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10 Nov 2019

I am required to synthesize Diethyl Maleate from Maleic Anhydride in a lab. Materials are limited and I really need help on how to go about it. Any bit of help will be appreciated! :)I'm thinking about dissolving the maleic Acid in ethenal and possibly adding sulfuric acid as the acid catalyst and then reflux. I'm not sure if this will work and don't know where to go from here :(

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Nelly Stracke
Nelly StrackeLv2
16 Feb 2019

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Related questions

For my Organic Chemistry lab, we are synthesizing esters via microwave-assisted Fischer esterification. My task is to synthesize n-butyl benzoate. The procedure provides us with two options, either use excess alcohol or excess carboxylic acid to obtain the highest yield and purest product. We get to pick which procedure we think is best. After looking into the equilibria behind this reaction, I am leaning towards using excess carboxylic acid over excess alcohol. According to Le Chateliers principle, doing either will drive the reaction towards the sythnesis of the ester. Here's my reasoning:

(1) Because I am synthesizing n-butyl benzoate, my alcohol/solvent is going to be 1-butanol. This has a relatively high boiling point (about 118 degrees Celcius), which is going to be hard to evaporate off by using steam distillation/rotary evaporation. Even though the n-butyl benzoate has a boiling point of about 250 degrees celcius and wouldn't be effected by steam distillation/rotary evaporation, I feel like it would be hard to evaporate off all of the excess alcohol and obtain the purest product (even boiling off excess methanol in a previous lab took a really long time using rotary evaporation)

(2) Adding excess carboxylic acid seems to be a lot easier to extract off by doing liquid-liquid extraction. Just rinse the solution with sodium bicarbonate, you create a carboxylate salt and that will cause it to associate with the aqueous layer. Even though I still have to do steam distillation/rotary evaporation, it would be much easier to boil off the remaining alcohol than if I were to use it in excess to begin with.

Additionally, one concern about the procedure I do have is during the liquid-liquid extraction of the ester. Because the density of the ester is at 1.00g/mL +/- 0.01 and water is also at 1.00g/mL, how does the ester separate from the aqueous layer if the densities are the same? Or is it just because the n-butyl benzoate is not polar and water is? In that case, despite their similar densities, ultimately the separation comes down to the differences in polarities, not the densities?

Finally, my only hesitation with using excess carboxylic acid is that standard procedures involving esterifications use excess alcohol. Can you please explain the costs and benefits to using both excess carboxylic acid excess alcohol? Any help would be appreciated, Will rate for a thorough answer, thank you.

For my Organic Chemistry lab, we are synthesizing esters via microwave-assisted Fischer esterification. My task is to synthesize n-butyl benzoate. The procedure provides us with two options, either use excess alcohol or excess carboxylic acid to obtain the highest yield and purest product. We get to pick which procedure we think is best. After looking into the equilibria behind this reaction, I am leaning towards using excess carboxylic acid over excess alcohol. Here's my reasoning:

(1) Because I am synthesizing n-butyl benzoate, my alcohol/solvent is going to be 1-butanol. This has a relatively high boiling point (about 118 degrees Celcius), which is going to be hard to evaporate off by using steam distillation/rotary evaporation. Even though the n-butyl benzoate has a boiling point of about 250 degrees celcius and wouldn't be effected by steam distillation/rotary evaporation, I feel like it would be hard to evaporate off all of the excess alcohol and obtain the purest product (even boiling off excess methanol in a previous lab took a really long time using rotary evaporation)

(2) Adding excess carboxylic acid seems to be a lot easier to extract off by doing liquid-liquid extraction. Just rinse the solution with sodium bicarbonate, you create a carboxylate salt and that will cause it to associate with the aqueous layer. Even though I still have to do steam distillation/rotary evaporation, it would be much easier to boil off the remaining alcohol than if I were to use it in excess to begin with.

Additionally, one concern about the procedure I do have is during the liquid-liquid extraction of the ester. Because the density of the ester is at 1.00g/mL +/- 0.01 and water is also at 1.00g/mL, how does the ester separate from the aqueous layer if the densities are the same? Or is it just because the n-butyl benzoate is not polar and water is? In that case, despite their similar densities, ultimately the separation comes down to the differences in polarities, not the densities?

Finally, my only hesitation with using excess carboxylic acid is that standard procedures involving esterifications use excess alcohol. In my particular reaction will using one reactant in excess produce a higher yield/purer compound over using the other reactant in excess? If so, which one do you think it would be? Any help would be appreciated, Will rate for a thorough answer, thank you.

I'm working on a project I need some help with (BTW I asked my teacher and I am allowed to ask for help). If there was anything I wasn't clear on please tell me because I'm just hopelessly lost on this. Also just to note this actually has a fair bit of chemistry in it but because it's all related to electricity and there is no chemistal engineering subject Tab I put it here.

Okay so in this project we have a hypothetical scenario. In this scenario I'm on an abandoned island and I need to power a satellite for 97 minutes at 12 volts at 30 amps and 5 volts at 45 amps. But on this island are various supplies including a 1987 V8 engine which I think will provide 12 volts at 30 amps. Now what I need is fuel to get it going. I have 4 deep friers full of oil, 3 cases of magnum bottles of champagne, salt water from the ocean, 21 2 gallon jars of pickled eggs, and 33-5 gallon containers of italian salad dressing, and 23 #10 cans of tomato sauce. There is also an abandoned moonshine still. So using the oil from the friers, the champagne, and getting the oil out of the salad dressing I should be able to get a decent amount of biofuel correct? I also have 9 full 20# propane tanks and I read that propane can be used to make fuel burn more efficiently by taking the place of the air injection. If there anything else from this list that I could make into fuel of some kind? What about Moonshine everything I read mentions sugar and yeast which I don't think I have either of.

So assuming I have that all worked out okay that gets me my 12 volts at 30 amps. But I still need the 5 volts at 45 amps. And one solution I was thinking of was making voltic cells. Amoung the materials I have to work with that are of use here are some 1/2'' and 3/4'' copper pipes, 8 roles of aluminum foil, 23 20ft lengths of 6 in. sch. 40 PVC pipe, 17 20ft lengths of 4in. sch. 40 PVC pipe, and 9 20ft lengths of 2 in. Sch. 40 PVC pipe. I also have some cans of cold galvanizing spray paint ( meaning I have zinc), and various containers including a lot of PVC pipe, 55 gallon plastic drums, and a complete set of commercial pots and pans. I also have various wires but I'll put that asside for now. I also have access to some PH adjust (down)

Now what I want to do is make a battery set up that can deliver 5 volts at 45 amps for 97 minutes.

I know I can make several battery cells and connect them in series and parallel to get the desires voltage and current. But i'm having trouble figuring out what my voltage and amperage would be for each cell. Also how long would the charge last?

I read something called aluminum-air batteries but I'm not clear on how they are made or if they are ideal for what I need. Would using the pickling solution from the pickled eggs as my electrolyte be better than using the salt water? Or should I separate the vinegar out of the salad dressing and us that? Would using the PH adjust (down) help?

I tried looking up some reduction charts but those were all in aqueous. What I was able to get was that for copper and aluminum it was about 2 v potential and for copper Zinc it was about 1.01 v. Is this correct? For a base line lets say I just use the PVC pips, copper pipe, aluminum foil, Salt water, and for wiring I use copper wire. if I"m correct and I get about 2 V from each battery how do I find my amperage? What part of all this affects the current and how would I calculate it? Would using a different kind of wire be better? I have access to a couple different kinds.

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