. What is pseudo 1st
order reaction? Give example?
Pseudo first order reaction:
if two reactants are available in reaction but reaction is depend only one reactant due to other large
excess reactant. This reaction is known as pseudo first order reaction.
Example: Hydrolysis of tertiary butyl bromide is pseudo first order reaction.

CCH3
CH3
CH3
Br + H2O CCH3
CH3
CH3
OH + HBr
ii. How can you define order of reaction?
Order of reaction:
The number of reaction molecules whose concentration changes during a reaction is called order of
reaction. Or
The sum of powers to which concentrations are raised in the rate law expression is called order of re-
action.
iii. What is zero order reaction? Example.
Zero order reaction:
When the reaction is independent of the concentration of reactants, it is called zero order reaction.
Example:
Decomposition of HI (on gold surface)
2HI
on gold surface
H2 + I2
The experimental rate equation for this reaction is;
Rate = k[HI]0
= k
This reaction is independent of the concentration of HI, hence, it is a zero order reaction. Photochem-
ical reactions are usually zero order reactions.
iv. What is dilatometric method?
This method is used for reactions in which volume is changed.
The volume change is directly proportional to the progress of reaction.
v. What is optical rotation method?
This method is used to when 1 of the substance is optically active. i.e. it can rotate the plane polarized
light. The angle of rotation is directly proportional to the progress of reaction.
After measurement, graph is plotted and rate of reaction is determined from the graph.
vi. What is catalytic poisoning?
Catalytic Poisoning:
The process of decreasing of the activity of a catalyst by the addition of small quantity of other sub-
stance is called catalytic poisoning.
Example:
in the manufacture of H2
SO4
, the traces of arsenic present as impurities in the reacting gases makes
platinum ineffective.
vii. How temperature affects the role of catalyst?
Physical states of some catalysts are changed by changing the T. Hence, their catalytic power will be

decreased e.g. colloidal catalysts like platinum may be coagulated with the rise in temperature.
viii. What is a catalyst? What are its types?
Catalyst: A substance that changes the rate of reaction but remains chemically unchanged at the end of
the reaction is called catalyst.
Types:
• Activator
• Promoter
• Negative catalyst
• Auto-catalyst
ix. Differentiate between activation energy and kinetic energy?
Sr.# Activation energy Kinetic energy
1. The minimum amount of energy which
is required to start chemical reactions,
called activation energy.
The minimum amount of energy present in the reactant
due to its movement is called kinetic energy.
2. It is denoted by Ea
It is represented by K.E
Section-lIl: Long Questions.
Attempt any THREE questions. 8 x 3 = 24
5) a) Write a detailed note on energy of activation.
b) A plot of Arrhenius equation for the thermal decomposition of N2
O5
when slope is found to be at
-5400K. Calculate the energy of activation of this reaction.
6) a) What is order of reaction and write detail the types of order of reaction with examples.
b) How the rate of reaction can be measured graphically?
7) a) write in detail the effect of temperature on the rate of reaction
b) What is half life method? Find the different order of reaction with this method?
8) Explain Arrhenius equation in detail.
b) Define catalyst. Write its types and describe the characteristics of catalysts.
9) a) What factors are affected on the rate of reactions?
b) What is determination of the rate of reaction in detail?

Papers Preparations Trick and tip
(2017)
Short Questions
Q.No. 2 : 1, 2, 3,8 ( 3 short questions)
Q. No. 3: 4 =4 , 5 =4, 9=2 ,10=2
Q.No.4: 6=4, 7=2, 11=3
Long Questions
Questons Chapters
Q# 5 (1+4)
Q#6 (3+5)
Q#7 (6+7)
Q#8 (8+10)
Q#9 (9+11)
MCQs===>
2 Question from CH# 1,3,4,5,6 & 8
One Question from CH# 2,7,9,10 & 11
Numericals: Ch # 1 & 8
1-7 chpaters preparation scheme (For average students)
Prepare only 7 chapters and All exercises mcqs. (in Sha Allah 90 % paper will be adopted)
With the help of scheme u can solved:
 11 mcqs (from 1-7 chapters )
 6 long questions, (Q,5,Q,6,Q,,7),[ (from 1-7 chapters )]
 9 short questions from Q.2, [(from 1-7 chapters )]
 8 short questions from Q.3, [(from 1-7 chapters )]
 6 short questions from Q.4 [(from 1-7 chapters )]
(23 short questions solved)
Malik Xufyan

F.Sc. Part 1 Chemistry.Ch.11.Test (Malik Xufyan)

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