Wired Faculty
For the chemical reaction,
2O3 ⇌ 3O2
The reaction proceeds as follows
O3 ⇌ O2 + O
O + O3 → 2O2 (slow)
The rate law expression will be
r = k' [O3]2
r = k' [O3]2[O2]-1
r = k'[O3][O2]
unpredictable
B.
r = k' [O3]2[O2]-1
As slowest step is the rate determining step. Hence, from slow reaction r = K[O][O3] ... (i)
From the fast reaction,
In the following graph
The slope of line AB give the information of the
value of
Value of
value of
value of
C.
value of
The correct difference between first and second order reactions is that
The rate of a first-order reaction does not depend on reactant concentrations; the rate of a second-order reaction does depend on reactant concentrations
The half-life of a first-order reaction does not depend on [A]0; the half-life of a second-order reaction does depend on [A]0
The rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations
A first-order reaction can catalyzed; a second-order reaction cannot be catalyzed
B.
The half-life of a first-order reaction does not depend on [A]0; the half-life of a second-order reaction does depend on [A]0
The first-order reaction is given by, which is independent of the initial concentration of reactant.
Second order reaction, , which depends on the initial concentration of reactant.
Sponsor Area
When initial concentration of the reactant is doubled, the half-life period of a zero order reaction
Is halved
Is doubled
Remains unchanged
Is tripled
B.
Is doubled
Sponsor Area
Sponsor Area
Mock Test Series
