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Investigation of the variation of boiling point with composition for different mixture of two miscible liquids

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Introduction

? Name: Penguin Chow Cheuk Yan ? ? Class: 6S Class Number: 14 ? ? Date: 17 - 05 - 2003 ? Chemistry Full Report Experiment 16 Title: Investigation of the variation of boiling point with composition for different mixture of two miscible liquids Aim: To study the situations of intermolecular forces between unlike molecules in a mixture of two miscible liquids. The situations may be either stronger or weaker or the same which depends on whether the solution is ideal or not. The boiling point of a liquid depends on the strength of intermolecular force. The higher the strength, the higher the boiling point. The formation of a liquid mixture involves changes in the strength of the intermolecular forces. The formation of ideal mixtures and non-ideal mixtures relates to how the intermolecular force is changed Theory: Firstly, it is important to have known the difference between ideal and non-ideal solution. Ideal solution is known as a solution formed with no accompanying energy change when the intermolecular forces between the molecules of the solvents are the same as those between the molecules in the separated components. Ethanol contains -OH group which can form hydrogen bond among its molecules. On mixing, the hydrogen bond are broken among ethanol molecules. ...read more.

Middle

6.8 The mixture was then reheated until boiling gently again. 6.9 Further additions of 3 ?3 and 5 ?3 of propanone was added into the mixture and boiling point of each mixture was recorded down in the TABLE 1. 6.10 After that, the flask was emptied out and it was kept away from any naked fire while at the same time it was allowed to dry as the mixture was volatile and flammable. 6.11 Adding in succession 2 ?3 and 3?3 and 5 ?3 of hexane was repeated and results were recorded in the TABLE 1. Apparatus: (-10 ?) - 110 ? thermometer 1 piece anti-bumping granules several pieces 10 cm3 measuring cylinders 4 pieces quickfit set 1 set Bunsen burner 1 set wire gauze 1 piece Chemicals: tichloromethane ethyl ethanoate propanone hexane Result: TABLE 1 Volume of trichloromethane / cm� 10 10 10 10 5 2 0 Volume of ethyl ethanoate / cm� 0 2 5 10 10 10 10 Volume % of ethyl ethanoate 0 16.67 33.33 50 66.67 83.33 100 Boiling point / ? 60.5 69.8 70.0 75.0 76.5 78.5 79.5 TABLE 2 Volume of hexane / cm� 10 10 10 10 5 2 0 Volume of propanone / cm� 0 2 5 10 10 10 10 Volume % of propanone 0 16.67 33.33 50 66.67 83.33 100 Boiling point / ? ...read more.

Conclusion

In such case, the molecules are held together by hydrogen bonds. On adding hexane to propanone, the hexane molecules interpose between the molecules of propanone and break the hydrogen bonds thereby reducing the intermolecular attraction between propanone molecules. This increases the tendency of the propanone molecules to escape more readily from the liquid to vapour phase. The vapour phase therefore increases and the boiling point decreases. The escape tendency of molecules in the mixture is higher than expected from the Raoult's Law. Therefore, this mixture has a positive deviation compared with ideal solution. TABLE 1 Volume of trichloromethane / cm� 10 10 10 10 5 2 0 Volume of ethyl ethanoate / cm� 0 2 5 10 10 10 10 Volume % of ethyl ethanoate 0 16.67 33.33 50 66.67 83.33 100 Mole Fraction of ethyl ethanoate 0 16.67 33.33 50 66.67 83.33 100 TABLE 2 Volume of hexane / cm� 10 10 10 10 5 2 0 Volume of propanone / cm� 0 2 5 10 10 10 10 Volume % of propanone 0 16.67 33.33 50 66.67 83.33 100 Mole Fraction of propanone 0 16.67 33.33 50 66.67 83.33 100 Reference: 1. http://hk.geocities.com/fatherofchemistry 2. SAT II Chemistry - Barron 3. Dictionary of Chemistry - Andrew Hunt ** END ** ...read more.

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