<p>I have a question about equilibrium: How do you write the net ionic equation for a reaction that occurs when C2H5NH2 solution is mixed with HCl?</p>
<p>If I don’t truncate my numbers until the very end in the Free REsponse section and end up off by a hundredth from the official score sheet, will I still receive credit?</p>
<p>
Not sure. My chemistry teacher would mark you wrong, but my physics teacher would mark you as right. (Not AP teachers though.)</p>
<p>But the AP exam specifically looks for significant digits, so I guess you have to round them?</p>
<p>I round to sig figs at the end of the problem for the answer. I don’t round while making the calculations.</p>
<p>Anyone have the answers for the 2004 released AP multiple choice?</p>
<p>
If you mean you round at the end of each part, ex. part a), b), etc, then you would be correct. If you only rounded at d) or e) I’m not sure if you’d be right or not.</p>
<p>Let me check if I have the 2004 answers.
edit: I don’t even have the questions, actually. Would you mind sending me those/the link for them? (:</p>
<p>
Yes, that’s right!</p>
<p>Yes can you send them to me too? It turns out the 2004 exam enclosed in my file was actually a 2002.</p>
<p>On the 2001 Free-response:
How does KMnO4 oxidize Cl- to Cl2?</p>
<p>@skateme</p>
<p>Here’s some multiple choice (answers not included and free response are floating everywhere so I’m not going to bother posting those)
2003: mr.nathan.hamblin.googlepages.com/2003apmc_20080108065817.pdf
Mock(I THINK): [AP</a> Calculus Practice Exams](<a href=“http://www.online.math.uh.edu/apcalculus/exams/]AP”>AP Calculus Practice Exams)</p>
<p>The 2008 one is released but I haven’t found it.
EDIT: I found a 2008 one but considering that I haven’t taken AP Calc BC yet, I’m not sure if it really is the exam or just a regular 2008 exam. I’d say that it’s the real thing but you should probably decide for yourself:</p>
<p><a href=“http://www.ilearnmath.net/help/index.php?page=apexamsuh2008bcexam1[/url]”>http://www.ilearnmath.net/help/index.php?page=apexamsuh2008bcexam1</a></p>
<p>Another question:</p>
<p>Can someone explain to me the relationship between temperature and solubility of gases?
Why does solubility of gases decrease as temperature increases?
I need to refreshen my memory :)</p>
<p>Thanks!</p>
<p>@Mikeypz</p>
<p>I’d assume it’s related to intermolecular forces: An increase in temperature = an increase in energy = less likely chance for IMFs to form.</p>
<p>Can someone confirm it please?</p>
<p>For question #7 part D on the 2001 Free Response (though this could apply to any situation really), why is it that when the cell potential is positive, K > 1?</p>
<p>A positive cell potential means ΔG is negative, which means the reaction is spontaneous. A reaction that is spontaneous in the forwards direction means that more products are produced at equilibrium. Remember K = products/reactants. If more products are present than reactants, K will be more than 1. If the reaction is not spontaneous in the forwards direction, there will be more reactants, so K will be less than 1. If products = reactants, then the cell is at equilibrium.</p>
<p>Thanks for the links!</p>
<p>@skateme</p>
<p>You’re welcome =] Your explanation made a lot of sense so thank you back!</p>
<p>so my teacher just assigned us a really long packet about reactions and organic chemistry this break, not good. It was really hard considering the fact we really never talked much about organics. How much of the test is about organic chemistry</p>
<p>
</p>
<p>But I thought if there were less IMFs, then it’d be more soluble because there isn’t as much force holding together molecules? I’m confused :p</p>
<p>Think of a soda, if it is colder, the gas particles are moving slower, and therefore are escaping less. Colder=more soluble FOR GASES. It’s the opposite for solids.</p>
<p>@Mikeypz</p>
<p>I just found this explanation. </p>
<p>
</p>
<p>Found on: [Temperature/Pressure</a> on Solubility](<a href=“http://www.elmhurst.edu/~chm/vchembook/174temppres.html]Temperature/Pressure”>http://www.elmhurst.edu/~chm/vchembook/174temppres.html)</p>
<p>Ohhh, gotcha. I think I understand better now!</p>
<p>So basically it’s more soluble at low temps because there’s not enough kinetic energy in molecules to break IMF, which means more particles are still in solution.</p>
<p>Oh, and @NYJ3TS
From what I can tell not many questions on the test are over organic chem.
All I’ve seen on practice tests (I’ve taken many… haha) are questions asking you to identify which structure is which.
Like, ketone, alcohol, aldehyde, etc etc.
You might want to memorize those! It won’t take long.</p>