Not exactly a chemistry joke, more like a pun.
It's the end of 14B and it's been a good run. Just wanted to say that we Lav-elle you, Professor :)
Search found 13 matches
- Thu Mar 10, 2016 11:13 am
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 2989078
- Thu Mar 03, 2016 11:09 am
- Forum: *Constitutional and Geometric Isomers (cis, Z and trans, E)
- Topic: Higher Priority
- Replies: 2
- Views: 9230
Re: Higher Priority
CH3 because it has a higher molecular weight, I think.
- Thu Feb 25, 2016 11:37 am
- Forum: *Free Energy of Activation vs Activation Energy
- Topic: Potential Energy vs Free Energy
- Replies: 1
- Views: 1269
Potential Energy vs Free Energy
On the homework we were asked to draw both a potential energy graph and a free energy graph (by this, I mean we used these as labels for the y-axis) for an organic reaction. I don't remember discussing potential energy of a reaction during lecture, is this something I might have just spaced out on o...
- Thu Feb 18, 2016 11:11 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: k in the Arrhenius Eq
- Replies: 1
- Views: 449
Re: k in the Arrhenius Eq
The slope is negative for the line but it doesn't mean that the k value is negative. If the k value itself was negative, then in the integrated rate law equations for first and zeroth order, we would have a double negative, resulting in a positive slope. Like if k=-1 for a first order reaction, then...
- Fri Feb 12, 2016 5:38 pm
- Forum: General Rate Laws
- Topic: Derivation of the Integrated Rate Law
- Replies: 1
- Views: 387
Re: Derivation of the Integrated Rate Law
It doesn't matter too much in my opinion. We'd just derive each one the same way and more or less get the same equation, just differing by a constant. 1/a, 1/b, 1/c and so on are just constants, which can be "pulled out" during integration. I don't think there's any different equation we h...
- Fri Feb 12, 2016 5:34 pm
- Forum: General Rate Laws
- Topic: Slow step vs fast step
- Replies: 1
- Views: 513
Re: Slow step vs fast step
Don't take my word for it, but most likely it'll be given to us. That's what I've been seeing so far from all the homework problems.
- Thu Feb 04, 2016 10:32 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Writing cell diagram: figuring out order
- Replies: 2
- Views: 572
Re: Writing cell diagram: figuring out order
From what it seems to me, in the anode we usually write the (s) form first, before the (aq). I'm not 100% sure why, but it's just a general pattern I've been seeing while doing these problems. I'm also thinking because it acts as a conductor or some sort, like how we write Pt(s) first on the left-ha...
- Thu Jan 28, 2016 8:03 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Two Gibbs Free Energy Formulas
- Replies: 1
- Views: 427
Re: Two Gibbs Free Energy Formulas
I think the question will make it very obvious which equation you should use. If it mentions equilibrium or concentrations then most likely you'll use the one you mentioned. If it gives you information about enthalpy and entropy then use the deltaG = deltaH - TdeltaS.
- Thu Jan 21, 2016 11:20 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy in irreversible processes
- Replies: 1
- Views: 362
Entropy in irreversible processes
Hi everyone! As I was doing the homework (and checking the solutions manual at the same time), it seems like we use the deltaS = nR ln V2/V1 formula even for irreversible processes. I think it's problem 9.13 where I encountered this. Since we "derived" this formula assuming that it was a r...
- Thu Jan 14, 2016 10:24 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Heat given off by reaction
- Replies: 1
- Views: 1334
Re: Heat given off by reaction
Where is this example? Exothermic reactions have negative enthalpy by definition, don't they? I feel like either there's a mistake or you're misinterpreting this example. When heat is given off by the reaction, it's already implied that there is a negative energy change in the system because the ene...
- Fri Jan 08, 2016 5:44 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Calculating Standard Reaction Enthalpy
- Replies: 1
- Views: 367
Re: Calculating Standard Reaction Enthalpy
It's because the products are being formed, whereas the reactants are being broken apart in the reaction. Take the example from our course reader, CH4 + 2 O2 --> CO2 + 2 H2O. CH4 is being broken down in this reaction, instead of taking the standard enthalpy of formation of CH4, we take its negative ...
- Mon Nov 23, 2015 7:26 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Video: Le Chatelier's Principle and Equilibrium Calculations
- Replies: 2
- Views: 783
Video: Le Chatelier's Principle and Equilibrium Calculations
Here is a video explaining problem 117 of chapter 17. We cover Le Chatelier's Principle and the ICE Box method of calculation.
Members of group: Raymond Le (3G), Trixie Le (3J), and Tram Vo (3J)
Members of group: Raymond Le (3G), Trixie Le (3J), and Tram Vo (3J)
- Fri Oct 09, 2015 10:22 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ionic radius
- Replies: 2
- Views: 619
Re: Ionic radius
The actual value of the radii probably doesn't matter. As long as you recognize the patterns/trends across the periodic table you should be able to rank them accordingly.