Determine the rate of a reaction that follows the rate law rate kAmBn where k 1 and Atilde and 151 10-2 A 2 M B 3 M m 2 n 1?

To determine the rate of the reaction following the rate law ( \text{rate} = k[A]^m[B]^n ), with ( k = 1 ), ( m = 2 ), and ( n = 1 ), we can substitute the concentrations of A and B. Given ( [A] = 1.51 \times 10^{-2} , \text{M} ) and ( [B] = 3 , \text{M} ), the rate is calculated as follows:

[ \text{rate} = 1 \times (1.51 \times 10^{-2})^2 \times (3)^1 = 1 \times (2.2801 \times 10^{-4}) \times 3 = 6.8403 \times 10^{-4} , \text{M/s}. ]

Thus, the rate of the reaction is approximately ( 6.84 \times 10^{-4} , \text{M/s} ).