For a certain reaction the expression for half life is $t \propto \frac{1}{{{a^{n - 1}}}}$ then the order of reaction is

The half-life of decomposition of gaseous $CH_3CHO$ at initial pressure of $364\, mm$ and $182\, mm$ of $Hg$ were $440\, sec$ and $880\, sec$ respectively. The order of the reaction is

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

From the following which is a second order reaction

For the reaction $A + B \rightarrow$ products, it is observed that

$(i)\,\,$on doubling the initial concentration of $A$ only, the rate of reaction is also doubled and

$(ii)$  on doubling the initial concentration of both $A$ and $B,$ there is a change by a factor of $8$ in the rate of the reaction.

The rate of this reaction is given by

For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?