What is the order of the following reaction: $2H_2O_2(l) \rightarrow 2H_2O(l) + O_2(g)$, given that the rate law is $\text{rate} = k[H_2O_2]^1$?

For a reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $2$ and with respect to $B$ is $3$. If the concentration of both is doubled,by how much will the rate increase?

For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:

For the reaction,$H_{2(g)} + Br_{2(g)} \longrightarrow 2 HBr_{(g)}$,$r = k[H_2][Br_2]^{\frac{1}{2}}$. What is the molecularity and order of reaction respectively?

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

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