Reaction rate between two substance $A$ and $B$ is expressed as following $:$ rate $= k[A ]^n[B]^m$ If the concentration of $A$ is doubled and concentration of $B$ is made half of initial concentration, the ratio of the new rate to the earlier rate will be

The rate constant for the reaction, $2N_2O_5 \to 4NO_2 + O_2$ is $3.0\times 10^{- 4}\,s^{-1}$ . If start made with $1.0\,mol\,L^{-1}$ of $N_2O_5$, calculate the rate of formation of $NO_2$ at the moment of the reaction when concentration of $O_2$ is $0.1\, mol\, L^{-1}$.

The hydrolysis of ethyl acetate is a reaction of ......... order

$C{{H}_{3}}COOEt+{{H}_{2}}O\xrightarrow{{{H}^{+}}}C{{H}_{3}}COOH+EtOH$

The reaction ${N_2}{O_5}$ (in $CCl_4$ solution) $ \to 2N{O_2}$ (solution) $ + \frac{1}{2}{O_2}(g)$ is of first order in ${N_2}{O_5}$ with rate constant $6.2 \times {10^{ - 1}}{s^{ - 1}}.$ What is the value of rate of reaction when $[{N_2}{O_5}] = 1.25\,mole\,{l^{ - 1}}$

For the reaction : $2A + B \to  A_2B$ ; the rate $= K[A]\, [B]^2$ with $K = 2.0\times10^{-6}\, lit^2\, mol^{-2}\, sec^{-1}$. Initial concentration of $A$ and $B$ are $0.2\, mol/lit$ and $0.4\, mol/lit$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12\, mol/litre$.

Order of radioactive disintegration reaction is