For a reaction $A \rightarrow \text{Product}$,the rate constant is $6.93 \times 10^{-3} \ hour^{-1}$. What is the order of the reaction?

The rate law for the reaction $RCl + NaOH_{(aq)} \to ROH + NaCl$ is given by $\text{Rate} = K_1[RCl]$. The rate of the reaction will be

For the chemical reaction $2O_3 \rightarrow 3O_2$,the mechanism is given below. What will be the rate law expression?
$O_3 \rightleftharpoons O_2 + O$ ...... (fast)
$O + O_3 \rightarrow 2O_2$ ...... (slow)

$A$ complex reaction takes place in the following steps:
$NO_2Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{(g)}$ (slow)
$NO_2Cl_{(g)} + Cl_{(g)} \longrightarrow NO_{2(g)} + Cl_{2(g)}$ (fast)
Identify the rate law equation for this reaction.

If $r = k[A]^2[B]$ is the rate law equation for the reaction $A + B \rightarrow C$,at $[A] = 1 \ M$ and $[B] = 0.2 \ M$,calculate the rate of reaction if the rate constant is $6.25 \ M^{-2} \ s^{-1}$. (in $M \ s^{-1}$)

The following results have been obtained during the kinetic studies of the reaction: $2 \ NO + 2 \ H_2 \longrightarrow N_2 + 2 \ H_2O$

Expt	$\frac{-d[NO]}{dt} \ (mol \ L^{-1} \ s^{-1})$	$[NO] \ (mol \ L^{-1})$	$[H_2] \ (mol \ L^{-1})$
$1$	$4.8 \times 10^{-5}$	$1 \times 10^{-2}$	$1 \times 10^{-3}$
$2$	$43.2 \times 10^{-5}$	$3 \times 10^{-2}$	$1 \times 10^{-3}$
$3$	$86.4 \times 10^{-5}$	$3 \times 10^{-2}$	$2 \times 10^{-3}$