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355
*10.
Ans.
How does a catalyst differs from a reaction intermediate?
Refer 5.4 (i).
*11.
Ans.
Explain briefly the collision theory of bimolecular reactions.
Refer 5.4 (a).
12.
Ans.
Derive Arrhenius equation from Collision theory of bimolecular reactions.
Refer 5.4 (b).
Multiple Choice Questions :
•
*1.
Theoretical MCQs :
The rate constant of a reaction .......
a) decreases with increasing Ea
b) decreases with decreasing Ea
c) is independent of Ea
d) decreases with increasing temperature
A catalyst increases the rate of the reaction by .......
b) increasing T
c) decreasing Ea d) decreasing T
a) increasing Ea
The Arrhenius equation is
*2.
*3.
– E /RT
a) A = ke e a
4.
b)
A E a / RT
e
k
c)
k = Ae E a /RT
d) k = Ae – RT/E a
The units of pre-exponential factor or frequency factor are same as .......
a) Rate of reaction
b) Rate constant
c) Order of reaction
d) Molecularity of reaction.
HOURS BEFORE EXAM
Chemical kinetics is concerned with the rates of reactions factors affecting the rates and the
mechanisms by which they proceed.
The rate of reaction is defined as the decrease is molar concentration of a reactant or increase
in molar concentration of a product per unit time.
It can be expressed as average rate during a given time interval or the instantaneous rate
at a specific time.
The reaction rate depends on five factors :
The concentration of reactants, temperature, presence of a catalyst nature of reactant and
pressure.
The concentration dependence is given by the rate law. The rate law for a general reaction,
aA + bB ⎯⎯
→ cC + dD , is given by the expression, rate = k[A]x[B]y, where k is the rate
constant of the reaction and x and y represent the order of the reaction with respect to reactants
A and B respectively. The overall order of the reaction is x + y.
Chapter - 5 Chemical Kinetics
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