The saponification (hydrolysis) of ethyl acetate occurs according to the stoichiometric relation CH3COOC2H5 + OH- → CH3COO- + C2H5OH. The reaction can be followed by monitoring the disappearance of OH-. The following experimental results were obtained at 25 °C:
Initial concentration | Initial concentration | Half-life, tVi, s |
of OH- (M) | of CH3COOC2H5 (M) | |
0.0050 | 0.0050 | 2000 |
0.0100 | 0.0100 | 1000 |
There is no significant dependence on the concentrations
of products of the reaction.
a. What is the overall kinetic order of the reaction?
b. Calculate a value for the rate coefficient, including appropriate units.
c. How long would it take for the concentration of OH- to reach 0.0025 M for each experiment?
d. Based on your answer to part (a), what are possible rate laws for this reaction?
e. Carefully describe a single experiment that would enable you to decide which of the possibilities of part (d) is most nearly correct.
We need at least 10 more requests to produce the solution.
0 / 10 have requested this problem solution
The more requests, the faster the answer.