ClkRxn - Chem 6 LECTURE DEMONSTRATION#1(CLOCK REACTION The...

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Clock reaction 1 Chem 6 LECTURE DEMONSTRATION #1 (CLOCK REACTION) The aqueous reaction between two anions, peroxydisulfate (S 2 O 8 2– ) and thiosulfate (S 2 O 3 2– ), to form sulfate (SO 4 2– ) and dithionate (S 4 O 6 2– ) anions is accelerated by iodide (I ). In the course of the reaction, iodide is converted to triiodide (I 3 ) temporarily, then I 3 is returned to I . Consequently, I 3 is an intermediate and iodide is a catalyst . The net reaction is, therefore, S 2 O 8 2– + 2 S 2 O 3 2– 2 SO 4 2– + S 4 O 6 2– peroxydisulfate thiosulfate sulfate dithionate while the two reactions involving the consumption and re-generation of the catalyst are S 2 O 8 2– + 3 I 2 SO 4 2– + I 3 2 S 2 O 3 2– + I 3 S 4 O 6 2– + 3 I which, you’ll note, add to the net reaction. Our goal is to find the kinetic rate law, which we’ll assume has the general form Rate = d [S 2 O 8 2– ] dt = k [S 2 O 8 2– ] m [I ] n where k is the rate constant, and m and n are reaction order exponents .
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