Chemical Kinetics

2) If I is the intensity of absorbed light and C is the concentration of AB for the photochemical process AB + hv → AB*, the rate of formation of aB* is directly proportional to
a) C
b) I
c) I²
d) CI

3) For the reaction 3BrO^- → BrO₃^- + 2Br^- in an alkaline aqueous solution, the value of the second order (in BrO^-) rate constant at 80°C in the rate law for -d[BrO^-]dt was found to be 0.056 Lmol^-1s^-1. Wha is the rate constant when the rate law is written for
(a) d[BrO₃^-]dt (b) d[Br^-]dt

NOTE:- its actually avg rate(delta)

question is simple but but i m not able to understand the sentence properly

4) Activation Energy changes in the presence of a catalyst. But does it change or remains constant with vatiation of temperature?

5) A catalyst lowers the energy of activation...

is above stmnt true???

but i have also come across the concept of negative catalyst which increases the E_a...

So how can we conclude without specifying the type of catalyst?

plzz help as this is making it difficult to answer Assertion-Reason type questions

1)calculate the value of k using k=.693/t_1/2

NOw initial concentration is given c .after say time t it is decomposed 99.99%
hence left=c-.9999c=.0001c

t=1/klog(c/.001c)
t=1/klog3
thus t can be found.

volume can be found through simple stoichiometry.

2)I think its answer is c

3)write the rate law expression in terms on the reactants a d products n quate to k()

4)k=ae^-E_a/RT
IF T is incresed or decreased the vakue of k changes keepinf the value of E_a constant.

5)IN such cases the graph of the catalyst action and ΔH shud be given.

thanx...

1) arey i toh needed ans to (b) as my ans is not matching..

2) no ans is (d)

3) could u plz make the line "the value of second order....for -d[BrO^-]dt"?