Search found 35 matches
- Sat Mar 18, 2023 10:28 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Final Grade Curve
- Replies: 2
- Views: 504
Final Grade Curve
Hi, I talked to several TAs and UAs and they all mentioned that after we get our final grades back, Professor Lavelle will see the averages and put a curve on our final grades if it is warranted. Although we haven't heard anything from Professor Lavelle himself so I'm not exactly sure either. Additi...
- Sat Mar 18, 2023 10:21 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalysts and Activation Energy
- Replies: 12
- Views: 967
Re: Catalysts and Activation Energy
To add to the other post that covered the answer. A good analogy to help with your question is thinking of a freeway with hundreds of cars in one line. If the slow step is the very first car in that one line and how they are below or maintaining the speed limit. It will slow down all of the other ca...
- Sat Mar 18, 2023 10:12 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: intermediate versus catalyst
- Replies: 10
- Views: 238
Re: intermediate versus catalyst
Through the different UA and TA sessions that I have gone to. They always say that an intermediate is thought of as being formed in the product and then used up in another step reactant. The catalyst was used up in the reactant and then formed in the product of another step.
- Sat Mar 18, 2023 10:08 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalyst Question
- Replies: 9
- Views: 688
Re: Catalyst Question
To add to the other posts that did a good job of explaining why the catalyst is not consumed in the course of a reaction. A simple way of thinking about it is like having a cookie jar and once you take out a cookie for a reaction then it will get replenished through the product of another reaction t...
- Sat Mar 18, 2023 9:58 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: How to determine the slow step?
- Replies: 18
- Views: 2552
Re: How to determine the slow step?
I know for the most part it should be stated in the given problem. Although earlier today in Gabriel Nitro's zoom he did show us how to tell which one was the slow/slowest step. This was by looking at the activation energy and if one of the reactions was much greater than the rest(takes a long time ...
- Sat Mar 18, 2023 9:55 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: initial rates method
- Replies: 6
- Views: 509
Re: initial rates method
To add to what Patrick said I remember in Gabriel Nitro's zoom, he mostly rounded for each number before continuing. Although he did mention that it would probably be best to wait until the end to round to get a more accurate value for the question. On the other hand, he also said that when you solv...
- Fri Mar 17, 2023 9:18 pm
- Forum: General Rate Laws
- Topic: Week 8-10 Assignment Question 7
- Replies: 9
- Views: 228
Week 8-10 Assignment Question 7
I'm wondering where I went wrong with trying to calculate the constant rate of K and how I do the last part of the question as well. I tried a couple of different ways to solve it but it doesn't seem to be correct. Any help would be appreciated. Screen Shot 2023-03-17 at 9.16.28 PM.png Screen Shot 2...
- Fri Mar 17, 2023 9:14 pm
- Forum: First Order Reactions
- Topic: Week 8-10 Assignment Question 11
- Replies: 8
- Views: 1448
Week 8-10 Assignment Question 11
I'm wondering where I went wrong with the last part of this question. I tried a couple of different ways to solve it but it doesn't seem to be correct. Any help would be appreciated.
- Sun Mar 12, 2023 10:57 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Units in Gibbs Equation
- Replies: 4
- Views: 193
Re: Units in Gibbs Equation
While you are correct with n referring to the moles, it refers to the moles of the electrons transfer instead of the moles of a reaction thus this wouldn't be canceled out the units. So you are left with J/mol as the final units.
- Sun Mar 12, 2023 10:51 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Concentration Cell, cathode vs anode
- Replies: 4
- Views: 176
Re: Concentration Cell, cathode vs anode
Yes, I do believe that the anode is the lower concentration of the two. As for the Nernst equation, it is anode/cathode.
- Sun Mar 12, 2023 10:48 pm
- Forum: Balancing Redox Reactions
- Topic: Reaction in basic/acidic solution
- Replies: 3
- Views: 108
Re: Reaction in basic/acidic solution
From what we have seen from our homework, I believe that it should indicate whether or not it is in a basic or acidic solution.
- Sun Mar 05, 2023 11:03 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Achieve #7
- Replies: 9
- Views: 262
Re: Achieve #7
For this question, I was first confused as well. What I did was started with the Pb(s) which is on the anode side then the half-reaction is Pbcl2(s) which should be on the anode side too. From there I looked at AgCl(s) and the half-reaction for that is Ag(s) which is on the cathode side. But you can...
