The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor

The order of the reaction occurring by following mechanism should be

$(i)$ ${A_2} \to A + A$ (fast)

$(ii)$ $A + {B_2} \to AB + B$ (slow)

$(iii)$ $A + B \to $ (fast)

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

$2 HI \rightarrow H _{2}+ I _{2}$

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

The rate of the reaction, $2NO + Cl_2 \rightarrow 2NOCl$ is given by the rate equation rate $= k[NO]^2[Cl_2].$ The value of the rate constant can be increased by

For the following parallel chain reaction. What will be that value of overall half-life of $A$ in minutes ?

Given that  $\left[ {\frac{{{{\left[ B \right]}_t}}}{{{{[C]}_t}}} = \frac{{16}}{9}} \right]$

$A\,\xrightarrow{{{K_1}\, = \,2\, \times \,{{10}^{^{ - 3}\,}}{S^{ - 1}}}}4B$

$A\to C$

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 $y ?$