The rate constant for a second order reaction,$A \rightarrow \text{Product}$ is $1.62 \ M^{-1} \ s^{-1}$. What will be the rate of reaction when concentration of reactant is $2 \times 10^{-3} \ M$ (in $M \ s^{-1}$)?

For a chemical reaction $A \rightarrow B$,the rate of the reaction is $2 \times 10^{-3} \ mol \ dm^{-3} \ s^{-1}$,when the initial concentration is $0.05 \ mol \ dm^{-3}$. The rate of the same reaction is $1.6 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$ when the initial concentration is $0.1 \ mol \ dm^{-3}$. The order of the reaction is

In a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:

The following graph shows how $T_{1/2}$ (half-life) of a reactant $R$ changes with the initial reactant concentration $a_0$. The order of the reaction will be:

........ of a reaction cannot be determined experimentally.

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?