If the concentration of the reactants is increased,the rate of reaction

The rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?

Why can’t molecularity of any reaction be equal to zero?

Consider the plots for the types of reaction $nA \to B + C$. These plots respectively correspond to the reaction orders:

The half-lives of two samples are $0.1 \ s$ and $0.4 \ s$. Their respective concentrations are $200$ and $50$. What is the order of the reaction?

The rate of reaction,$A + B + C \longrightarrow P$ is given by
$r = K[A]^{1/2} [B]^{1/2} [C]^{1/4}$
The order of reaction is