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 $0.12\, mol/litre$.

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

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

${B_2} + A \to D$          [Fast]

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

For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is

For reaction $2A + B \to $ products, the active mass of $ B $ is kept constant and that of $A$ is doubled. The rate of reaction will then

A study of chemical kinetics of the reaction $A + B \to$  Products, gave the following data at $25\,^oC$.

Find out rate law

For a chemical reaction $A + B \rightarrow$ Product, the order is $1$ with respect to $A$ and $B$.

What is the value of $x$ and $y ?$