Study on Activation Energy of Ethyl Acetate Saponification Reaction
1. Introduction
The rate of chemical reaction is affected by many factors, among which activation energy is one of the key factors determining the reaction rate. In many chemical reaction studies, ethyl acetate saponification reaction is often used to explore reaction kinetics and activation energy related issues because of its relatively simple and typical reaction process. The study of Activation Energy of Ethyl Acetate Saponification is helpful to deeply understand the mechanism of the reaction and the influence of temperature and other factors on the reaction rate, and then provide theoretical support for related industrial production and chemical research.

Second, experimental principle
The saponification of ethyl acetate is a typical second-order reaction, and its reaction equation is: $CH_3COOC_2H_5 + NaOH\ longrightarrow CH_3COONa + C_2H_5OH $. During the reaction, since the conductivity of $OH ^ - $ions is much greater than that of $CH_3COO ^ - $ions, the conductivity of the solution gradually decreases as the reaction proceeds. By measuring the change of conductivity of the solution at different times, combined with the second-order reaction kinetic equation, the relationship between the reaction rate constant $k $and the temperature $T $can be deduced, and then according to the Arrhenius formula $k = A e ^ {-\ frac {E_a} {RT}} $ (where $E_a $is the activation energy, $A $is the pre-index factor, $R $is the gas constant, and $T $is the absolute temperature) The activation energy of the saponification reaction of ethyl acetate is calculated.

III. Experimental materials and methods
1. ** EXPERIMENTAL MATERIALS **
-Ethyl acetate (analytical purity)
-Sodium hydroxide (analytical purity)
-Distilled water
-Conductivity meter
-Thermostatic water bath pot
-Glass instruments such as pipettes and volumetric bottles
2. ** EXPERIMENTAL METHODS **
- * Solution Preparation **: Accurately prepare a certain concentration of ethyl acetate solution and sodium hydroxide solution.
- ** Conductivity Measurement **: Adjust the thermostatic water bath pot to different temperatures, and measure the conductivity of the reaction system at different times at the beginning of the reaction and during the reaction at different temperatures in turn.
- ** Data recording and processing **: Record the conductivity of each measurement and the corresponding time, process the data according to the second-order reaction kinetic equation and Arrhenius formula, and calculate the reaction rate constant at different temperatures $k $, and then obtain the activation energy of the saponification reaction of ethyl acetate.

IV. Experimental results and discussion
1. ** Experimental results **
The rate constants of ethyl acetate saponification at different temperatures were obtained by experimental measurement and data processing, as shown in the following table:

| temperature ($T $, $K $) | rate constants ($k $, $L\ cdot mol ^ {-1}\ cdot s ^ {-1} $) |
|---|---|
| $T_1 $| $k_1 $|
| $T_2 $| $k_2 $|
| $\ cdots $| $\ cdots $|

as $\ ln k $vs $\ frac {1} {T} $ Figure, a straight line is obtained, and the activation energy of ethyl acetate saponification reaction is calculated according to the slope of the straight line $-\ frac {E_a} {R} $.
2. ** RESULTS DISCUSSION **
The activation energy values obtained by the experiment are compared with the theoretical values or other reported values in the literature to analyze possible sources of error. Errors may come from the accuracy of the experimental instrument, errors in the preparation process of the solution, fluctuations in temperature control, and deviations from the ideal state of the reaction system. For example, the measurement error of the conductivity meter may lead to inaccurate conductivity data, thus affecting the calculation of the reaction rate constant; Minor fluctuations in the temperature of the constant temperature water bath may make the actual reaction temperature different from the set temperature, which in turn affects the experimental results. Through the analysis of the error, it provides a reference for further optimizing the experimental method and improving the experimental accuracy.

5. Conclusion
In this experiment, by measuring the conductivity change of the ethyl acetate saponification reaction system at different temperatures, the activation energy of the ethyl acetate saponification reaction was successfully calculated by using the second-order reaction kinetic equation and Arrhenius formula. Although there are certain errors in the experimental process, through the analysis and discussion of the experimental results, the source of the errors is clarified, which provides experience and reference for subsequent related research. Accurate determination of the activation energy of the saponification reaction of ethyl acetate is helpful to further understand the kinetic characteristics of the reaction, and provides a theoretical basis for the process optimization of such reactions in the chemical industry.