The boiling point of ethyl acetate, a widely used organic solvent, is a crucial property that has been extensively studied and reported in various scientific sources. This comprehensive guide delves into the technical details, experimental data, and theoretical underpinnings of the boiling point of ethyl acetate, providing a valuable resource for science students and researchers.
Understanding the Boiling Point of Ethyl Acetate
The boiling point of a substance is the temperature at which the vapor pressure of the liquid equals the pressure surrounding the liquid, and bubbles of vapor form inside the liquid. For ethyl acetate, the normal boiling point, which is the boiling point at standard atmospheric pressure (1 atm or 101.325 kPa), is 349.25 K (76.1°C) with an uncertainty of 0.3 K, as reported by Manjeshwar and Aminabhavi (1988) in the NIST WebBook.
The boiling point of ethyl acetate is influenced by various factors, including:
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Intermolecular Forces: The strength of the intermolecular forces, such as dipole-dipole interactions and van der Waals forces, between ethyl acetate molecules plays a crucial role in determining the boiling point. Stronger intermolecular forces require more energy to overcome, resulting in a higher boiling point.
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Molecular Structure: The molecular structure of ethyl acetate, with its ester functional group and alkyl chains, affects the intermolecular interactions and, consequently, the boiling point.
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Pressure: The boiling point of ethyl acetate, like any other substance, is dependent on the surrounding pressure. As the pressure increases, the boiling point also increases, as described by the Clausius-Clapeyron equation:
ln(P2/P1) = (ΔHvap/R) * (1/T1 - 1/T2)
where P1 and P2 are the vapor pressures at temperatures T1 and T2, respectively, ΔHvap is the enthalpy of vaporization, and R is the universal gas constant.
- Impurities: The presence of impurities in ethyl acetate can affect its boiling point, as the impurities can alter the intermolecular interactions and the vapor pressure of the solution.
Experimental Measurements of the Boiling Point
The boiling point of ethyl acetate has been measured and reported in various experimental studies. One such study by Blanco and Ortega (1998) focused on the vapor-liquid equilibrium (VLE) values for binary mixtures composed of methanol and an ethyl ester, including ethyl acetate, at 141.3 kPa. The researchers used a dynamic recirculating still to obtain the VLE data, which can be used to determine the boiling point of ethyl acetate under the specified pressure conditions.
Another study by Li et al. (2023) investigated the ternary vapor-liquid equilibrium (VLE) data of ethyl acetate + chloroform + [EMIM][OAc] at 101.3 kPa. The researchers used a static equilibrium cell and a gas chromatography (GC) analysis method to measure the VLE compositions, which can provide insights into the boiling point of ethyl acetate in the presence of other components.
Theoretical Considerations
The boiling point of ethyl acetate can also be estimated using theoretical models and equations. One widely used approach is the application of the Clausius-Clapeyron equation, which relates the vapor pressure of a substance to its temperature and enthalpy of vaporization. By rearranging the Clausius-Clapeyron equation, the boiling point can be calculated as:
Tb = ΔHvap / (R * ln(Pb / P0))
where Tb is the boiling point, ΔHvap is the enthalpy of vaporization, R is the universal gas constant, Pb is the boiling point pressure, and P0 is the reference pressure.
The enthalpy of vaporization of ethyl acetate has been reported in various sources, such as the CRC Handbook of Data on Organic Compounds, 2nd Edition (Weast and Grasselli, 1989), which lists the enthalpy of vaporization as 35.9 kJ/mol at the normal boiling point.
Practical Applications and Considerations
The boiling point of ethyl acetate is an important property in various applications, such as:
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Solvent Selection: The boiling point of ethyl acetate is a key factor in determining its suitability as a solvent in chemical processes, as it affects the ease of separation and recovery.
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Reaction Conditions: The boiling point of ethyl acetate is crucial in designing reaction conditions, as it influences the temperature range at which the reaction can be carried out.
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Distillation and Purification: The boiling point of ethyl acetate is essential in the design and optimization of distillation and purification processes, such as the separation of ethyl acetate from reaction mixtures or the recovery of ethyl acetate from waste streams.
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Safety Considerations: The boiling point of ethyl acetate is also relevant for safety considerations, as it affects the volatility and flammability of the substance, which are important factors in handling and storage.
Comparison with Other Solvents
To provide a broader context, it is useful to compare the boiling point of ethyl acetate with those of other common organic solvents:
| Solvent | Boiling Point (°C) |
|---|---|
| Methanol | 64.7 |
| Ethanol | 78.3 |
| Acetone | 56.2 |
| Dichloromethane | 39.6 |
| Toluene | 110.6 |
| Ethyl acetate | 76.1 |
As shown in the table, the boiling point of ethyl acetate (76.1°C) is higher than that of methanol, acetone, and dichloromethane, but lower than that of ethanol, toluene, and other higher-boiling solvents. This range of boiling points allows ethyl acetate to be used in a variety of applications where the desired volatility and ease of separation are important factors.
Conclusion
The boiling point of ethyl acetate is a well-studied and widely reported property that is crucial in various scientific and industrial applications. This comprehensive guide has provided detailed information on the factors influencing the boiling point, experimental measurements, theoretical considerations, and practical applications of this important organic solvent. By understanding the technical aspects of the boiling point of ethyl acetate, science students and researchers can make informed decisions and optimize processes involving this versatile compound.
References
- Li, P., Cui, X., Zhang, H., Feng, T., & Feng, H. (2023). Isobaric Vapor–Liquid Equilibrium for Ethyl Acetate + Chloroform with Ionic Liquids [EMIM][OAc], [BMIM][OAc], and DMSO + [EMIM][OAc] as Entrainers at 101.3 kPa. ACS Journal of Chemical & Engineering Data, 68(2), 726-733.
- Ethyl Acetate – the NIST WebBook. (n.d.). Retrieved from https://webbook.nist.gov/cgi/cbook.cgi?ID=C141786&Type=TBOIL
- Blanco, A. M., & Ortega, J. (1998). Densities and Vapor-Liquid Equilibrium Values for Binary Mixtures Composed of Methanol + an Ethyl Ester at 141.3 kPa with Application of an Extended Correlation Equation for Isobaric VLE Data. Journal of Chemical & Engineering Data, 43(4), 638-645.
- Weast, R. C., & Grasselli, J. G. (1989). CRC Handbook of Data on Organic Compounds, 2nd Edition. Boca Raton, FL: CRC Press, Inc.
- American Tokyo Kasei. (1988). TCI American Organic Chemical 88/89 Catalog. Portland, OR: American Tokyo Kasei.
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