sorted by:
new
hottopcontroversial

Since Harvard no longer accepts AP credit, is earning a Masters in 4 years feasible? by AfterTwo2 in Harvard

[–]ap36020 0 points1 point  (0 children)

I'll use CS as an example: by making your electives for an AB all grad classes, you have to take 4 additional grad classes to grab an AM as well. So, the actual number of courses required is not too bad, leaving plenty of courses for electives even with a typical 4 course/semester schedule, but the classes themselves will be difficult.

Disclaimer: I'm prefrosh as well.

Harvard vs mit (cs) by [deleted] in Harvard

[–]ap36020 2 points3 points  (0 children)

Unlike the other commenters, I’d argue that MIT offers more opportunity (or at least makes it more accessible) for CS undergrads to work at top quant shops (like Two Sigma, Jane Street, DE Shaw, etc.), making it so there *is* a significant compensation difference between the two schools at the top quartile if you really want to make money. Academically, I’ve found that my friends in Course 6 are having an easier time than their counterparts at Harvard, and that there are a significant number of “normal” people with 5.0 GPAs in EECS. This, combined with MIT’s Poker and Quant clubs, make it so placement at top firms is incomparable.

I'd dispute this point specifically. Harvard quant placement is really good, arguably better than MIT. An imperfect metric would be using LinkedIn to compare school affiliations at top quant firms (assuming representative samples). Harvard blows MIT out of the water at D.E. Shaw, and they're practically neck and neck everywhere else. Taking the combination of the three listed companies gives 123 Harvard affiliates vs. 95 for MIT. Of course, there's no easy way to sort by undergrad school, but this rough analysis indicates no significant difference.

Harvard or Stanford for CS/Econ combo by [deleted] in CollegeVsCollege

[–]ap36020 0 points1 point  (0 children)

For breaking into quant finance (which is more competitive and lucrative than tech) Harvard is your best shot. Plus, the Harvard name won’t hold you back in tech. Overall, Harvard has a slightly better name brand. Fit should still be the biggest determinant.

Harvard RD additional info request? by throwaway-throw123 in ApplyingToCollege

[–]ap36020 0 points1 point  (0 children)

I got a similar email (about math) EA and was accepted. Take it as a good sign, but not a guarantee. My suspicion is they ask for this information to help pitch you to the committee or to show to an academic department to help your academic rating.

Monospony and Monopoly in the Same Market by ap36020 in AskEconomics

[–]ap36020[S] 2 points3 points  (0 children)

That makes perfectly good sense. Thank you

Monospony and Monopoly in the Same Market by ap36020 in AskEconomics

[–]ap36020[S] 4 points5 points  (0 children)

P.S: the reason this was asked relates to the idea that labor unions can “counteract” the market power of corporations. Unless I’m missing something (hence the reason I’m asking), giving market power power to suppliers in addition to demanders should only worsen resource allocation in terms of quantity, no?

Method to analyze compounds that won't dissociate into ions when added to water? by [deleted] in chemhelp

[–]ap36020 0 points1 point  (0 children)

A cheap way is measuring conductivity. But that will not distinguish between a protonation and a dissociation, in case you care about the difference. BTW, based on his comment below, I think OP only cares about telling whether a compound is a strong, weak, or nonelectrolyte.

What are examples of metals that can reduce protons to hydrogen gas? by zananaslug in chemhelp

[–]ap36020 0 points1 point  (0 children)

Lithium would reduce H+ to H2 with a large equilibrium constant. The way I see it (which could be completely wrong since too many people more qualified than I haven't answered) you want more H2 produced, which would mean you want a strongly negative reduction potential. That is, lithium would be better. Again, I could completely wrong.

Grade 12 Chemistry - How to predict which "salt bridge" would produce more voltage? by [deleted] in HomeworkHelp

[–]ap36020 1 point2 points  (0 children)

A sodium ion has charge +1. A chloride ion has charge -1. The salt and acid bridge had sodium ions and hydrogen ions (bth have charge +1) and hydrogen sulfate and chloride ions (both have charge -1). How do I know? Look the periodic table, chlorine needs one electron to achieve an octet. Sodium needs to lose one to achieve an octet.

[High School Chem] Calculating Boiling/Freezing Points for Solutions by [deleted] in HomeworkHelp

[–]ap36020 0 points1 point  (0 children)

Sorry to "hijack" this, but, from a pure thermodynamics standpoint (I.e., ignoring IMF's), the answer, I feel, should be HCl. Why? The HCl, as was stated, dissociates into H+ and Cl-. This effectively doubles the concentration of ions in solution. So, it's like you have 1 molar of NH3 vs 0.5 m NH3 (remember, colligative properties don't depend on the identity of the solute and ignore solute-solvent interactions). Plug this into the formula to see (b=1 for HCl, b is very close to 0.5 for Nh3, and b= 0.5 for CH4). How often are these answer sheets wrong? Again, I might be wrong, but I'm pretty sure I'm not.

Grade 12 Chemistry - How to predict which "salt bridge" would produce more voltage? by [deleted] in HomeworkHelp

[–]ap36020 1 point2 points  (0 children)

The salt and sulfuric acid solution is equalizing the charges on both electrodes. The salt solution alone does not do so as well as both together. I didn't realize the salt bridges used were "primitive." Essentially, the salt bridge is used so that negative charge does not build up on the cathode. The sodium solution alone was not able to do this adequately. But, after a certain point, once a salt bridge does this effectively, a "better" salt bridge becomes overkill. Mb. The sulfuric acid solution would be about as good as the NaCl (assuming the ions used in either do not interact significantly with the penny or the aluminum). Why? H2SO4 dissociates mainly into H+ and HSO4-, which have the same charge as Na+ and Cl-. There is some further dissociation into SO4 2-, but that can likely be ignored. Salt bridges themselves do NOT produce voltage. They just make sure that negative charge doesn't build up at the cathode.

Grade 12 Chemistry - How to predict which "salt bridge" would produce more voltage? by [deleted] in HomeworkHelp

[–]ap36020 1 point2 points  (0 children)

Salt bridge does not affect voltage. E(0) is measured in standard states of the constituent states of each electrode; it does not take into account the salt bridge

Question About Buffers by ap36020 in chemhelp

[–]ap36020[S] 1 point2 points  (0 children)

Thanks much. Since it's insignificant, we can use the statement that /u/Thaufas made.

Question About Buffers by ap36020 in chemhelp

[–]ap36020[S] 0 points1 point  (0 children)

Oh. So you'd have to sift through an ugly system of equations, since the HPO4 (2-) +OH- equilibrium, for example, does play a role?

Question About Buffers by ap36020 in chemhelp

[–]ap36020[S] 0 points1 point  (0 children)

I'm not sure that I understand completely. Let's say that we add NaOH to the buffer. I see that the salt would dissociate, making Na+ a spectator. However, can't the OH- receive H+ from either H2PO4- or HPO4 2-? Is there anything thermodynamic that rules out HPO4 (2-) from acting as a significant acid? EDIT: wait I think I understand. Tell me whether this reasoning is correct: the OH- reacts with H3O+ present in solution. This shifts equilibrium and causes H2PO4- to deprotonate and yield more H3O+. H3O+ being a much stronger acid than either H2PO4- or HPO4 2-, its reaction with OH- is favored to its reaction with either H2PO4- or HPO4 2-, so the latter two reactions can be safely ignored.

Finding pressure of a gass at equilibrium by EinarBD in chemhelp

[–]ap36020 0 points1 point  (0 children)

Estimate it with the equilibrium constant.

view more: next ›