For a reaction $A + B \rightarrow \text{product}$,if $[A]$ is doubled keeping $[B]$ constant,the rate of reaction doubles. Calculate the order of reaction with respect to $A$.

Which of the following rate laws has an overall order of $0.5$ for a reaction involving substances $x$,$y$,and $z$?

For a reaction $2A + B \to \text{Products}$,doubling the initial concentration of both the reactants increases the rate by a factor of $8$,and doubling the concentration of $B$ alone doubles the rate. The rate law for the reaction is

For a zero order reaction,will the molecularity be equal to zero? Explain.

If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction increases $100$ times. What is the order of reaction if the rate law is $r = k[A]^x$?

For a chemical reaction,$m A \rightarrow x B$,the rate law is $r = k[A]^{2}$. If the concentration of $A$ is doubled,the reaction rate will be,