Possible Error In Distillation
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the condenser need to flow? A: Very slowly. If you notice a sink filling up, let the instructor know. Q: Why do we need to anchor
Sources Of Error In Fractional Distillation Experiment
the drain hose? A: So the water drains in the trough only. We have sources of error in steam distillation flooded the optics lab downstairs in the past. Q: Should I distill as much as I can? A: No. Stop
Experimental Errors In Simple Distillation
when there is still a milliliter or so in the pot, so the flask does not get too hot. (In the research lab, you may have reactions in which there is a significant amount of distillation thermometer placement higher molecular weigh byproducts from which you are distilling and there will be considerably more residue than will be our experience in the teaching lab.) Q: When I look up boiling points, I find different values for the same compound with superscripted numbers - what does this mean? A: Those are boiling points at different pressures, and the superscripts refer to pressure in mm of Hg. The reason for this if two miscible liquids found boil is that we often do distillation under vacuum to lower the boiling point, and thus prevent decomposition. In Chem 113A we will not be doing vacuum distillation. Q: What are the most common experimental errors in distillation? A: Placing the thermometer too high will lead to a low value for boiling point - be sure all the mercury in the bulb is below the sidearm of the still head. Inadequately clamping the apparatus can be dangerous. Over clamping can be a problem, since it causes stress in the apparatus. Refer to the Distillation section for detail on clamping the apparatus in place and clamping the pieces together. It is especially important to tighten the nut which keeps the utility clamp from rotating. Check that the joints are well greased and that all the joints are seated before turning on the thermowell. Remember to turn on the cooling water. Remember to use boiling chips. Q: I see my distilland boiling and going down in volume but there is no distillate appearing - what is wrong? A: Check that the cooling water is on - if it is then you must have a leak in the system. Stop the distillation immediately (turn off and lower the thermowell) and locate the p
tube connects to another, similarly shaped tube that sticks out from its side, and is pointed downward. This tube, called the "condenser" has water running through a cavity between the inside and outside of the
Distillation Thermometer Too High
glass -- sort of like having a glass tube within a slightly larger glass tube. what happens if distillation occurs too quickly This tube ends in a spout, where some sort of receptacle is placed for collection. In the picture above, the receptacle is
What Is The Purpose Of The Boiling Chips
a graduated cylinder with a red plastic bottom.What occurs macroscopically in a distillation is pretty common to everyday experience: You add heat to some liquid, and the liquid evaporates up the tube and eventually travels through the condenser, http://www.chemistry.sjsu.edu/straus/FAQ/Technique%20FAQ/DistillationFAQ.htm where the water quickly cools the vapor, and drips out of the spout and into the receptacle. In particular, this is how liquor companies obtain higher concentrations of alcohol. When you make alcohol, the alcohol is fully dissolved in water -- like beer, or wine. The trick to higher alcohol content lies in... Chemistry!So, suppose a beaker full of recently made alcohol -- it will be clear, and from appearances look to be the same http://fug-experimentalerror.blogspot.com/2009/09/distillation.html liquid. This is because alcohol is miscible in water, which is the opposite of what happens when you mix oil and water. No matter how much water and alcohol you mix together, they will always freely intermingle. So, you're left with a beaker of water and alcohol molecules:Behold the power of paint! The blue atoms with two red atoms coming off of them is a water molecule. The other one is a molecule of the drinking variety of alcohol. It has a blue atom as well because both water and alcohol have Oxygen in them.How would you separate these?A quick look at ethanol's MSDS sheet tells us that the alcohol has a boiling point of 78 degrees Centigrade. Water's boiling point is 100 degrees centigrade. Attempting to boil the mixed liquid seems like a good idea. And, in fact, this is how alcohol and water are separated -- first the alcohol evaporates and is collected, then the water will stop evaporating. If you want to keep them separate, you stop the distillation once you have collected the majority of your alcohol. How does one tell when that happens?You'll notice in the photograph a thermometer. If we plot a graph of the amount of liquid collected on the x-axis versus the temperature of the vapor (which corresponds to the liquid's temperature) on the y-axis,
Files Members Favorites 20 All Pages 20 AcetylationOfFerrocene Crystallization and Recrystallization Lab DistillationLab ElectrophilicAromaticIodinationOfVanillin Extraction A&B Lab GreenBrominationOfStilbene Kristal'sGreenChemistryPaper Kristal'sReflection LabReport1 Michelle's Bend Research Reflection Michelle'sgreenchempaper NMR and MRI Philip's Bend Research Reflection PreparationOfCyclohexene SloventEffectsInSN1 SublimationLab https://ochemwonderstudents.wikispaces.com/DistillationLab Tristan's GC Lab Tristan's Seventh inning stretch Add Add "All Pages" Done DistillationLab Edit 0 22 … 1 Tags distillation Notify RSS Backlinks Source Print Export (PDF) Philip Deenik Michelle Guerin Kristal Kiel Lab 3: Distillation Carol: Although http://www.chegg.com/homework-help/questions-and-answers/could-possible-sources-error-fractional-distillation-experiment-q3053588 this edit is only under one name, we were all sitting here doing it together. We did this so it would be easier for you since you only had to look at one "redone" document. Introduction: Distillation is error in a common technique involving separating of liquids by boiling point. Certain substances begin boiling (and vaporize) at a more given temp, making it possible to isolate the substances into separate phases based on their boiling point (while one may vaporize at a lower temp, the other may remain in liquid form.) be careful how you say this: it's not that one component vaporizes first, it is that it vaporizes more at a given temp (more molecules are sources of error in the gas phase). By isolating the vapor at different temperatures, the impure substance can be purified. There are many factors contributing to the effectiveness of the distillation process. A major factor is the range difference between boiling points of the substances. If the substances have very similar boiling points, it will be very difficult to isolate the impurities. This experiment involved a simple distillation where the acetone had a much lower boiling point than the impurities. A more complex set up would be required for the distillation of two or more substances with similar boiling points. This experiment involves the distillation of impure acetone for a the Great American Paint Company. Procedure: Following the proceeding instructions, use a macroscale glassware kit to assemble the apparatus in figure 1. Set up a ring stand and place heating stir plate on top of a slightly-extended lab jack on it's base. Use a wide-mouthed dish filled with water instead of a Thermowell. Place the dish on the heating stir plate and clamp a 100 mL round-bottom flask so that it rests an inch or so deep in the water bath. Make sure the flask is secure and immobile. Add 40 mL of contaminated acetone to the 100 mL flask via funnel. Drop in a stir bar. Attach a three-way adapter with the 'Y' facing down. Insert a thermometer ada
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