Search found 53 matches
- Tue Mar 16, 2021 12:27 am
- Forum: Student Social/Study Group
- Topic: Book Recommendations
- Replies: 135
- Views: 18480
Re: Book Recommendations
I've read the Selection Series so many times and love it more and more each time. Definitely recommend! It's kind of like a cross between The Bachelorette and Hunger Games.
- Tue Mar 16, 2021 12:15 am
- Forum: Student Social/Study Group
- Topic: Playlist
- Replies: 86
- Views: 8648
Re: Playlist
I've been in love with Japanese 80s City Pop for the past couple of months! It's literally the best! Here's a compilation I found and love a lot. I literally listen to it everyday. https://www.youtube.com/watch?v=0cxJ4Mg_q1M&t=66s
- Tue Mar 16, 2021 12:07 am
- Forum: Student Social/Study Group
- Topic: On Campus class vs. remote
- Replies: 21
- Views: 1578
Re: On Campus class vs. remote
I really hope they do hybrid if they don't go with fully remote. I definitely don't want in-person if theres going to be like 400+ students in a lecture. Plus, I really enjoy the flexibility of having classes online. Also, I don't have to stress about walking and making it to my 8am on time if it's ...
- Tue Mar 16, 2021 12:01 am
- Forum: Student Social/Study Group
- Topic: Plans for Summer/school year
- Replies: 34
- Views: 1832
Re: Plans for Summer/school year
I'm trying to take BL and CL during the summer but they got filled up when I tried to enroll. :( Does anyone know what the likelihood of getting off the waitlist is? I think I'm like the third person on the waitlist. Aside from that, I have a whole list of TV shows, animes, and kdramas to catch up on.
- Mon Mar 15, 2021 11:57 pm
- Forum: Student Social/Study Group
- Topic: Planning on dorming in the Fall?
- Replies: 61
- Views: 4037
Re: Planning on dorming in the Fall?
I love being home, but I also want to get out (I think my family is tired of me too lol). I want to dorm if things with covid get better. However, I've also thought about getting an apartment instead too. Either way, I'm probably not going to be home in the fall (or at least try to).
- Fri Mar 12, 2021 10:14 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidation Numbers: Provided or memorize?
- Replies: 26
- Views: 2130
Re: Oxidation Numbers: Provided or memorize?
You'll probably have to figure them out yourself, but there are lots of videos on youtube that are really helpful. There are general rules to follow when trying to find the oxidation numbers, but it's pretty simple once you get the hang of it.
- Fri Mar 12, 2021 10:07 pm
- Forum: Balancing Redox Reactions
- Topic: Balance reaction using OH- or H+
- Replies: 18
- Views: 859
Re: Balance reaction using OH- or H+
When it's in an acidic solution, then you use H+. When it's in a basic solution, then you use OH-. However, when solving for a basic solution, some people actually solve it like an acidic solution at first and then add OH- to both sides, turning the H+ into water. There are multiple ways to balance ...
- Fri Mar 12, 2021 10:00 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: EA
- Replies: 23
- Views: 1360
Re: EA
They are both the same thing. Different people write it differently, but pretty much the same.
- Fri Mar 12, 2021 9:41 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Chemical Kinetics Review session with TA
- Replies: 4
- Views: 295
Re: Chemical Kinetics Review session with TA
Some TAs might have posted on CCLE too, but if you can't find them then I would definitely email. :)
- Wed Mar 10, 2021 4:38 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 6L.5 d
- Replies: 1
- Views: 165
6L.5 d
Hi! Can someone please help me with 6L.5 d? I looked at the solution manual, and it says that the cell is Au(s)|Au3+(aq)||Au+(aq)|Au(s). How did they get that answer? Like why is there solid Au on both sides?
- Sun Mar 07, 2021 8:40 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: graphs and order
- Replies: 19
- Views: 959
Re: graphs and order
0th order: [A] vs time (decreasing linear)
1st order: ln[A] vs time (decreasing linear)
2nd order: 1/[A] vs time (increasing linear)
I would look back at Lavelle's lecture. He draws them out on the board and explains them.
