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 rate of reaction, $A + B + C \longrightarrow P$ is given by

$r = \frac{{ - d\left[ A \right]}}{{dt}} = K\,{\left[ A \right]^{\frac{1}{2}}}\,{\left[ B \right]^{\frac{1}{2}}}\,{\left[ C \right]^{\frac{1}{4}}}$

The order of reaction is

The reaction $2NO + Br_2 \rightarrow  2NOBr,$ follows the mechanism given below

$(I)$  $NO + Br_2 \rightleftharpoons  NOBr_2 $    ........ Fast

$(II)$  $NOBr_2 + NO \rightarrow 2NOBr$     ......... Slow

The overall order of this reaction is

If in a certain reaction, two different reactants take part then

$A $ gaseous hypothetical chemical equation $2A$ $ \rightleftharpoons  $ $4B + C$ is carried out in a closed vessel. The concentration of $ B$  is found to increase by $5 \times {10^{ - 3}}mol\,\,{l^{ - 1}}$ in $10 $ second. The rate of appearance of $B$  is

The rate law for the reaction  Sucrose + Water $\xrightarrow{{[{H^ + }]}}$ Glucose + Fructose is given by