For the reaction $2NO + Cl_2 \rightarrow 2NOCl$,the following mechanism is proposed. What will be the rate law for the reaction? $NO + Cl_2 \rightleftharpoons NOCl_2$ (fast); $NOCl_2 + NO \rightarrow 2NOCl$ (slow)

An elementary reaction between $A$ and $B$ is a second order reaction. Which of the following rate equations must be correct?

$A \rightarrow$ products ($1^{st}$ order reaction). Three sets of experiment were performed for a reaction under similar experimental conditions. Run $1 \Rightarrow 100 \ mL$ of $10 \ M$ solution of reactant $A$. Run $2 \Rightarrow 200 \ mL$ of $10 \ M$ solution of reactant $A$. Run $3 \Rightarrow 100 \ mL$ of $10 \ M$ solution of reactant $A + 100 \ mL$ of $H_2O$ added. The correct variation of rate of reaction is:

The given data are for the reaction:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$

Experiment	$[Cl_2] \ (M)$	$[NO] \ (M)$	Rate $(mol \ L^{-1} \sec^{-1})$
$I$	$0.05$	$0.05$	$1 \times 10^{-3}$
$II$	$0.15$	$0.05$	$3 \times 10^{-3}$
$III$	$0.05$	$0.15$	$9 \times 10^{-3}$

The rate law for the reaction is:

For the reaction $A \to xP$,when $[A] = 2.2 \, mM$,the rate was found to be $2.4 \, mM \, s^{-1}$. On reducing the concentration of $A$ to half,the rate changes to $0.6 \, mM \, s^{-1}$. The order of reaction with respect to $A$ is

Total order of reaction $X + Y \rightarrow XY$ is $3$. The order of reaction with respect to $X$ is $2$. State the differential rate equation for the reaction.