In the below given hypothetical equation

\(r = k[A]^x[B]^y\)

If the concentration of [B] is kept constant and concentration of [A] is increased to 3 times, the reaction rate increases 27 times, then the order of reaction with respect to A is

3

The correct answer is option 1. 3.

To determine the order of the reaction with respect to A, we can use the given information about how the reaction rate changes when the concentration of A is increased. According to the equation:

\[ r = k[A]^x[B]^y \]

If the concentration of B is kept constant and the concentration of A is increased to 3 times, and the reaction rate increases 27 times, it means:

\[ (k[3A]^x[B]^y) = 27(k[A]^x[B]^y) \]

\[ 3^x = 27 \]

\[ x = 3 \]

So, the order of the reaction with respect to A is 3.