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

$$=\cfrac { 1 }{ 2 } \cfrac { d[C] }{ dt } =-\frac { 1 }{ 3 } \frac { d[D] }{ dt } =\frac { 1 }{ 4 } \frac { d[A] }{ dt } =-\frac { d[B] }{ dt }$$

. 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 |