The rate law for the decomposition of hydrogen iodide is $-\frac{d[HI]}{dt}=k[HI]^2$. The units of rate constant $k$ are

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 $0.5 \, M$?

For a reaction $A + B \to$ product,it was found that the rate of reaction increases four times if the concentration of $A$ is doubled,but the rate of reaction remains unaffected if the concentration of $B$ is doubled. Hence,the rate law for the reaction is

For a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:

The rate law for the reaction $A + B \rightarrow C$ at $25^{\circ} C$ is given by $\text{rate} = k[A][B]^2$. Calculate the rate of reaction if the rate constant at the same temperature is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$ where $[A] = 1 \ M$ and $[B] = 0.2 \ M$.

Which of the following statements is incorrect?