<p>sushant, not helpful</p>
<p>Thank god for that.</p>
<p>Got a question similar, if you increase concentration of the Anode, what will happen? What about increasing cathode?</p>
<p>anyone cramming right now? I need to but im not cuz i think its pointless. At this point, i cant get much better.</p>
<p>My comment was actually in response to #20.</p>
<p>okay look at the reaction. Ag is being oxidized! So its the anode. Anode = Oxidization. Cathode = Reduction.</p>
<p>Okay, I have no idea how this is working. I posted #26 before #25</p>
<p>But I asked, what does one do WITHOUT the equation?</p>
<p>And do they give us the Eo chart???</p>
<p>they wont be that gay on the FRQ. they ll give u the equation jeez. If they dont, they ll have a picture. Then there wont be a problem at all.</p>
<p>and yes they do give u a chart with all the Eo.</p>
<p>I don't think they can give us the problem w/out the eqn. If they do, look at electronegativity in regards to the periodic table.</p>
<p>even if they dont give you the eq you have the potential chart so you can just look up the values there and decide which one will form a metal and which will form an ion</p>
<p>I have an old AP problem with a pic of an electrochemical cell with Cr and Cu, no indicated directionality, and no eqn. That's why I asked.</p>
<p>They provide the chart of reduction potentials. That's where you look if there's no equation, or if they ask you to write the equations.</p>
<p>Thanks. You all are compositely so helpful! Another question. Could someone clarify the diff btwn Eo and E? as in the two e's in the equation E= Eo -RT/nF ln Q? (thanks.)</p>
<p>Eo is the standard and the E is when you change the Q.</p>
<p>Nernst equation, right?</p>
<p>E is the actual reduction potential. It's like deviation from ideal.</p>
<p>Eo is the standard (ideal) potential.</p>
<p>Thanks again, yall.</p>