For a reaction,$A + B \rightarrow \text{Product}$; the rate law is given by,$r = k[A]^{1/2}[B]^2$. What is the order of the reaction?

$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is:

In the reaction $A + B \to \text{Products}$,the initial concentration of both $A$ and $B$ is $0.1 \, M$. When the concentration decreases to $1.0 \times 10^{-2} \, M$,the half-life period increases by ten times. The rate of the reaction is:

For a reaction involving substances $x$,$y$,and $z$,if the overall order of the reaction is $0.5$,which of the following rate laws is applicable?

What is rate law? Give a relation between rate of reaction and concentration of reactants.

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