What two factors determine the vapor composition above a liquid mixture at any g

Question

What two factors determine the vapor composition above a liquid mixture at any given temperature? Define the term "zoetrope". What is the minimum difference in boiling points needed in order to cleanly separate a mixture two liquids by simple distillation?. Explain why there is a difference (if any) between the boiling point of pure methyl acetate boiling points you recorded for the distillates you collected in the simple and the fractional distillations. If you distilled a mixture which was made from 17 moles of MeOAc and 34 moles of EtO Ac, would it boil at 62 degree C? Why or why not? What are the results of the following procedural errors: Heating the solution too quickly Opening a cold sample vial Not capping a vial tightly Having the oven temperature too hot on the GC Having an air bubble in the syringe when injecting your GC sample

Explanation / Answer

1.amount of vapour composition above a liquid mixture depend on several factors,

The concentration of a vapor in contact with its liquid, especially at equilibrium, is expressed as vapor pressure,partial pressure.The equilibrium vapor pressure of a liquid is dependent on temperature. At vapor–liquid equilibrium, a liquid with individual components in certain concentrations will have an equilibrium vapor in which the concentrations or partial pressures of the vapor components have certain values depending on all of the liquid component concentrations and the temperature.The equilibrium concentration of each component in the liquid phase is often different from its concentration in the vapor phase, but there is a relationship

2.Azeotropes(Mixtures of liquids) can be encountered that mimic the boiling behavior of pure liquids. These mixtures when present at specific concentrations distill at a constant boiling temperature and can not be separated by distillation. Examples of such mixtures are 95% ethanol-5% water (bp 78.1 °C).The azeotropic composition sometimes boils lower the than boiling point of its components and sometimes higher.

3.The reason is in pure liquid we measure its real boiling point but in fractional distillation we always get a ratio of a mixture of compounds so the boiling points get from distillations can be differ from real liquid sample.In most of the time the boiling point of a mixture is the median of two pure boiling points of two compounds.

4. BP of MtOAc -56.9             BP of EtOAc -77C

boiling point must be in between these 2 temperatures. But due to the factors such as ratio of amount of substance present in the mixture and the volatality rate will effect for the resultant bp of the mixture.

5.heating the solution quickly cause to reduce the reaction if take place but it cause to the degradation of compuond before vapuorizatoin.

not capping the vial cause to remove the vapour to the outside environment. All calculations and assumption of ideal conditions will not valied. some amount is loss.

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