1st order: ln[A] vs time (decreasing linear)
2nd order: 1/[A] vs time (increasing linear)
I would look back at Lavelle's lecture. He draws them out on the board and explains them.
- Sun Mar 07, 2021 8:31 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: K
- Replies: 10
- Views: 696
Re: K
You can determine k depending on the question. For instance, you can calculate it if you are given multiple rates with concentrations and initial rates. You can also figure out by looking at a graph. I recommend checking out some week 9 worksheets from the UA sessions. They were really helpful with ...
- Sun Mar 07, 2021 8:22 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Units for reaction rates
- Replies: 15
- Views: 1143
Re: Units for reaction rates
Someone already said what the units are above, but you can also figure it out by writing out the equation and cancelling out the units. Reaction rate = Molarity/time Units for k: 0th order: rate = k[A] 0 -> M/s 1st order: rate = k[A] 1 -> rate/[A] = k -> (M/s)/M -> 1/s 2nd order: rate = k[A] 2 -> ra...
- Sun Mar 07, 2021 8:08 pm
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: What was your favorite chem topic?
- Replies: 137
- Views: 12969
Re: What was your favorite chem topic?
I didn't have Lavelle for 14A but I really enjoyed learning about Lewis structures and molecular structures. Brought back a lot memories of chem in high school. :)
- Sun Mar 07, 2021 8:02 pm
- Forum: General Rate Laws
- Topic: Units
- Replies: 10
- Views: 478
Re: Units
Remember that the units are always concentration per time. Lucy is right when she said that zero order is generally M/s, 1st order is 1/s and 2nd order is 1/M*s, but I would say the best thing to do is just write it out and cancel them out manually if you can't tell.
- Sun Feb 28, 2021 10:53 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: E naught = 0
- Replies: 13
- Views: 2037
Re: E naught = 0
E naught is zero, because at standard condition, the concentrations are equal in the cell.
- Sun Feb 28, 2021 9:34 pm
- Forum: Balancing Redox Reactions
- Topic: Standard Potentials and Reactions
- Replies: 12
- Views: 721
Re: Standard Potentials and Reactions
Yes, I'm pretty sure the standard potentials and reaction or at least enough information for us to write out the reaction will be provided for us.
- Sun Feb 28, 2021 9:27 pm
- Forum: Balancing Redox Reactions
- Topic: states of matter
- Replies: 58
- Views: 2712
Re: states of matter
Yes, unless otherwise stated, you include the phases. I spent 30 mins on a problem because I was only missing the phases.
- Sun Feb 28, 2021 9:23 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing Redox Reactions
- Replies: 6
- Views: 401
Re: Balancing Redox Reactions
You add H2O to balance oxygen atoms, so you add it to the side with less oxygen atoms.
- Sun Feb 28, 2021 9:17 pm
- Forum: Balancing Redox Reactions
- Topic: Sapling #1 Glitch
- Replies: 16
- Views: 903
Re: Sapling #1 Glitch
Usually when a glitch occurs, I either refresh the page, log out and log back in, or change browsers. One of them usually works for me.
- Sun Feb 21, 2021 9:08 pm
- Forum: Balancing Redox Reactions
- Topic: Reducing vs oxidizing agents
- Replies: 16
- Views: 914
Re: Reducing vs oxidizing agents
Probably not the most helpful, but I always thought of the opposites. Oxidizing agents are the things getting reduced and reducing agents are the things that are getting oxidized.
- Sun Feb 21, 2021 9:00 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: delta U=0
- Replies: 17
- Views: 2704
Re: delta U=0
In an isothermal process, temperature is constant, so the heat absorbed by the gas equals the work done by the ideal gas on its surroundings. Thus, q=-w and by the equation ΔU = q+w , the net change in the internal energy is 0.
