$A + 2B \to C$, the rate equation for this reaction is given as Rate $= K[A][B]$ . If the concentration of $A$ is kept the same but that of $B$ is doubled what will happen to the rate it self ?

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(i)$ $3 NO ( g ) \rightarrow N _{2} O$ $(g)$ Rate $=k[ NO ]^{2}$

If doubling the initial concentration of reactant doubles $t_{1/2}$ of reaction, the order of reaction is

Write unit of rate constant of following reaction :

$1.$ zero order

$2.$ second order

The experimental data for decomposition of $N _{2} O _{5}$

$\left[2 N _{2} O _{5} \rightarrow 4 NO _{2}+ O _{2}\right]$

in gas phase at $318 \,K$ are given below:

$(i)$ Plot $\left[ N _{2} O _{5}\right]$ against $t$

$(ii)$ Find the half-life period for the reaction.

$(iii)$ Draw a graph between $\log \left[ N _{2} O _{5}\right]$ and $t$

$(iv)$ What is the rate law $?$

$(v)$ Calculate the rate constant.

$(vi)$ Calculate the half-life period from $k$ and compare it with $(ii)$.

Diazonium salt decomposes as ${C_6}{H_5}N_2^ + C{l^ - } \to {C_6}{H_5}Cl + {N_2}$ At ${0\,^o}C$, the evolution of ${N_2}$ becomes two times faster when the initial concentration of the salt is doubled. Therefore, it is