Acetone in water influence its enthelpy of vaporization

In summary, the conversation revolved around the development of a waste heat recovery device that uses a solution of acetone and water. The question was raised about the enthalpy of vaporization of acetone from solution and how it is affected by the ratio of acetone to water. It was also mentioned that acetone undergoes hydrogen bonding with water and a paper was cited on the binding energy between the two substances. The potential use of information on hydrogen bonding to determine the enthalpy of vaporization was also discussed, with a suggestion to look at the vapor pressure and temperature coefficient of the Gibbs free energy.
  • #1
ejnovek
18
0
Hi Everyone,

I'm currently developing a waste heat recovery device as a side project. The system I've created uses a solution of acetone and water. One step in the process involves vaporizing acetone from the water at a low grade heat temperature (note: acetone does not form an azeotrope with water).

Based on the fact that the acetone is dissolved in water, I've assumed that the enthalpy of vaporization of acetone from solution would be greater than if acetone were not in solution.

However, I have been unable to find specific information on the enthalpy of vaporization of acetone dissolved in water and how this energy changes depending on the ratio of acetone to water in solution.

If anyone can find some or all of this information it would be greatly appreciated!

Thanks,

EJ
 
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  • #2
Does acetone undergo hydrogen-bonding with water?
 
  • #3
Yes, acetone does undergo hydrogen bonding with water and that is the reason acetone is miscible in water. This paper details the binding energy between acetone and water:https://www.researchgate.net/publication/228425952_Theoretical_analysis_of_the_hydrogen_bond_interaction_between_acetone_and_water

How can information on hydrogen bonding be used to determine the enthalpy of vaporization of acetone in water?
 
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  • #4
How do you determine the enthalpy of vaporization of the acetone from the acetone-water solution?
 
  • #5
A quick thought or two, without thinking it through in detail: If you can find information on the vapor pressure of both water and acetone as a function of composition and temperature you might be able to tease out the enthalpy and entropy of the process.

Basically, the vapor pressure can be related to the Gibbs free energy and the entropy can be related to the temperature coefficient of the Gibbs free energy. Subtracting the TS term will give you the entropy.

As I mentioned, I have not thought this through in detail, so please just consider it a hint as to how one might proceed.
 

1. How does the presence of acetone affect the enthalpy of vaporization of water?

The presence of acetone in water can significantly impact the enthalpy of vaporization, which is the amount of energy required to convert a liquid into a gas. Acetone is a volatile organic compound (VOC) that has a lower boiling point than water. This means that when it is mixed with water, it will evaporate more quickly and decrease the enthalpy of vaporization of the mixture.

2. Does the amount of acetone in water affect its enthalpy of vaporization?

Yes, the amount of acetone in water does have an impact on the enthalpy of vaporization. As the concentration of acetone increases, the enthalpy of vaporization decreases. This is because more acetone molecules are present in the mixture, and they have a lower boiling point than water, making them easier to vaporize.

3. How does temperature play a role in the enthalpy of vaporization of water with acetone?

The temperature of the mixture can also affect the enthalpy of vaporization. As the temperature increases, the molecules in the mixture gain more energy and can overcome the intermolecular forces holding them together. This makes it easier for the molecules to break free and vaporize, resulting in a lower enthalpy of vaporization.

4. Can the presence of other substances in water also influence the enthalpy of vaporization?

Yes, the presence of other substances in water can also have an impact on the enthalpy of vaporization. Similar to acetone, other volatile compounds with lower boiling points can decrease the enthalpy of vaporization when mixed with water. In contrast, substances with higher boiling points may increase the enthalpy of vaporization.

5. Why is understanding the enthalpy of vaporization important for scientific research?

The enthalpy of vaporization is an essential factor in many scientific processes, such as distillation, evaporation, and phase changes. It is also crucial in industries that involve the use of mixtures, such as pharmaceuticals, cosmetics, and food production. Understanding how different substances affect the enthalpy of vaporization can help scientists and engineers optimize processes and improve product quality.

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