- Sun Mar 05, 2023 9:32 pm
- Forum: Balancing Redox Reactions
- Topic: Week 5 and 6 Assignment Question 3 - Where did I go wrong
- Replies: 2
- Views: 103
Week 5 and 6 Assignment Question 3 - Where did I go wrong
I've attached an image of my balanced equation. From achieve it said that I balanced the oxygen and hydrogen but I didn't balance the electron transfer correctly. I have tried everything to help balance the electron transfer but I still can't figure it out. So I was wondering where am I going wrong ...
- Sun Mar 05, 2023 9:26 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagram
- Replies: 5
- Views: 157
Cell Diagram
For cell diagrams problems I understand that for the cathode side, you have to put Pt(s) for the electrode only when there are no solid metals on that and vice versa for the anode but why do we specifically use Pt(s) instead of something else?
- Sun Feb 26, 2023 10:42 pm
- Forum: Calculating Work of Expansion
- Topic: How do you do question 3 on homework 4&5
- Replies: 5
- Views: 200
Re: How do you do question 3 on homework 4&5
Why don't we use w=-P*deltaV for path A? I believe we don't use w=-P*deltaV for path A because it doesn't mention anything about external pressure. It does state the volume at which it expanding but for path B it specifically states external pressure which is when we would use the equation w=-P*del...
- Sun Feb 26, 2023 10:34 pm
- Forum: Calculating Work of Expansion
- Topic: Achieve Week 5 and 6 Assignment Q 3
- Replies: 4
- Views: 232
Re: Achieve Week 5 and 6 Assignment Q 3
You would first need to use the equation PV = nRT with the initial volume and R being 0.08206 because it is in units of L atm/mol K. Then plug the moles (n) into the work equation to get your answer.
- Sun Feb 26, 2023 10:30 pm
- Forum: Calculating Work of Expansion
- Topic: Achieve #3
- Replies: 7
- Views: 228
Re: Achieve #3
You would have to use the initial volume in the PV=nRT as it is asking for the volume at which we know the initial moles of
- Sun Feb 19, 2023 11:57 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Delta H at constant pressure
- Replies: 4
- Views: 180
Re: Delta H at constant pressure
When Qp is under constant pressure and when the system has no work done. Delta H would be the same as Qp
- Sun Feb 19, 2023 11:20 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy and Enthalpy
- Replies: 4
- Views: 115
Re: Entropy and Enthalpy
Enthalpy is the total amount of energy a system whereas entropy is the measurement of the change in enthalpy or temperature.
- Sun Feb 19, 2023 11:14 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Gibbs Free Energy
- Replies: 16
- Views: 571
Re: Gibbs Free Energy
When the reaction is non-spontaneous this will result in Gibbs free energy is positive. Thus the entropy is negative and the enthalpy is positive. If the reaction is positive then it will be negative with the entropy being positive and the enthalpy being negative
- Sun Feb 12, 2023 11:11 pm
- Forum: Calculating Work of Expansion
- Topic: Unit Conversion for w=-PV Problems
- Replies: 1
- Views: 57
Re: Unit Conversion for w=-PV Problems
I believe that those types of conversions are going to be on the Constants and Formula sheet that we are allowed to have with us for the exams.
- Sun Feb 12, 2023 11:05 pm
- Forum: Calculating Work of Expansion
- Topic: w=∆nRT, use T initial or T final?
- Replies: 7
- Views: 556
Re: w=∆nRT, use T initial or T final?
For w=∆nRT, the T should be delta T and to find that you need to first find the final temperature and then subtract that from the initial temperature. For question 17 they already gave you delta T which is 18.9 K.
- Sun Feb 12, 2023 10:53 pm
- Forum: Calculating Work of Expansion
- Topic: Work done by a system
- Replies: 17
- Views: 312
Re: Work done by a system
In the case that 350 J of work is done by the system. This would be added to U because the energy is being added.
- Sun Feb 05, 2023 11:16 pm
- Forum: Phase Changes & Related Calculations
- Topic: Why are ice packs endothermic?
- Replies: 22
- Views: 3806
Re: Why are ice packs endothermic?
From my understanding of what's in an instant ice pack, it has ammonium-nitrate fertilizer in some sort of concealed part in the pack with the water. When you squeeze the pack to make it cold, the water and the ammonium-nitrate fertilizer mix together causing the mixture to become an endothermic rea...
