Question

The reaction $F_2\left(g\right)+2Cl{O}_2\left(g\right)\Rightarrow 2FeCl{O}_2\left(g\right)$ is first order in each of the reactants. The rate of the reaction is $4.88\times {10}^{-4}M/s$, when [$F_2$] = 0.015M and [$Cl{O}_2$] = 0.025 M. Calculate the rate constant of the reaction.

Answer 1

$-\frac{dR}{dt}=k\left[F_2\right]\left[Cl{O}_2\right]$

$-\frac{dR}{dt}=4.88\times {10}^{-4}M/s$

$\left[F_2\right]=0.015M,\left[Cl{O}_2\right]=0.025M$

$4.88\times {10}^{-4}=K\times 0.015\times 0.025$

$k=\frac{4.88\times {10}^{-4}}{0.015\times 0.025}=1.301m^{-1}{s}^{-1}$