1) The half-time of first order decomposition of nitramide is 2.1hr at 15°C
NH2NO2(aq) → N2O(g) + H2O(l)
If 6.2g of NH2NO2 is allowed to decompose, calculate
a) time taken for NH2NO2 to decompose 99%.
b) volume of dry N2O produced at this point, measured at STP.
plz explain (b) a bit elaborately..
12) 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
13) 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
14) Activation Energy changes in the presence of a catalyst. But does it change or remains constant with vatiation of temperature?
15) 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 Ea...
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
111)calculate the value of k using k=.693/t1/2
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-Ea/RT
IF T is incresed or decreased the vakue of k changes keepinf the value of Ea constant.
5)IN such cases the graph of the catalyst action and ΔH shud be given.
1thanx...
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"?