What is the rate constant of a reaction if rate 0.2 mol L s A and B are each 3 M m 1 and n 2?

To find the rate constant ( k ) of the reaction, we can use the rate law equation:

[ \text{rate} = k [A]^m [B]^n ]

Given that the rate is 0.2 mol L⁻¹ s⁻¹, with concentrations ( [A] = 3 , \text{M} ), ( m = 1 ), ( [B] = 3 , \text{M} ), and ( n = 2 ), we can substitute these values into the equation:

[ 0.2 = k (3)^1 (3)^2 ]

This simplifies to:

[ 0.2 = k (3)(9) = 27k ]

Solving for ( k ), we find:

[ k = \frac{0.2}{27} \approx 0.00741 , \text{L}^2 \text{mol}^{-2} \text{s}^{-1} ]