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k = A.e – A.e –E a /RT
ln k = ln A –
Where k = Rate constant at absolute temperature T.
Ea = Energy of activation
R = Gas constant
A = Frequency factor or pre-exponential factor.
log10k = log10A –
Explain with the help of potential energy barrier, how does increase in temperature increases
the rate of reaction.
Refer 5.4 (c)
Define Activation Energy.
Activation energy is defined as the minimum kinetic energy required for a molecular collision
to lead to a reaction.
Using Arrhenius equation explain why the rate of reaction increases with increase in temperature.
Refer 5.4 (c).
Derive an expression for Arrhenius equation and temperature variation. OR Derive an expression
showing variation in rate constant with temperature.
Refer 5.4 (d).
How will you determine activation energy with the help of a graph.
(Intext question Textbook page no : 213)
Refer 5.4 (f).
Explain, with the help of potential energy barrier, how does a catalyst increase the speed of
a reaction.
Refer 5.4 (g).
Comment on the effect of catalyst on each of the following :
a) Activation energy
b) Rate of forward reaction
c) Rate of backward reaction.
a) Activation energy : It lowers the activation energy of the reaction.
b) Rate of forward reaction : A catalyst increases the rate of forward reaction.
c) Rate of backward reaction : A catalyst increases the rate of backward reaction to the
same extent as the rate of forward reaction.
Hence, a catalyst does not effect the reaction equilibrium it just helps to achieve the equilibrium
Unique Solutions ®
S.Y.J.C. Science - Chemistry - Part I