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2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
1
Physical
Chemistry
TOPIC: CHEMICAL KINETICS
Target CSIR-NET/GATE
2637, Hudson Lane, Behind Khalsa College, Near G.T.B.
Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail:
info@asfinstitute.com, www.asfinstitute.com
Page 2
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
1
Physical
Chemistry
TOPIC: CHEMICAL KINETICS
Target CSIR-NET/GATE
2637, Hudson Lane, Behind Khalsa College, Near G.T.B.
Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail:
info@asfinstitute.com, www.asfinstitute.com
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
2
SOME IMPORTANT GRAPH REPRESENTATION
Use in chemical kinetics :
(1) y = mx + C
(2) y = –mx + C
(3) y = mx
Page 3
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
1
Physical
Chemistry
TOPIC: CHEMICAL KINETICS
Target CSIR-NET/GATE
2637, Hudson Lane, Behind Khalsa College, Near G.T.B.
Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail:
info@asfinstitute.com, www.asfinstitute.com
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
2
SOME IMPORTANT GRAPH REPRESENTATION
Use in chemical kinetics :
(1) y = mx + C
(2) y = –mx + C
(3) y = mx
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
3
(4) y = –mx
Slope = –m = tan ?
Intercept = zero
(5) y = e
x
(6) y = e
–x
Page 4
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
1
Physical
Chemistry
TOPIC: CHEMICAL KINETICS
Target CSIR-NET/GATE
2637, Hudson Lane, Behind Khalsa College, Near G.T.B.
Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail:
info@asfinstitute.com, www.asfinstitute.com
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
2
SOME IMPORTANT GRAPH REPRESENTATION
Use in chemical kinetics :
(1) y = mx + C
(2) y = –mx + C
(3) y = mx
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
3
(4) y = –mx
Slope = –m = tan ?
Intercept = zero
(5) y = e
x
(6) y = e
–x
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
4
(7) y =
1
x
Page 5
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
1
Physical
Chemistry
TOPIC: CHEMICAL KINETICS
Target CSIR-NET/GATE
2637, Hudson Lane, Behind Khalsa College, Near G.T.B.
Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail:
info@asfinstitute.com, www.asfinstitute.com
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
2
SOME IMPORTANT GRAPH REPRESENTATION
Use in chemical kinetics :
(1) y = mx + C
(2) y = –mx + C
(3) y = mx
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
3
(4) y = –mx
Slope = –m = tan ?
Intercept = zero
(5) y = e
x
(6) y = e
–x
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
4
(7) y =
1
x
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009
Mob. 09555785548, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com
5
CHEMICAL KINETICS
“Chemical kinetics involves the study of the rates and mechanism of chemical reactions.”
The rates of reactions :
(a) The definition of rate : Consider a reaction of the form
A + 2B ? 3C + D …(1)
in which the molar concentration of participants are [A], [B], [C] & [D].
The rate of consumption or decomposition of the one of the reactants at a given time is
[ ] d R
dt
? , where R is A or B. The rate of formation of one of the products is
[ ] d P
dt
, where P is C or D.
The rate of reaction can be expressed with respect to any species in equation (1).
Rate =
[ ] 1 [ ] 1 [ ] [ ]
2 3
d A d B d C d D
dt dt dt dt
? ? ? ?
Thus, the rate of reaction can be defined with respect to both reactants and products.
For example :
4NO
2
(g) + O
2
(g) ? 2N
2
O
2
(g)
find the expression for rate of reaction.
Sol. 4NO
2
(g) + O
2
(g) ? 2N
2
O
2
(g)
rate =
2 5 2 2
[ ] 1 [ ] [ ] 1
4 2
d N O d NO d O
dt dt dt
? ? ?
(b) Rate laws and rate constant :
The rate of a reaction will generally depends on temperature pressure and concentration of
species involving in the reaction.
The rate of reaction is proportional to the molar concentration of reacting species.
i.e. A + B + C + D + ……. ? Product
then, rate of reaction = k[A]
a
[B]
b
[C]
c
[D]
d
………..
Read More
FAQs on Chemical kinetics - Additional Documents & Tests for IIT JAM
| 1. What is chemical kinetics? |  |
Ans. Chemical kinetics is the branch of chemistry that studies the rates of chemical reactions and the factors that influence these rates. It involves the study of how fast or slow a reaction occurs, the mechanisms by which reactions take place, and the factors that affect the rate of reaction.
| 2. What are the factors that affect the rate of a chemical reaction? | |
Ans. Several factors can influence the rate of a chemical reaction. These include temperature, concentration of reactants, surface area, presence of catalysts, and the nature of the reactants and their physical state. Increasing the temperature, concentration, or surface area, and using catalysts, can generally increase the rate of reaction.
| 3. How is reaction rate determined experimentally? | |
Ans. The rate of a chemical reaction can be determined experimentally by measuring the change in concentration of reactants or products over time. This can be achieved by monitoring the color change, pH change, or using techniques such as spectroscopy or chromatography. By measuring the initial rate of reaction at different conditions, it is possible to study the effect of various factors on the rate.
| 4. What is the collision theory in chemical kinetics? | |
Ans. The collision theory is a fundamental concept in chemical kinetics that explains how chemical reactions occur at the molecular level. According to this theory, for a reaction to occur, the reactant molecules must collide with sufficient energy and with the proper orientation. The collision theory helps in understanding the factors that affect the rate of a chemical reaction.
| 5. What are elementary reactions in chemical kinetics? | |
Ans. Elementary reactions are individual steps that make up a complex chemical reaction. They are the simplest possible reactions and involve the collision and transformation of reactant molecules into products. Elementary reactions have specific reaction rate laws and can be combined to form the overall reaction mechanism. Understanding the kinetics of elementary reactions is crucial for studying the overall rate of complex reactions.
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