- Sun Feb 21, 2021 8:52 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Delta G and G naught
- Replies: 46
- Views: 4755
Re: Delta G and G naught
Delta G naught is the change in Gibbs free energy at standard conditions (1 atm and 25 degrees Celsius/298.15 K) , whereas Delta G is the change at a specific condition.
- Sun Feb 21, 2021 8:49 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Q and K
- Replies: 40
- Views: 2996
Re: Q and K
If Q<K, there are more reactants than products. The formation of products is favored in the forward reaction, because there is more reactants to make products. The opposite is also true. If Q > K, there are more products than reactants. The formation of products is favored in the reverse reaction (f...
- Sun Feb 21, 2021 8:42 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Closed System
- Replies: 52
- Views: 2996
Re: Closed System
A closed system is not necessarily insulated, but rather sealed. As a result, matter cannot be transferred, but energy can. An example would be an ice back and how the contents inside sealed within, but the heat between body and ice pack are still being transferred between one another.
- Sun Feb 14, 2021 9:30 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Is it necessary to memorize Cp,m or Cv,m values? [ENDORSED]
- Replies: 26
- Views: 1456
Re: Is it necessary to memorize Cp,m or Cv,m values? [ENDORSED]
Kaleb Tuliau 3E wrote:Is it necessary to remember the change of G values of each bond ?
If you are referring to delta G of each compound in a reaction, then I do not think so. It will probably be provided for us in a table or something like that.
- Sun Feb 14, 2021 9:18 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Likeliness to form products/reactants
- Replies: 27
- Views: 1026
Re: Likeliness to form products/reactants
When ∆G < 0 (negative) the forward reaction is spontaneous. Products are favored.
When ∆G > 0 (positive), the forward reaction is non spontaneous (reverse reaction spontaneous). Reactants are favored.
When ∆G > 0 (positive), the forward reaction is non spontaneous (reverse reaction spontaneous). Reactants are favored.
- Sun Feb 14, 2021 9:12 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Equilibrium constant
- Replies: 3
- Views: 264
Re: Equilibrium constant
The more negative the delta G, the larger your K value will be. A negative delta G means that the reaction is spontaneous, which favors the formation of products. More products equal a larger K value.
- Sun Feb 14, 2021 9:04 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: What's the difference between delta G and delta G°
- Replies: 7
- Views: 16925
Re: What's the difference between delta G and delta G°
Where ∆G is the difference in the energy between reactants and products. ∆G° is at standard conditions (1 atm and 25 degrees Celsius). ∆G° is always the same because it is referring to when the reactants/products are at standard temperature/pressure. As the rxn goes towards equilibrium, ∆G changes b...
- Sun Feb 14, 2021 8:54 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: R Constant
- Replies: 91
- Views: 7625
Re: R Constant
To figure out which R value to use, you pretty much look at the units involved. See which ones you want to match up/cancel out.
- Sun Feb 07, 2021 5:20 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Combustion = Exothermic
- Replies: 23
- Views: 929
Re: Combustion = Exothermic
Yes, combustion does require energy to break bonds, however, the energy released to form the new bonds is greater than the energy taken in. Thus, the reaction is overall releasing energy and exothermic.
- Sun Feb 07, 2021 5:06 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: enthalpy and heat
- Replies: 10
- Views: 456
Re: enthalpy and heat
q and delta H are not interchangeable unless they are under constant pressure. When they are under constant pressure, q and delta H are equal to each other.
- Sun Feb 07, 2021 5:01 pm
- Forum: Phase Changes & Related Calculations
- Topic: Endothermic v. Exothermic
- Replies: 139
- Views: 17415
Re: Endothermic v. Exothermic
Endothermic reactions will always have a positive delta H, because they are taking in heat/energy. Exothermic reactions will always have a negative delta H, because they are releasing heat/energy.
