What is the order of the following reaction: $2H_2O_2(l) \rightarrow 2H_2O(l) + O_2(g)$, given that the rate law is $\text{rate} = k[H_2O_2]^1$?

The data for the reaction $A + B \to C$ is given below:

$Exp$	$[A]_0$	$[B]_0$	Initial Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.035$	$0.80$
$3$	$0.012$	$0.070$	$0.10$
$4$	$0.024$	$0.070$	$0.80$

Determine the rate law for the reaction.

For the reaction $A + B \longrightarrow \text{product}$,the rate law equation is $\text{rate} = k[A]^2[B]$. If the rate of reaction is $0.22 \ mol \ L^{-1} \ s^{-1}$,calculate the rate constant $k$. Given: $[A] = 1 \ mol \ L^{-1}, [B] = 0.25 \ mol \ L^{-1}$.

Which one of the following is a second order reaction?

The rate law for the reaction $A + 2B \rightarrow C + 2D$ is given by:

For a certain reaction,the rate $= k[A]^2[B]$. When the initial concentration of $A$ is tripled keeping the concentration of $B$ constant,the initial rate would: