Chemistry, 11.04.2020 00:49 camillexv2668
Chlorine dioxide (ClO2) is a disinfectant in municipal water-treatment plants. It dissolves in basic solution, producing ClO3- and ClO2- according to the redox reaction: 2ClO2(g) + 2OH-(aq) ?ClO3-(aq) + ClO2-(aq) +H2O. The following kinetic data were obtained at 298 K for the reaction:
Expt # [ClO2]0, M [OH-]0, M Initial rate (M/s)
1 0.060 0.030 0.0248
2 0.020 0.030 0.00827
3 0.020 0.090 0.0247
Determine the rate law, overall order of reaction, and the rate constant for this reaction at 298 K.
Answers: 3
![\text{ rate = k[ClO$_{2}$][OH$^{-}$]; 2nd order; 138 M$^{-1}$s$^{-1}$}](/tpl/images/0594/7180/03545.png)
![\rm rate =k[ClO_{2}]^{m}[OH^{-}]^{n}](/tpl/images/0594/7180/25576.png)
![\begin{array}{cccl}\textbf{Expt} & \textbf{[ClO$_{2}]_{0}$/M} & \textbf{[OH$^{-}]_{0}$/M} & \textbf{rate/(M/s)}\\1 & 0.060 & 0.030 & 0.248\\2 & 0.020 & 0.030 & 0.00827\\3 & 0.020 & 0.090 & 0.0247\\\end{array}](/tpl/images/0594/7180/54044.png)
![\rm \dfrac{[ClO_{2}]_{1} }{[ClO_{2}]_{2}} = \dfrac{0.60}{0.00 } = 3.0 \approx 3\\\\\rm \dfrac{rate_{1}}{rate_{2}} = \dfrac{0.0248}{0.00827} = 3.00 \approx 3](/tpl/images/0594/7180/84e10.png)
![\rm rate =k[ClO_{2}][OH^{-}]^{n}](/tpl/images/0594/7180/7b1dd.png)
![\rm \dfrac{[ OH^{-}]_{3} }{[ OH^{-}]_{2}} = \dfrac{0.0900}{0.030 } = 3.0 \approx 3\\\\\rm \dfrac{rate_{3} }{rate_{2}} = \dfrac{0.0247}{0.00827} = 2.99 \approx 3](/tpl/images/0594/7180/a1053.png)
![\large \boxed{\textbf{ rate = k[ClO$_{2}$][OH$^{-}$]}}](/tpl/images/0594/7180/48fba.png)
![\begin{array}{rcl}\text{rate} &=& \text{[ClO$_{2}$][OH$^{-}]$}\\0.248 & = & k \rm \times 0.060 \times 0.030\\& = & k \times 1.8 \times 10^{-3}\\k & = & \dfrac{0.248}{1.8 \times 10^{-3}}\\\\ &=& \textbf{138 M$^{\mathbf{-1}}$s$^{\mathbf{-1}}$}\\\end{array}](/tpl/images/0594/7180/318a7.png)
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Chlorine dioxide (ClO2) is a disinfectant in municipal water-treatment plants. It dissolves in basic...
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