A reaction : $2A\left(g\right)+3B\left(g\right)⟶C\left(g\right)$ obeys the following rate law, Rate of reaction $=\left[A{]}^3\right[B{]}^{-2}$.

Select the incorrect options.

If 'B' is taken in very large amount as compared to 'A' then half life of the reaction will be inversely dependent on cube of its initial concentration.

The reaction will occur in a single step.

If both 'A' and 'B' are taken in equal concentration then half life will be dependent on their concentration.

If concentration of 'A' and 'B' both are doubled then rate will increase to double the original value.