INTRODUCTION THE ACTIVATION ENERGY OF THE REACTION OF ETHYLETHE ACETATE WITH SODIUM HYDROXIDE
I. INTRODUCTION The activation energy of a chemical reaction is one of the key factors determining the reaction rate. For the reaction of ethyl acetate with sodium hydroxide, it is essential to clarify its activation energy in order to deeply understand the kinetic process of the reaction. The purpose of this study is to accurately determine the activation energy of the reaction of ethyl acetate with sodium hydroxide through reasonable experimental design and theoretical analysis.

Second, experimental principle
The reaction of ethyl acetate with sodium hydroxide is a typical second-order reaction, and the reaction equation is as follows:
\ (CH_ {3} COOC_ {2} H_ {5} + NaOH\ longrightarrow CH_ {3} COONa + C_ {2} H_ {5} OH\)
According to the Arrhenius formula:\ (k = A e ^ {-\ frac {E_ {a}} {RT}}\) (where\ (k\) is the reaction rate constant,\ (A\) is the pre-exponential factor,\ (E_ {a}\) is the activation energy,\ (R\) is the molar gas constant,\ (T\) Absolute temperature). Take the logarithm of this equation to get:\ (\ lnk = -\ frac {E_ {a}} {RT} +\ lnA\). By measuring the reaction rate constant\ (k\) at different temperatures and plotting\ (\ lnk\) against\ (\ frac {1} {T}\), a straight line can be obtained, the slope of the straight line is\ (-\ frac {E_ {a}} {R}\), from which the activation energy of the reaction can be calculated\ (E_ {a}\).

3. Experimental Methods
1. ** Reagents and Instruments **
- ** Reagents **: ethyl acetate, sodium hydroxide, phenolphthalein indicators, etc. The reagents used are all analytically pure.
- ** Instrument **: Thermostatic water bath, magnetic stirrer, conductivity meter, pipette, volumetric flask, etc.
2. ** Experimental steps **
- ** Solution preparation **: Accurately prepare a certain concentration of ethyl acetate solution and sodium hydroxide solution.
- ** Determination of reaction rate constants at different temperatures **: Adjust the thermostatic water bath to different temperatures, followed by\ (T_ {1}\),\ (T_ {2}\),\ (T_ {3}\), etc. At each temperature, quickly mix equal volumes of ethyl acetate solution and sodium hydroxide solution, put them in a preheated reaction vessel, turn on the magnetic stirrer, and measure the change of the conductivity of the reaction system with time with a conductivity meter. Since sodium hydroxide is a strong electrolyte in this reaction, the concentration of ions in the solution changes before and after the reaction, resulting in the change of conductivity. Through the relationship between conductivity and time, the reaction rate constants at different temperatures are calculated by the second-order reaction kinetics formula\ (k_ {1}\),\ (k_ {2}\),\ (k_ {3}\), etc.

IV. Experimental results and analysis
1. ** DATA RECORD **
Record different temperatures\ (T\) and corresponding reaction rate constants\ (k\) as shown in the following table:
|\ (T (K )\) | \(\ frac {1} {T} (K ^ {-1 })\) | \( k (mol ^ {-1} · L · min ^ {-1 })\) | \(\ ln k\) |
| ---- | ---- | ---- | ---- |
|\ (T_ {1 }\) | \(\ frac {1 } {T_ {1 }}\) | \( k_ {1 }\) | \(\ ln k_ {1}\) |
|\ (T_ {2 }\) | \(\ frac {1} {T_ {2 }}\) | \( k_ {2 }\) | \(\ ln k_ {2}\) |
|\ (T_ {3 }\) | \(\ frac {1} {T_ {3 }}\) | \( k_ {3 }\) | \(\ ln k_ {3}\) |
2. ** Draw a\ (\ ln k -\ frac {1} {T}\) graph **
with\ (\ ln k\) as the ordinate and\ (\ frac {1} {T}\) as the abscissa, draw a scatter plot, and perform a linear fit to obtain a straight line equation\ (y = mx + c\), where\ (m\) is the slope and\ (c\) is the intercept.
3. ** Activation energy calculation **
From\ (\ ln k = -\ frac {E_ {a}} {RT} +\ ln A\), the slope is\ (m = -\ frac {E_ {a}} {R}\). Given\ (R = 8.314 J · mol ^ {-1} · K ^ {-1}\), the activation energy is\ (E_ {a} = -mR\). The value of the activation energy\ (E_ {a}\) for the reaction of ethyl acetate with sodium hydroxide is calculated.

Fifth, Conclusion
Through this experiment, using the Arrhenius formula, the activation energy of the reaction of ethyl acetate and sodium hydroxide was successfully calculated by measuring the rate constants of the reaction at different temperatures. This activation energy data provides an important parameter basis for further study of the kinetic characteristics and reaction mechanism of the reaction, which is helpful to a deeper understanding of the chemical reaction process, and also provides theoretical support for the optimization of reaction conditions in related industrial production.