The iodine "clock reaction" involves the following sequence of reactions occurring in a reaction mixture in a single beaker. IO₃(aq) + 5I^-(aq) + 6H⁺(aq) → 3I₂(aq) + 3H₂O(l)
I₂(aq) + 2S₂O₃²^-(aq) → 2I^-(aq) + S₄O₆²^-(aq)
The molecular iodine (I₂) formed in reaction 1 is immediately used up in reaction 2, so that no iodine accumulates. In one experiment, a student made up a reaction mixture which initially contained 0.0020 mol of iodate ions (IO₃⁻) . If the iodate ions reacted completely, how many moles of thiosulfate ions (S₂O₃²⁻) were needed in reaction 2, in order to react completely with the iodine (I₂) produced in reaction 1?

Question

Quizplus · Accepted Answer

The Answer of The iodine "clock reaction" involves the following sequence of reactions occurring in a reaction mixture in a single beaker. IO₃(aq) + 5I^-(aq) + 6H⁺(aq) → 3I₂(aq) + 3H₂O(l) I₂(aq) + 2S₂O₃²^-(aq) → 2I^-(aq) + S₄O₆²^-(aq) The molecular iodine (I₂) formed in reaction 1 is immediately used up in reaction 2, so that no iodine accumulates. In one experiment, a student made up a reaction mixture which initially contained 0.0020 mol of iodate ions (IO₃⁻). If the iodate ions reacted completely, how many moles of thiosulfate ions (S₂O₃²⁻) were needed in reaction 2, in order to react completely with the iodine (I₂) produced in reaction 1? A)0.0020 mol B)0.012 mol C)0.0040 mol D)0.0010 mol E)0.0060 mol

The Iodine "Clock Reaction" Involves the Following Sequence of Reactions