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352
∴ ln k = ln A –
Ea
RT
∴ log10k = log10 A –
Ea
2.303RT
– Ea
+ log10 A
2.303RT
(y = mx + c)
4. log10 k is plotted against reciprocal of temperature T.
– Ea
5. The slope of the straight line graph is
from which energy of activation can be
2.303R
Ea
calculated as follows slope =
2.303R
∴ Ea = slope × 2.303 R
logk =
(g) Effect of catalyst on rates of reactions :
1. A catalyst is a substance, when added
to the reactants, increases the rate of
reaction without itself being consumed.
2. The catalyst enters the reaction but
does not appear in the balanced
equation. This is because it is
consumed in one step and regenerated
in the another.
3. The catalyst provides an alternative
pathway (mechanism) of lower
activation energy for the reaction to
occur.
4. The height of the barrier for
uncatalysed reaction is greater than
that in a catalysed reaction.
5. Therefore, the number of molecules
that possesses minimum kinetic energy
[Ea] increases.
6.
According to Arrhenius equation.
k = A.e – E a /RT
Unique Solutions ®
S.Y.J.C. Science - Chemistry - Part I
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