Explanation
Order of reaction can be zero, negative or positive.
Number of collisions of one molecule / unit time = X
As in one collision, two molecules are involved,
collision frequency = N X / 2 .
Presence of enzyme lowers the activation energy.
A catalyst alters the reaction mechanism.
(a) is a reaction of 1st order.
Higher the activation energy, lower is the rate constant.
A reaction with two reactants cannot be unimolecular.
With increase in temperature, population of activated molecules increases.
Greater the value of k, faster is the reaction.
t1/2 t of 1st order reaction is independent of ‘a’.
H+ ions act as catalyst for the given reaction.
A straight line is obtained when log k is plotted against 1/T.
A straight line plot of [A] vs t with negative slope is for a reaction of zero order.
The given reaction is of 3rd order.
For 1st order reaction, t1/2 is independent of initial concentration.
The activation energy can be determined by evaluating rate constants at two different temperatures (Arrhenius equation).
Rate of reaction increases with increase in temperature because number of collisions increases.
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