The rate of reaction between $A$ and $B$ increases by a factor of  $100,$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is

units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

The mechanism of the reaction $A + 2B \to  D$ is

$2B\xrightarrow{k}{B_2}\,\left[ {Slow} \right]$

${B_2} + A \to D\,\left[ {Fast} \right]$

The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order of reaction are respectively

For a chemical reaction,$ A + 2B \to C + D,$ the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\,times,$ then rate of reaction also increases $2\,times$. The order of this reaction is

In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$  torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$

For the reaction $A \to B$, the rate law expression is : Rate $ = \,k\,[A]$ Which of the following statements is incorrect