For a reaction $r = k[A][B]^2$,if the concentration of $A$ is doubled,the rate of reaction:

The alkaline hydrolysis of ethyl acetate is represented by the equation $CH_3COOC_2H_5 + NaOH \to CH_3COONa + C_2H_5OH$. Experimentally,it is found that for this reaction $\frac{dx}{dt} = k[CH_3COOC_2H_5][NaOH]$. Then the reaction is

For the reaction, $A + B \rightarrow P$, the rate law is $\text{rate} = k[A][B]^2$. The rate of reaction is $0.25 \text{ Ms}^{-1}$ when $[A] = 1 \text{ M}$ and $[B] = 0.2 \text{ M}$ at $25^\circ \text{C}$. Calculate the rate constant $k$ of the reaction at the same temperature.

Consider the plots,given below,for the reaction $A \rightarrow B + C$. The plots respectively correspond to the reaction order:

For a reaction $A \rightarrow 2 B + C$ the half-lives are $100 \ s$ and $50 \ s$ when the concentration of reactant $A$ is $0.5 \ mol \ L^{-1}$ and $1.0 \ mol \ L^{-1}$ respectively. The order of the reaction is (Nearest Integer).

For the reaction $A + B \to$ products,doubling the concentration of $A$ the rate of the reaction is doubled,but on doubling the concentration of $B$ the rate remains unaltered. The overall order of the reaction is: