### Chemical Kinetics

goals
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 $25^{\circ}$ $C.$ $\, CH_3OH\, +\, (C_6H_5)_3CCl\, \rightarrow\, (C_6H_5)_3COCH_3\, +\, HCl$
 Set Initial concentration(M) Initial concentration(M) time ($\Delta$ t)(min) Final concnetration $[A]_0$ $[B]_0$ I 0.10 0.05 25 0.0033 II 0.10 0.10 15 0.0039 III 0.20 0.10 7.5 0.0077