Chemical Kinetics

Molecularity of a reaction cannot be more than three.
The rate of reaction is expressed as rate 
$$=\cfrac { 1 }{ 2 } \cfrac { d[C] }{ dt } =-\frac { 1 }{ 3 } \frac { d[D] }{ dt } =\frac { 1 }{ 4 } \frac { d[A] }{ dt } =-\frac { d[B] }{ dt }$$
. The reaction is
For the reaction, $$A\rightleftharpoons B, \Delta E$$ for the reaction is $$-33.0\ kJ \ mol^{-1}$$. Assuming pre-exponential factor same for forward and backward reaction.
The half time of first order decomposition of nitramide is 2.1 hrs at $$15^{0}C$$. $$NH_2NO_2(aq)\, \rightarrow\, N_2O(g)\, +\, H_2)(l)$$.
6.2 g of $$NH_2NO_2$$ is allowed to decompose.
The following data were observed for the following reaction at $$25^{\circ}$$ $$C.$$ $$\, CH_3OH\, +\, (C_6H_5)_3CCl\, \rightarrow\, (C_6H_5)_3COCH_3\, +\, HCl$$
SetInitial concentration
(M)
Initial concentration
(M)
time ($$\Delta$$ t)
(min)
Final concnetration
$$[A]_0$$$$[B]_0$$
I0.100.05250.0033
II0.100.10150.0039
III0.200.107.50.0077