The following mechanism had been proposed for the reaction of H$_2$(g) and ICI(g). 1. H$_2$(g) + ICI(g) $\rightarrow$ HI(g) + HCI(g) slow 2. HI(g) + ICI(g) $\rightarrow$ I$_2$(g) + HCl(g) fast H$_2$(g) + 2ICI(g) $\rightarrow$ I$_2$(g) + 2HCI(g) The intermediate in this reaction is: OH$_2$ OICI OHCI HI OI$_2$
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Susan H.
The following mechanism has been proposed for the gasphase reaction of $\mathrm{H}_{2}$ with ICl: $$\begin{array}{c}{\mathrm{H}_{2}(g)+\mathrm{ICl}(g) \longrightarrow \mathrm{HI}(g)+\mathrm{HCl}(g)} \\ {\mathrm{HI}(g)+\mathrm{ICl}(g) \longrightarrow \mathrm{I}_{2}(g)+\mathrm{HCl}(g)}\end{array}$$ $\begin{array}{l}{\text { (a) Write the balanced equation for the overall reaction. }} \\ {\text { (b) Identify any intermediates in the mechanism. (c) If }}\end{array}$ the first step is slow and the second one is fast, which rate law do you expect to be observed for the overall reaction?
The elementary reaction: 2 HCl → H2 + Cl2, is an example of a bimolecular reaction. A three-step mechanism has been suggested for the formation of COI2: Step 1: I2 → 2 I Step 2: I + CO → COI Step 3: COI + I2 → COI2 + I Which species is an intermediate in the mechanism? COI2, CO, COI, I
Sri K.
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