- Sun Feb 07, 2021 4:10 pm
- Forum: Phase Changes & Related Calculations
- Topic: Define Phase Change
- Replies: 78
- Views: 5781
Re: Define Phase Change
A phase change is when a substance changes from one state of matter to another. i.e. solid -> liquid (melting), liquid -> gas (vaporization), gas -> liquid (condensation), liquid -> solid (freezing), solid -> gas (sublimation), gas ->solid (deposition).
- Sun Feb 07, 2021 4:04 pm
- Forum: Phase Changes & Related Calculations
- Topic: Vapor vs gas
- Replies: 121
- Views: 14337
Re: Vapor vs gas
Yes! Both vapor and gas are the same and interchangeable. :)
- Sun Jan 31, 2021 10:21 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Sapling WEEK 3/4 Q #5
- Replies: 4
- Views: 182
Re: Sapling WEEK 3/4 Q #5
Hi! It seems like other people already gave you the process on how to solve it, but something to also notice are the phases! HCl is both an aqueous solution and gas here, so you have to make sure you are cancelling out the ones with the same phases. I had some difficulty on this question earlier bec...
- Sun Jan 31, 2021 10:09 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Syllabus Problems
- Replies: 6
- Views: 203
Re: Syllabus Problems
Dr. Lavelle said that he's going to be going out of order, so he'll probably go over the skipped material but later on. I don't think you should worry too much. :)
- Sun Jan 31, 2021 10:05 pm
- Forum: Ideal Gases
- Topic: Chem BL
- Replies: 107
- Views: 10056
Re: Chem BL
Hi! I actually have a similar problem. I'm not sure if I should take chem 14BL next quarter with 14C or take 14BL and 14CL during the summer. Does anyone have any advice? Thanks :)
- Sun Jan 31, 2021 9:52 pm
- Forum: Ideal Gases
- Topic: Reversing Reactions
- Replies: 68
- Views: 2675
Re: Reversing Reactions
The K of the reverse reaction is the inverse of the forward reaction.
A + B <-> C
Forward reaction: K = [C] / [A][B]
Reverse Reaction: K = [A][B] / [C] = 1/K
A + B <-> C
Forward reaction: K = [C] / [A][B]
Reverse Reaction: K = [A][B] / [C] = 1/K
- Sun Jan 31, 2021 9:45 pm
- Forum: Ideal Gases
- Topic: Kp?
- Replies: 30
- Views: 1125
Re: Kp?
Yes, Kp only applies to partial pressure of gases, while Kc can have concentrations of both gases and aqueous solutions.
- Sun Jan 24, 2021 8:20 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Making the Approximating for X: K or % Ionization?
- Replies: 6
- Views: 294
Re: Making the Approximating for X: K or % Ionization?
It's better to check with % ionization. If the % ionization is greater than 5% then you can not approximate even if your K is less than 10^-3.
- Sun Jan 24, 2021 7:59 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: X Approximations
- Replies: 23
- Views: 963
Re: X Approximations
You can approximate when your K value is less than 10^-4. We can assume that x is small enough that we can ignore -x. Remember that this does not mean we can ignore x^2 (I'm just adding this bit b/c someone asked about this on another post). The approximation can be checked by finding the % ionizati...
- Sun Jan 24, 2021 7:20 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Sapling Question 3
- Replies: 8
- Views: 621
Re: Sapling Question 3
I began by writing out the equation and then made an ice box. I wrote out the Ka expression and solved for x using the quadratic formula. The % ionization is higher than 5%, so you can't approximate for this problem. The value that you find for x is also equal to [H+]. To find the % ionization, divi...
- Sun Jan 24, 2021 6:57 pm
- Forum: Ideal Gases
- Topic: Omitting solid/liquid
- Replies: 19
- Views: 810
Re: Omitting solid/liquid
Solids and liquids are omitted from the equilibrium constant, because they have a constant concentration. They don't make a difference in the expression, and thus omitted.
- Sun Jan 24, 2021 6:49 pm
- Forum: Ideal Gases
- Topic: How can we identify when to use the ideal gas law?
