The following observation was made during a distillation of water and dimrthylsu
ID: 890886 • Letter: T
Question
The following observation was made during a distillation of water and dimrthylsulphoxide: After leveling off in vapor temperature at 100 degree C for a considerable amount of time, the temperature actually decreased to about 25 degree C even though there was lots of boiling liquid still left in the boiling flask. What has happened? What is the composition of the boiling liquid in the boiling flask? Explain why the graph for simple distillation appears differently from the graph for fractional distillation. From your graphs, what is the boiling point of ethanol at the time you performed the experiment? What is the boiling point of water taken at the same time and conditions? Never fill a distilling flask to more than half-fullness when distilling. Why? Why should we never heat a flask to dryness? What is bumping? How does a boiling chip prevent bumping? Should the water be introduced from the top or the bottom of the condenser? Explain your reasoning. Would water boil at a higher or lower temperature in Denver, CO, USA as compared to Regina? Explain why. What would you expect the vapor temperature to be after collecting 5 mL of distillate in a mixture containing 10 mL of acetone and 10 mL of for a fractional distillation? What would the vapor temperature be a simple distillation?Explanation / Answer
1) Boiling point of water = 1000c and Boiling point of Dimethyl sulphoxide = 1890c and after levelling off vapor temeperature to 1000c, water under goes boiling and converted to vapor state and decreasing of temperature to 250c the vaporing of water decreases and the remaining solution in the boiling flask contains mainly dimethyl sulphoxide.
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