CHEMISTRY 2020 Experiment 4: Kinetics of Nucleophilic Substitutions
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Course
CHEMISTRY 2020
Institution
CHEMISTRY 2020
CHEMISTRY 2020 Experiment 4: Kinetics of
Nucleophilic Substitutions
Chetna Raj June 14th, 2016
Chemistry 2020
Lab 3
Results
1. Determine the effect of varying [OH-] on the rate of the reaction. To do this, you should complete the following table:
Table 1: Reaction Rat...
Since the rate constants remained relatively similar with varying [OH -] concentrations; in other words, it
is independent of the rate law since it does not affect the rate to a great degree. In addition, because
this is an SN1 mechanism, it takes a great deal of energy to ionize the tertiary halide into a carbocation,
which is the slow step, hence the rate limiting step. The hydroxide ion is protic solvent and only helps to
stabilize the carbocation.
Calculations:
[tBuCl] = C2 = C1V1 /V2 = (3 mL × 0.1 mol/L) ÷ 10 mL = 0.03
Experiment 1: M [OH-] = 10% of 0.03M = 0.003 M
k = 2.303 log10 [1 / (1-χt)] ÷ t = 2.303 log10 [1 / (1-0.1)] ÷ 44 = 2.39 × 10-3 s-1
rate = k[tBuCl] = (2.39 × 10-3)(0.03) = 7.18 × 10-5 Ms-1
2. Determine the effect of varying [tBuCl] on the reaction rate. Completing the following table will
assist you.
What is the dependence of [tBuCl] on the rate law?
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