- Replies: 11
- Views: 703
Re: How can we identify when to use the ideal gas law?
Hi!
We can use the ideal gas law when we are given values for pressure, volume, concentration, and temp except for one. You can use it to solve for the missing variable. For example, in some of the problems we've done, we've used it to convert from concentration to pressure and vice versa.
We can use the ideal gas law when we are given values for pressure, volume, concentration, and temp except for one. You can use it to solve for the missing variable. For example, in some of the problems we've done, we've used it to convert from concentration to pressure and vice versa.
- Sun Jan 17, 2021 7:47 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Accessing the E-textbook [ENDORSED]
- Replies: 125
- Views: 34727
Re: Accessing the E-textbook [ENDORSED]
Pretty sure that Sapling is mandatory, and will actually be collected midnight of the following Sunday, however, is this the only "homework" due?? Yes, I believe Sapling is the only mandatory homework. Professor Lavelle gives us textbook problems as well but those problems are not graded....
- Sun Jan 17, 2021 7:41 pm
- Forum: Ideal Gases
- Topic: reversing reactions
- Replies: 83
- Views: 6001
Re: reversing reactions
The K of the reverse reaction would be the inverse. 1/K or K-1.
EX. [A] + [B] <-> [C]
KFORWARD = [C] / [A][B]
KREVERSE =[A][B] / [C] , which is the reciprocal/inverse of the forward reaction.
EX. [A] + [B] <-> [C]
KFORWARD = [C] / [A][B]
KREVERSE =[A][B] / [C] , which is the reciprocal/inverse of the forward reaction.
- Sun Jan 17, 2021 7:30 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kw constant
- Replies: 25
- Views: 930
Re: Kw constant
[H2O] is in excess. Because there is a lot of H2O a change in concentration would have minimal effect, and thus it is negligible.
- Sun Jan 17, 2021 3:54 am
- Forum: Student Social/Study Group
- Topic: New Joke Chain
- Replies: 46
- Views: 3387
Re: New Joke Chain
Why should you go drinking with neutrons?
Because wherever they go, there's no charge!
Because wherever they go, there's no charge!
- Sun Jan 17, 2021 3:37 am
- Forum: Student Social/Study Group
- Topic: Comfort Movies
- Replies: 168
- Views: 36314
Re: Comfort Movies
I love watching Disney movies, especially Mulan, High School Musical, and The Parent Trap. I just love watching these movies so much and find them very comforting. I lowkey also have the entire script for these movies memorized haha. That's literally how much I love watching them. :)
- Fri Jan 08, 2021 3:27 am
- Forum: Ideal Gases
- Topic: Chemical Equilibrium Part 1A Post-Module Assessment
- Replies: 11
- Views: 2118
Re: Chemical Equilibrium Part 1A Post-Module Assessment
The correct answer would be A, because reactions never stop, but they do reach equilibrium when the concentrations of the products and reactants don't change. In order for this to happen, the forward and reverse reaction rates must be the same so there is no net change in the concentrations of reac...
- Thu Jan 07, 2021 4:59 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: concentration or partial pressure
- Replies: 7
- Views: 358
Re: concentration or partial pressure
Hi!
Yeah you wouldn't need to convert since they are asking for molar concentration and the values you're given are already in concentration (mol/L). If they asked for/given Kp or partial pressures, then you would need to convert using PV=nRT.
Yeah you wouldn't need to convert since they are asking for molar concentration and the values you're given are already in concentration (mol/L). If they asked for/given Kp or partial pressures, then you would need to convert using PV=nRT.
- Tue Jan 05, 2021 10:07 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kc vs Kp
- Replies: 14
- Views: 566
Re: Kc vs Kp
In terms of steps, I believe it's the same K = [product]/[reactant], but Kc uses concentration and Kp uses partial pressure. You can use PV=nRT to convert concentration to pressure and vice versa. Also, Kp is only for gases, while Kc is for gases and aqueous solutions. I think the values will be dif...