Submitted by: Submitted by beke
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Pages: 7
Category: Science and Technology
Date Submitted: 05/29/2013 04:07 PM
Name: Beklau Abebe
5/8/2013
Iodine Clock
Abstract: The purpose of this lab is to determine the orders of reaction and the rate constant of reaction between I- and S2O82- and to examine the effect of catalyst.
Chemical Equations:
3 I-(aq) + S2O82-(aq) I3-(aq) + 2 SO42-(aq)
I3-(aq) + 2 S2O32-(aq) 3 I-(aq) + S4O62-(aq)
I3-(aq) + Starch(aq) Starch—I3- complex
Formulae:
Rate = k[reactant 1]a[reactant 2]b[reactant 3]c…
where: k: rate constant
[reactant 1/2/3/…]: concentration of reactant 1/2/3/…
a/b/c/…: order of reaction with respect to each reactant
k = Ae-Ea/RT or ln k= -EaR1T + ln A
where: A: Arrhenius proportionality factor (unique to each reaction)
R: Universal constant
T: Temperature
Ea: Activation energy
Objective: To understand the orders of reaction and the rate constant
Procedure: Sodium meta-bisulfite (Na2S2O5) undergoes the following transformation when dissolved in water where it dissolves and reacts with the water to form bisulfite (HSO3-) :
Na2S2O5 + H2O --- > 2HSO3-+ 2Na+
When mixed with potassium iodate (KIO3) the following reaction mechanism is proposed leading to the observed color change:
1. Data and calculations:
Table 1. Rates of reactions |
| Trial | [I-]o (M) | [S2O82-]o (M) | Time 1 (s) | Time 2 (s) | Average time (s) | Δ[S2O82-] (M) | Rate (M/s) |
Part A | 1 | 0.084 | 0.042 | 26.5 | 25.7 | 26.1 | 6.3E-04 | 2.4E-05 |
| 2 | 0.042 | 0.042 | 57.6 | 49.0 | 53.3 | 6.3E-04 | 1.2E-05 |
| 3 | 0.021 | 0.042 | 97.7 | 90.2 | 94.0 | 6.3E-04 | 6.7E-06 |
| 4 | 0.011 | 0.042 | 195.3 | 185.6 | 190.5 | 6.3E-04 | 3.3E-06 |
Part B | 5 | 0.042 | 0.084 | 22.8 | 22.8 | 22.8 | 6.3E-04 | 2.8E-05 |
| 6 | 0.042 | 0.042 | 47.2 | 51.2 | 49.2 | 6.3E-04 | 1.3E-05 |
| 7 | 0.042 | 0.021 | 88.3 | 94.5 | 91.4 | 6.3E-04 | 6.9E-06 |
| 8 | 0.042 | 0.011 | 159.9 | 160.3 | 160.1 | 6.3E-04 | 3.9E-06 |
Part C | 9 | 0.042 |...