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

The rate law for the reaction $RCl + NaOH_{(aq)} \to ROH + NaCl$ is given by $\text{Rate} = K_1[RCl]$. The rate of the reaction will be

The units for the rate constant and the rate of reaction are same for a reaction. What will be the order of the reaction?

Which of the following statements about the rate constant is $NOT$ true?

If a reaction occurs in the following two steps:
$i) \ 2 ClO^{-} \rightarrow ClO_2^{-} + Cl^{-}$
$ii) \ ClO_2^{-} + ClO^{-} \rightarrow ClO_3^{-} + Cl^{-}$
Find the reaction intermediate.

In a chemical reaction $A$ is converted into $B$. The rates of reaction,starting with initial concentrations of $A$ as $2 \times 10^{-3} \ M$ and $1 \times 10^{-3} \ M$,are equal to $2.40 \times 10^{-4} \ M s^{-1}$ and $0.60 \times 10^{-4} \ M s^{-1}$ respectively. The order of reaction with respect to reactant $A$ will be