For a chemical reaction,$m A \rightarrow x B$,the rate law is $r = k[A]^{2}$. If the concentration of $A$ is doubled,the reaction rate will be,

The following data was obtained for the chemical reaction given below at $975 \ K$: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$

Experiment	$[NO] \ (mol \ L^{-1})$	$[H_{2}] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ s^{-1})$
$1$	$8 \times 10^{-5}$	$8 \times 10^{-5}$	$7 \times 10^{-9}$
$2$	$24 \times 10^{-5}$	$8 \times 10^{-5}$	$2.1 \times 10^{-8}$
$3$	$24 \times 10^{-5}$	$32 \times 10^{-5}$	$8.4 \times 10^{-8}$

The order of the reaction with respect to $NO$ is ..... .

In a reaction involving hydrolysis of an organic chloride in the presence of a large excess of water,$RCl + H_2O \to ROH + HCl$.

The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the

The rate law for the reaction,$NO_{2(g)} + CO_{(g)} \rightarrow NO_{(g)} + CO_{2(g)}$ is given as $R = k[NO_2]^2$. What is the order of reaction with respect to $CO$?

For the reaction,$2A + B \to \text{products}$,when the concentrations of $A$ and $B$ both were doubled,the rate of the reaction increased from $0.3 \ mol \ L^{-1} \ s^{-1}$ to $2.4 \ mol \ L^{-1} \ s^{-1}$. When the concentration of $A$ alone is doubled,the rate increased from $0.3 \ mol \ L^{-1} \ s^{-1}$ to $0.6 \ mol \ L^{-1} \ s^{-1}$. Which one of the following statements is correct?