<p>^umm i would memorize all of them?</p>
<p>does anybody else absolutely hate the relationship analysis questions? I lose half my points on those, is there some easy way to get them right? lol</p>
<p>Well, the problem is that different sites and textbooks usually have slightly different version of solubility rules? Where can I find a site where they have solubility rules that are tested on the SAT II test but doesn’t overkill on information?</p>
<p>Does anyone know if kaplan tests are notoriously more difficult than the real test because i just got around a 710/720 ish on the kaplan practice test 3 lol…</p>
<p>well 8 careless errors so actuall 740-760 assuming on test date i am less careless(very attentive test taker under pressure)</p>
<p>t-10 hours</p>
<p>LETS GOOO!OO!O!O!O!O </p>
<p>GO BIG OR GO HOME (800)!!!</p>
<p>yea!</p>
<p>I hate careless mistakes. I’m hoping for an 800 if everything goes right. Quick question to you Chem takers: If both ions of a salt hydrolyze in water, how do you know whether the solution will be basic or acidic?</p>
<p>depends on the strong acids and bases list i think</p>
<p>cb didn’t include explanations for the answers in their sat ii study guide book… can anybody explain these to me? </p>
<ol>
<li>The volume of the dry hydrogen gas at 1 atm and room temperature would be
a) (25.2)(749 + 19.8)/760 mL
b) (25.2)(760-19.8)/749.8 mL
c) (25.2)(749.8-19.8)/760 mL
d) (749.8-19.8)/(760)(25.2) mL
e) (760-19.8)/(749.8)(25.2) mL</li>
</ol>
<p>The answer is “c”</p>
<p>from user rockermcr:</p>
<p>"Initial conditions:
V= 25.3 mL
P= The atmospheric pressure and the vapor pressure are opposed in direction, and two opposing vectors counteract one another. As such, the pressure is 749.8 mm Hg - 19.8 mm Hg. Don’t bother attempting to convert this to kPa because you don’t have a calculator.</p>
<p>The temperature remains constant, and is thus not a necessary aspect of the calculations.</p>
<p>Now, you should recall Boyle’s gas law, which may be expressed as:</p>
<p>P1<em>V1 = P2</em>V2</p>
<p>You know that P2 is equal to 1 atm, and you should be aware that 1 atm is equal to 760 mm Hg. Now, your pressure is expressed in the same units, and all that’s left is to calculate the final volume, the volume under a pressure of 760 mm Hg</p>
<p>P1V1 = P2V2
(749.8 mm Hg - 19.8 mm Hg)(25.2 mL) = (760 mm Hg)V2
V2 = ((749.8 mm Hg - 19.8 mm Hg)(25.2 mL))/760 mm Hg"</p>
<p>here you go.</p>
<p>ahh thank you so much!
edit: oh i realized i forgot to include the lab data that goes along with that question, i’m glad you knew which question i was referring to haha </p>
<p>Also, can anybody explain this one to me: </p>
<p>Temperature (C)<br>
60<br>
70<br>
80<br>
90<br>
100 </p>
<p>Vapor Pressure of Ethyl Alcohol (mm Hg)
350
538<br>
813
1182
1698 </p>
<p>The barometric pressure on Pikes Peak (14109 ft) in Colorado averages 455 mm Hg. From the table above, one can conclude that the boiling point of ethyl alcohol at this altitude would be</p>
<p>a) 100C
b) between 90C and 100C
c) between 80C and 90C
d) between 70C and 80C
e) between 60C and 70C</p>
<p>the answer is e</p>
<p>@IAmCool
Assuming that it’s a chart, its boiling temperature is 60 C at 350 mm Hg and 70 at 538 mm Hg. 455 lies between 350 and 538, so it’s e</p>
<p>Yeah it is a chart I couldn’t format it here. Thanks!!</p>
<p>How helpful do you guys think it would be to memorize the VSEPR chart, with the hybridizations and orbitals and so on? My Barrons book had a few questions that would necessitate knowing it, but on the Princeton Review test I took, there weren’t any. What do you guys suggest?</p>
<p>@anrajg
seriously Barron’s do not really help, unless you already gained 800s on other practice tests and need more challenges. I only worked on PR and a bit Kaplan in like two months to get a 790 on Jan test. Good luck :)</p>
<p>Ah it’s over now. That wasn’t so bad, was it?</p>
<p>So how do u guys think u did? Which types of questions did u find the hardest?</p>
<p>I thought it was pretty alright, there were still some questions that had me completely stumped, but overall, it was easier than I thought it’d be!</p>
<p>harmful chemical?</p>
<p>It was…okay.</p>