For the reaction $A\to B$ , the rate law expression is  $-\frac{d\left[A\right]}{dt}=k{\left[A\right]}^{1/2}$. If initial concentration of A is  $A_0$. Which of the following statement is/are correct regarding this reaction?

There is a linear decrease of rate of reaction with time

The integrated form of rate expression is  $\sqrt{A}=\frac{-Kt}{2}+\sqrt{A_0}$

The half life period is  $t_{1/2}=\frac{\sqrt{2}(\sqrt{2}-1)}{K}\sqrt{A_0}$

The plot of $\sqrt{A}$  against ‘t’ will be non-linear.