The reaction of chloromethane (CH3Cn with the hydroxide ion yields methanol (CH3OH) and the chloride ion: CH3Cl + OH- >CH3OH + Cl-
The generic rate law for the reaction is written as
R = k[CH3Cl]x[OH-]y
However, given a relatively large concentration of hydroxide ion, as in Experiments #1 - #3 (below), the rate law can be written as: R = k'[CH3Cl]*
a. Determine the order with respect to the chloromethane by producing the three integrated rate law plots ([CH3Cl], Ln[CH3Cl] and 1/[CH3Cl]t versus time) for all three experiments (Attach all 9 plots and relevant spreadsheets).
Experiment #1 at 61 °Cl Experiment #2 at 61 °C Experiment #3 at 61 °C
Time, min [CH3CI], M Time, min [CH3CI], M Time, min [CH3CI], M
3.0 9.1 x 10-4 3.0 7.6 x 10-4 3.0 6.2 x 10-4
6.0 8.4 x 10-4 6.0 5.7 x 10-4 6.0 3.9 x 10-4
9.0 7.6 x 10-4 9.0 4.4 x 10-4 9.0 2.4 x 10-4
12.0 7.0 x 10-4 12.0 3.3 x 10-4 12.0 1.5 x 10-4
15.0 6.4 x 10-4 15.0 2.5 x 10-4 15.0 9.2 x 10-5
18.0 5.8 x 10-4 18.0 1.9 x 10-4 18.0 5.7 x 10-5
21.0 5.3 x 10-4 21.0 1.4 x 10-4 21.0 3.5 x 10-5
24.0 4.9 x 10-4 24.0 1.1 x 10-4 24.0 2.2 x 10-5
27.0 4.5 x 10-4 27.0 8.3 x 10-5 27.0 1.4 x 10-5
30.0 4.1 x 10-4 30.0 6.3 x 10-5 30.0 8.5 x 10-6