Write differential rate expression of following reaction and give its order of reaction :

$2 N _{2} O _{5} \rightarrow 4 NO _{2}( g )+ O _{2}$

$C _{4} H _{9} Cl + OH ^{-} \rightarrow C _{4} H _{9} OH + Cl ^{-}$

The unit of rate constant for a zero order reaction is

Consider a reaction $\mathrm{aG}+\mathrm{bH} \rightarrow$ Products. When concentration of both the reactants $\mathrm{G}$ and $\mathrm{H}$ is doubled, the rate increases by eight times. However, when concentration of $\mathrm{G}$ is doubled keeping the concentration of $\mathrm{H}$ fixed, the rate is doubled. The overall order of the reaction is

The mechanism of the reaction $A + 2B \to  D$ is

$2B\xrightarrow{k}{B_2}\,\left[ {Slow} \right]$

${B_2} + A \to D\,\left[ {Fast} \right]$

The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order of reaction are respectively

Select the rate law that corresponds to the data shown for the following reaction $A+ B\to C$

In a reaction involving hydrolysis of an organic chloride in presence of large excess of water$RCl + {H_2}O \to ROH + HCl$