Question

For the reaction 2A + B + C $\to A_{2}B$ + C the rate law is found to be Rate =k[A][B]${}^2$ with $k=2\times {10}^{-6}mo{l}^{-2}{L}^2{s}^{-1}$
The initial rate of reaction with $\left[A\right]=0.1mol{L}^{-1},\left[B\right]=0.2mol{L}^{-1}and\left[C\right]=0.8mol{L}^{-1}$ is

• A. $6.4\times {10}^{-8}mol{L}^{-1}{s}^{-1}$
• B. $4\times {10}^{-3}mol{L}^{-1}{s}^{-1}$
• C. $8\times {10}^{-9}mol{L}^{-1}{s}^{-1}$
• D. $4\times {10}^{-7}mol{L}^{-1}{s}^{-1}$

Answer 1

The correct option is C $8\times {10}^{-9}mol{L}^{-1}{s}^{-1}$

$Rate=k\left[A\right][B{]}^2=(2\times {10}^{-6}\left)\right(0.1\left)\right(0.2{)}^2=8\times {10}^{-9}$