- Sun Feb 05, 2023 11:05 pm
- Forum: Phase Changes & Related Calculations
- Topic: Week 3 Q3
- Replies: 5
- Views: 116
Re: Week 3 Q3
"Do work on the surroundings" in this context would be an Exothermic reaction due to the fact that heat is being expelled into the surroundings.
- Sun Feb 05, 2023 10:56 pm
- Forum: Phase Changes & Related Calculations
- Topic: phase change curve
- Replies: 4
- Views: 128
Re: phase change curve
Isabella is 100% correct in that the whole system would increase. Both the water and the ice will begin to heat up but it may take a few degrees more for the ice to melt while in the water completely.
- Sun Jan 29, 2023 11:25 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: book answers
- Replies: 2
- Views: 107
Re: book answers
If you scroll down to the end of the table of contents in the textbook, there is a section called "Back Matter." The "odd-numbered exercises" tab should have the answer to every odd-numbered question in the book. I had the exact same question. Thank you so much for answering thi...
- Sun Jan 29, 2023 11:16 pm
- Forum: Ideal Gases
- Topic: achieve assignment, q5
- Replies: 2
- Views: 169
Re: achieve assignment, q5
I'm not 100% confident on this, but I figure I'll try to do it and explain because I need more practice. You want to start by converting the pH given to pOH. pOH = 14 - 9.325 = 4.675 Next, use the pOH to determine the concentrations of the protonated amine BH+ and OH-. [BH+] = [OH-] = 10^-pOH = 10^...
- Sun Jan 29, 2023 11:08 pm
- Forum: Phase Changes & Related Calculations
- Topic: HW 2 Q 7/8
- Replies: 5
- Views: 193
Re: HW 2 Q 7/8
For homework questions 7 and 8. After you get your x value and use -log to find the pOH you can simplify the pH+poH=14 where you can use subtraction to get the pH of the solution. Hope this helps!
- Sun Jan 22, 2023 11:48 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Week 2 Achieve #2
- Replies: 2
- Views: 96
Re: Week 2 Achieve #2
I believe the issue is that for this equation x^2 - 0.00487x + 9.5452 * 10^-4 = 0 you have the plus and minus in the opposite positions. It should be x^2 + 0.00487x - 9.5452 * 10^-4 = 0 instead and that would work.
- Sun Jan 22, 2023 11:35 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Homework Question #5
- Replies: 1
- Views: 79
Re: Homework Question #5
For this type of question, It is simply where you can choose any of the equations that were given. The ones that I used were 3H2(g)+3I2(g) ↽−−⇀6HI(g) and 2NH3(g)−⇀N2(g)+3H2(g). They give you the K values for them so I balanced the equations to get 2NH3(g)+3I2(g) ↽−−−⇀N2(g)+6HI(g). And so the k value...
- Sun Jan 22, 2023 11:23 pm
- Forum: Phase Changes & Related Calculations
- Topic: Achieve question #2
- Replies: 3
- Views: 167
Re: Achieve question #2
For this question, you don't need to plug x into -log(H3O+) and get 1.602. Instead, take your x value of 0.0025 and divide it by 0.137 M which is your percent ionization solution. As well as multiply that by 100% to get the percentage. So (0.0025/0.137)*100% will get you the percent ionization. Hope...
- Sun Jan 15, 2023 8:19 pm
- Forum: General Science Questions
- Topic: Rusty on High School Chem [ENDORSED]
- Replies: 347
- Views: 573998
Re: Rusty on High School Chem [ENDORSED]
I would say that looking at youtube videos or channels will greatly help. I know that I used to watch videos on subjects learned in 14A to have a deeper understanding of what was going on. As well as if I was confused about something that I could watch a video on quickly. I would suggest "Ninja...
- Sun Jan 15, 2023 8:12 pm
- Forum: Student Social/Study Group
- Topic: Final Jitters
- Replies: 457
- Views: 637838
Re: Final Jitters
Definitely start studying a while before the exams, and do as many practice problems as you can! Working out problems really helps solidify concepts and makes you prepared. Do not try cramming the night before; it never helps. Exactly. For this type of class doing practice problems will be the only...
- Sun Jan 15, 2023 8:05 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Question 9 on Week 1 HW
- Replies: 1
- Views: 83
Question 9 on Week 1 HW
I got my x value from the quadratic formal but what is the next step to get [NO]final as my answer? Thanks for any and all help.