1.[ Plot temperature (oC) vs. volume of distillate (ml) collected for the mixture with and without the fractionating column. Use the graph to determine the boiling ranges of the two compounds in the mixture and identify the compounds. Plot both sets of data on the same graph]- I know how to do that part and by the way the unknown compounds are acetone and 1-propanol. --Also plot on this graph an ideal distillation curve. Why are the real distillation curves different from the ideal? 2. Use a vapor/liquid diagram to explain the differences in the simple and fractional distillation plots. Describe what is happening in the fractionation column and explain why this results in a better separation with purer components isolated. 3. Why is it important to maintain a distilling rate of ~0.5 drop/s? Why not faster or slower? 4. What is an azeotrope? Sketch a distillation curve (as in Question 1) for a simple distillation of a mixture of toluene (70 ml) and water (30 ml). Explain the behavior of the curve.
1.[ Plot temperature (oC) vs. volume of distillate (ml) collected for the mixture with and without the fractionating column. Use the graph to determine the boiling ranges of the two compounds in the mixture and identify the compounds. Plot both sets of data on the same graph]- I know how to do that part and by the way the unknown compounds are acetone and 1-propanol. --Also plot on this graph an ideal distillation curve. Why are the real distillation curves different from the ideal? 2. Use a vapor/liquid diagram to explain the differences in the simple and fractional distillation plots. Describe what is happening in the fractionation column and explain why this results in a better separation with purer components isolated. 3. Why is it important to maintain a distilling rate of ~0.5 drop/s? Why not faster or slower? 4. What is an azeotrope? Sketch a distillation curve (as in Question 1) for a simple distillation of a mixture of toluene (70 ml) and water (30 ml). Explain the behavior of the curve.
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