Theoretical Yield of Aspirin?
824180
AA is not the limiting reagent, there is an excess amount of it. AA (from Aldrich catalog) has a density of 1.08g/ml, then 8ml contains .085 mol (1.08g/ml*8ml/102.09g/mol). \n6.0004g of Sal. acid is .043mol then you are correct that sal. acid is limiting, giving a theoretical maximum yield of 7.8266g. (if AA is limiting thoeretical max would be 15.2336g)
588570
Over 50, I would say just aspirin.\n\nTo be on the safeside ask your doctor.
952592
First thing you always need to do is balance your equation. While a balanced equation in the case doesn't matter math wise (because the mole ratio between CO2 and Li2CO3 is 1:1), it's still a good idea to get into the habit of balancing first. So:\n\n2LiOH + CO2 --> Li2CO3 + H2O\n\nUse this balanced equation, molecular weights of compounds, and molar ratio to find your answer:\n\n176.04 g CO2  x ( 1 mol CO2 / 44 g CO2) x (1 mol Li2CO3 / 1 mol CO2) x (73.88 g Li2CO3 / 1 mole Li2CO3) = 295.59 grams\n\nThen you use the information you just got (AKA Theoretical yield) to find the actual yield:\n\nPercent Yield =  (Actual Yield / Theoretical Yield)  x 100\n\nSo:\n\n (X / 295.59) = .9192   <--- this is the percent in decimal form so we don't have to worry about multiplying by 100. Just rearrange this equation to solve for X and you get your actual yield.\n\n X = (295.59)(0.9192)   =  271.71 grams\n\nHope this helped! Good luck with chemistry!!\n\n**EDIT** To Peter's response: He is correct. It should only be 4 sig figs, making it 271.7 grams. Sorry about my mistake :)
975985
Okie dokie. First, you balance out the equation. You want to make sure you have the same amount of sodium, phospohorous, and oxygen atoms on each side of the "yield" sign. The outcome could be 12Na+P(little 4)+8O(little 2) Yields 4(Na(little 3)PO(little4)). Then you use your periodic table to tell you how many grams per mole are in Na(little3)PO(little 4). The molar mass is 164 g. You only have 156 g, which means you have 0.95 moles (156/164). Now you know that you have half as many moles of oxygen, therefore you only have 0.475 moles of O2. Now all you have to do is do 0.475 moles of O(;little 2) multiplied by its molar mass, which is 32 grams. This will give you 15.2 grams of O(little 2). Note that for the atomic/molar masses, I rounded the numbers to whole grams. I hope that this helped.
748854
You are correct... just divide by 12, so 2.989E-8 slugs/in-s.  The only unit you are changing is the length.  I had no idea people used the slug/ft-s as a unit of viscosity.
333808
Well that previous answer was confusing!\n\nI'm assuming the mass of the aspirin tablet is 0.3711g or 371.1 mg.  The active ingredient is aspirin at 325 mg.\n\n325/371.1 x 100 = about 87.6% active ingredient  the reminder is inert material.\n\nEasy huh?!
781038
I agree with birchardv here...........we need the rest of the problem, and you would learn a lot more if you did the homework yourself.  But do whatever floats your boat.  Add the rest of the problem and I'll get back to you.\n\nOkay Chemist, this problem is really long; if you want a good answer with plenty of steps, I'll need more room.  Email me and I'll send you the solution.
961401
Try a pharmaceutical chemist. They may be able to obtain a small quantity for you.
887614
I'm sure not a Dr. but it looks like 50 mg / minute of Drug E are needed which (I think) translates to 1/5 of of a ml / min. (.2 ml / min) of what is on hand.
687306
Check the Michaelis-Menten equation.It's too long to write it all down for you ;)
753121
Ok, now this one I can do:\n\nMg3N2  ---> 3Mg (s) + N2 (g)
486450
Kind of depends on the Aspirin tablet. If it is coated or bufferend, it will have less. But generally, the percentage that is acetylsalicylic acid is quite high. Other ingredients may include corn starch and cellulose.\n\nSorry. I don't have the actual percentage. However, if you have an accurate (and precise) scale, weigh a 325mg pill and calculate the percentage.
1049722
Not particularly, but don't overdo it. Too much aspirin isn't good. Ice packs will probably give you better relief anyway.
185787
Every bond angle in aspirin is 120 degrees, with the exception of the bond angle around the oxygen that comes off the benzene ring ortho to the carboxylic acid and the bond angle of the oxygen in the hydroxyl group of the carboxylic acid. Those bond angles are approximately 109.5 degrees. Also the methyl group of the ester is CH3 and the angles around the methyl carbon are 109.5 degrees.
834060
def C6H14. i'm positive. hope this helps!!!
695903
Depends on the industry.  No set formula that I know of.
832153
2 moles of reactant  (C2H4F2) give you 4 moles of HF\nC2H4F2 : 66 g/mol\nHF: 20g/mol\nTherefore\n79,3g  C2H4F2*(1mol  C2H4F2/66g  C2H4F2)*(4 moles HF/ 2moles C2H4F2)*(20g HF/ 1mol HF)= 48,1g HF\nThe amount of HF you are expected to get with 100% yield is 48,1g. If you got 18g, then\n(18g/48,1g)*100= 37% yield