For the reaction taking place on water, the order of reaction is

${{H}_{2}}+C{{l}_{2}}\xrightarrow{\text{Sunlight}}2HCl$

The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism

$(i)$ $X + Y \rightleftharpoons M$      very rapid equilibrium

$(ii)$ $M + Z \to P$      slow

$(iii)$ $O + Y \to N$      very fast

What is the rate law for this reaction

If a reaction has the experimental rate expression rate $= K [A]^2[B]$, if the concentration of $A$ is doubled and the concentration of $B$ is halved, the what happens to the reaction rate

Assertion :The order of a reaction can have fractional value.

Reason : The order of a reaction cannot be written from balanced equation of a reaction.

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 $(ii)$.

Reaction $aA + bB\,\to $ product. The rate of reaction $= k[A]^3\, [B]^0$ if the concentration of $A$ is double and concentration of $B$ is half the rate will be ?