$A$ reaction is first order in terms of $A$ and second order in terms of $B$. What will be the rate of reaction,if the concentration of $B$ is increased two times?

The order of a reaction is said to be $2$ with respect to a reactant $X$,when

If the reaction between $A$ and $B$ to give $C$ shows first-order kinetics in $A$ and second-order in $B$,the rate equation can be written as:

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 reaction,$A + B \longrightarrow \text{product}$,it is found that the rate law is $r = k[A]^{1.5}[B]^{2.5}$. What is the order of reaction?

The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.