INTRODUCTION ON ACTIVATION ENERGY OF THE SAPONIZATION REACTION OF ETHYLETHE ACETATE AND SODIUM HYDROXIDE
I. INTRODUCTION
In chemical kinetics, the activation energy of the reaction is a key parameter, which has a profound impact on understanding the reaction mechanism and rate. As a classic chemical reaction, the saponification of ethyl acetate and sodium hydroxide is of great significance to explore its activation energy in depth. This reaction is widely used in many fields, and it is crucial to optimize the reaction conditions and improve the reaction efficiency.

Second, experimental principle
The saponification reaction of ethyl acetate ($CH_3COOC_2H_5 $) with sodium hydroxide ($NaOH $) is a second-order reaction. The reaction equation is as follows:
$CH_3COOC_2H_5 + NaOH\ longrightarrow CH_3COONa + C_2H_5OH $
During the reaction process, the concentration of the reactants varies with time according to the second-order reaction kinetic equation. By measuring the reaction rates at different temperatures, according to the Arrhenius formula:
$k = A e ^ {-\ frac {E_a} {RT}} $
where $k $is the reaction rate constant, $A $is the pre-index factor, $E_a $is the activation energy, $R $is the gas constant, and $T $is the absolute temperature. Take the logarithm of this formula to get:
$\ ln k =\ ln A -\ frac {E_a} {RT} $
By measuring the rate constant $k $at different temperatures $T $, plot $\ ln k $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 $.

III. Experimental Materials and Methods
(1) Experimental Materials
1. Ethyl acetate (analytical pure)
2. Sodium hydroxide (analytical pure)
3. Distilled water
4. Thermostatic water bath
5. Conductivity meter
6. Pipettes, volumetric flasks, conical bottles and other glass instruments

(ii) Experimental steps
1. ** Solution preparation **
- Accurately prepare a certain concentration of ethyl acetate solution and sodium hydroxide solution.
- For example, accurately measure a certain volume of ethyl acetate with a pipette, add an appropriate amount of distilled water, bandwidth evaluation in a volumetric flask, prepare a concentration of $c_1 $ethyl acetate solution; Similarly, prepare a concentration of $c_2 $sodium hydroxide solution.
2. ** Determination of reaction rate constants at different temperatures **
- Adjust the thermostatic water bath to a certain temperature of $T_1 $, such as 25 dollars ^ {\ circ} C $ ($298.15K $).
- Take an appropriate amount of equal volume of ethyl acetate solution and sodium hydroxide solution, quickly mix them in a conical bottle, and start the stopwatch timer at the same time.
- Use a conductivity meter to measure the conductivity of the reaction system at regular intervals $t $until the conductivity change stabilizes, and record the data.
- Calculate the reaction rate constant at this temperature $k_1 $according to the second-order reaction kinetic equation and the relationship between conductivity and concentration.
- Repeat the above steps, were measured at different temperatures (e.g., 30 dollars ^ {\ circ} C $, 35 dollars ^ {\ circ} C $, etc.) the reaction rate constants $k_2 $, $k_3 $and the like.

IV. EXPERIMENTAL DATA PROCESSING AND ANALYSIS
(I) DATA RECORDING
Data for different temperatures $T $, corresponding reaction times $t $and conductivity $\ kappa_t $are recorded in tabular form, as follows:

| temperature $T (K) $| time $t (min) $| conductivity $\ kappa_t (\ mu S/cm) $|
|---|---|---|
| 298.15 | 1 | $\ kappa_ {11} $|
| 298.15 | 2 | $\ kappa_ {12} $|
|... |... |
| 303.15 | 1 | $\ kappa_ {21} $|
| 303.15 | 2 | $\ kappa_ {22} $|
|... |... |

(ii) Rate Constant Calculation
Calculate the reaction rate constant $k $at each temperature according to the second-order reaction kinetic equation and the relationship between conductivity and concentration. For example, calculated by the following formula:
$k =\ frac {1} {t (a-x) } $
where $a $is the initial concentration of the reactant and $x $is the concentration of the reactant reacted at $t $, which can be converted from the conductivity data.

(3) Activation energy calculation
With $\ ln k $to $\ frac {1} {T} $plotted, using Origin and other software for linear fitting, obtained linear equation. From the slope of the line $m = -\ frac {E_a} {R} $, it is known that $R = 8.314 J\ cdot mol ^ {-1}\ cdot K ^ {-1} $, the activation energy of the reaction is calculated $E_a = - mR $.

Fifth, Conclusion
The rate constants of the saponification reaction of ethyl acetate and sodium hydroxide at different temperatures were experimentally determined, and the activation energy of the reaction was calculated according to the Arrhenius formula. This activation energy value is of great significance for in-depth understanding of the kinetic process of the saponification reaction, and provides an important theoretical basis for further study of the reaction characteristics under different conditions and applications in industrial production and other fields.