The Iodine Clock Reaction

Topics: Chemical kinetics, Chemical reaction, Reaction rate Pages: 3 (824 words) Published: April 24, 2013
Chemical Kinetics: The Iodine-Clock Reaction: S2O82−(aq) + 2 I−(aq) → I2(aq) + 2 SO42−(aq) To measure the rate of this reaction we must measure the rate of concentration change of one of the reactants or products. Here, it is convenient to carry out a clock reaction involving the product I2. To do this, you will include (to the reacting S2O82− and I−) i) a small (but accurately known) amount of sodium thiosulfate, Na2S2O3, and ii) some starch indicator. The added Na2S2O3 does not interfere with the rate of above reaction, but it does consume the I2 as soon as it is formed (see below):

2 S2O32−(aq) + I2(aq) → S4O62−(aq) + 2 I−(aq) This reaction is much faster than the previous, so the conversion of I2 back to I− is essentially instantaneous. In a typical experiment, known concentrations of S2O82- and I− are mixed with a small amount of S2O32- and starch. As reaction the first proceeds, S2O82- and I− react to produce I2, but nothing appears to be happening because the second reaction is consuming the I2 as quickly as it is formed. The important moment is when the S2O32- runs out, for then the I2 is no longer consumed (see the second reaction), and the dark blue starch−I2 complex forms. The stoichiometry of the second reaction indicates that one I2 molecule must have been generated for every 2 ions of S2O32 − initially present in the solution. [I2 ] generated(from first reaction) = [I2 ] consumed(in second reaction) = {1/2[S2O32-] initially present} Note that the change in concentration of I2 (before the blue complex forms) is fixed by amount of S2O32- included in the initial reaction mixture. 1 [ S O2 − ] d [ I2 ] 2 2 3 rate = = dt t Where t = time for blue color to appear. In this experiment you will: A. Determine Rate Law and Rate Constant {k is constant at constant temperature} B. Vary temperature and estimate EA {Using the Arrhenius Equation} A. Determining the rate constant (k) and the rate law for the iodine-clock reaction:

We know [S2O82-] and [I-],...
Continue Reading

Please join StudyMode to read the full document

You May Also Find These Documents Helpful

  • To Observe the Effect of Temperature on the Rate of the Iodine Clock Reaction Using Ammonium Persulfate Essay
  • Section 1 Harcourt-Essen Reaction Essay
  • Iodine-Clock Reaction Essay
  • The Iodine Clock Reaction Essay
  • Formal Report- Kinetics of Reaction: the Iodine Clock Reaction Essay
  • Chemical Kinetics The Iodine Clock Reaction Essay
  • Essay on Chemical Kinetics: the Iodine-Clock Reaction
  • Kinetics: Iodine Clock Reaction Essay

Become a StudyMode Member

Sign Up - It's Free