If the rate of reaction is given by $Rate = K [A]^{3/2} [B]^{-1/2}$,then find the order of the reaction.

Identify the order of reaction for which the unit of the rate constant is $\text{mol dm}^{-3} \text{s}^{-1}$.

The rate law for the decomposition of hydrogen iodide is $-\frac{d[HI]}{dt}=k[HI]^2$. The units of rate constant $k$ are

The experimental data for the reaction $2A + B_2 \longrightarrow 2AB$ is given below:

Exp.	$[A] \ (mol \ L^{-1})$	$[B_2] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ S^{-1})$
$1$	$0.50$	$0.50$	$1.6 \times 10^{-4}$
$2$	$0.50$	$1.00$	$3.2 \times 10^{-4}$
$3$	$1.00$	$1.00$	$3.2 \times 10^{-4}$

Determine the rate law for the reaction.

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

Which of the following statements is incorrect?