For the following homogeneous reaction scheme,the rate constant has units for the reaction $A + B \xrightarrow{K} C$:

For the reaction $A \to B$,the rate increases by a factor of $2.25$ when the concentration of $A$ is increased by $1.5$. What is the order of the reaction?

For the reaction $A + B \rightarrow C$,we have the following data:

Initial concentration of $A$ $(M)$	Initial concentration of $B$ $(M)$	Initial Rate $(M \cdot s^{-1})$
$1$	$10$	$100$
$1$	$1$	$1$
$10$	$1$	$10$

The order of the reaction with respect to $A$ and $B$ are:

Which one of the following statements regarding the order of a reaction is not correct?

For the reaction $X_{2(g)} + Y_{2(g)} \rightarrow 2XY_{(g)}$,the following data are observed:

$[X_{2}] \ (M)$	$[Y_{2}] \ (M)$	Rate of appearance of $XY \ (M \ sec^{-1})$
$0.1$	$0.1$	$5 \times 10^{-6}$
$0.2$	$0.1$	$10^{-5}$
$0.2$	$0.2$	$4 \times 10^{-5}$

Calculate the rate constant of the reaction (in $M^{1-n} \ sec^{-1}$),where $n$ is the order of the reaction.

Inversion of cane sugar in dilute acid (conversion into glucose and fructose) is a: