Question

Be sure to answer all parts. Consider the following mechanism: (1) ClO−(aq) + H2O(l) ⇌ HClO(aq) + OH−(aq)  [fast] (2) I−(aq) + HClO(aq) → HIO(aq) + Cl−(aq)  [slow] (3) OH−(aq) + HIO(aq) → H2O(l) + IO−(aq)  [fast] (a) What is the overall equation? Select the single best answer.    ClO−(aq) + I−(aq) ⇌ IO−(aq) + H2O(l) + Cl−(aq)    ClO−(aq) + I−(aq) → IO−(aq) + H2O(l) + Cl−(aq)    ClO−(aq) + I−(aq) → IO−(aq) + Cl−(aq)    ClO−(aq) + I−(aq) ⇌ IO−(aq) + Cl−(aq) (b) Identify the intermediate(s), if any. Select the single best answer.    No intermediates    HClO, OH−, HIO, H2O    Cl−, OH−, I−, ClO−, IO−    HClO, OH−, HIO (c) What are the molecularity and the rate law for each step? Select the single best answers. (1):    unimolecular    bimolecular    termolecular rate =    k1[ClO−][H2O]    k1[HClO][OH−]    k1([HClO][OH−])/([HClO][OH−]) (2):    unimolecular    bimolecular    termolecular rate =    k2[HIO][Cl−]    k2[I−][HClO]    k2([HIO][Cl−])/([I−][HClO]) (3):    unimolecular    bimolecular    termolecular rate =    k3[OH−][HIO]    k3([H2O][IO−])/([OH−][HIO])    k3[H2O][IO−] (d) Is the mechanism consistent with the actual rate law: rate = k[ClO−][I−]?    yes    no

Answer 1

Please let me know if you have any doubt. Thanks