For the reaction $2A + B \rightarrow \text{product}$,the rate of the reaction is $15 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$ when $[A] = 0.3 \ mol \ dm^{-3}$ and $[B] = 0.05 \ mol \ dm^{-3}$. What is the value of the rate constant if the reaction is first order in both the reactants?

The unit of the rate constant for a second-order reaction is ......

The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is

For a reaction $A \longrightarrow P$,a plot between $[A]_0$ $Vs$ $\frac{1}{t_{1/2}}$ is a straight line having a positive slope. When the initial concentration is $1 \times 10^{-2} \ M$,its half-life period is found to be $20 \ min$. When the concentration of $A$ is $2 \times 10^{-2} \ M$,then the half-life will be (in $min$)?

What will be the overall order of a reaction for which the rate expression is given as $Rate = K[A]^{\frac{1}{2}}[B]^{\frac{3}{2}}$?

For a second-order reaction,the rate constant is $8 \times 10^{-5} \, M^{-1} \, \text{min}^{-1}$. In how much time will a $1 \, M$ solution decrease to $0.5 \, M$?