Which will be the unit of rate constant for the reaction having Rate $= K[A]^{\frac{1}{2}} \cdot [B]^{\frac{3}{2}}$ ?

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

Which of the following statements regarding the molecularity of a reaction is wrong?

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: $[A] = 1 \ mol \ L^{-1}, [B] = 0.25 \ mol \ L^{-1}$.

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:

Entry	$[A]$ in $M$	$[B]$ in $M$	Initial rate $(M/s)$
$1$	$0.02$	$0.02$	$2 \times 10^{-2}$
$2$	$0.02$	$0.04$	$4 \times 10^{-2}$
$3$	$0.04$	$0.04$	$8 \times 10^{-2}$

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