Search found 35 matches
- Mon Mar 20, 2023 2:59 pm
- Forum: Calculating Work of Expansion
- Topic: reversible vs. irreversible expansion
- Replies: 2
- Views: 814
Re: reversible vs. irreversible expansion
Yes and we can see in an equation based on the arrow too if it goes in both directions. We discussed that phase changes are always reversible when we do problems with them.
- Mon Mar 20, 2023 2:56 pm
- Forum: Ideal Gases
- Topic: When to use R
- Replies: 3
- Views: 2079
Re: When to use R
Hi it should just be the 8.3145 value typically, but you use any R value that cancels out the other units in your problem.
- Mon Mar 20, 2023 2:54 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Saying Thank You to Dr. Lavelle
- Replies: 490
- Views: 708065
Re: Saying Thank You to Dr. Lavelle
Dr. Lavelle,
Thank you for showing up to each lecture with positive and happy energy. It made my mornings much more bearable and more motivated to pay attention and work hard!
Thank you for showing up to each lecture with positive and happy energy. It made my mornings much more bearable and more motivated to pay attention and work hard!
- Mon Mar 20, 2023 2:53 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: achieve #14
- Replies: 2
- Views: 458
Re: achieve #14
Hi! So on the left it is the ln(8) and then one thing to make sure is that your Ea is in the same units as R. After this it should just be cross-dividing and solving for T2.
- Fri Mar 17, 2023 11:39 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Achieve Weeks 8-10 Question 20
- Replies: 6
- Views: 218
Re: Achieve Weeks 8-10 Question 20
Hi! So to do this question you just plug the Ea into the Arrhenius equation and then you can divide the catalyst solution by the noncatalyzed solution which will give you how many times faster the catalyzed reaction is compared to the noncatalyzed reaction.
- Fri Mar 17, 2023 11:00 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Derived Arrhenius Equation for T1 and T2
- Replies: 3
- Views: 134
Re: Derived Arrhenius Equation for T1 and T2
I dont recall learning this equation, I just figured it out through the practice problems. But I think that you also could derive it if need be, but it isnt really necessary
- Fri Mar 17, 2023 10:58 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Greater Standard Molar Entropies
- Replies: 2
- Views: 407
Re: Greater Standard Molar Entropies
Hi yes that was all right! I conceptualize it by thinking if there are more positions for the molecules like with gas and then liquid then there is higher entropy. Also, increasing molecular complexity directly goes up with entropy.
- Fri Mar 17, 2023 10:51 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalysts
- Replies: 3
- Views: 112
Re: Catalysts
I think there typically is not more than 1 catalyst but it is possible to have 2 that work together. Not sure how to figure out the strength though, interesting question! That definitely wont be on the exam though.
- Fri Mar 17, 2023 10:49 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Arrhenius equation understanding
- Replies: 2
- Views: 80
Re: Arrhenius equation understanding
^^ most of the practice problems ignore the A from the reaction altogether and therefore just assume that it is equal to 1 so unless given you can essentially just ignore it.
- Fri Mar 17, 2023 4:15 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Spontaneity in ∆G and E°
- Replies: 4
- Views: 146
Re: Spontaneity in ∆G and E°
Yes that is correct! A positive voltage is needed for E in order for it to be spontaneous and opposite for Gibbs.
- Thu Mar 16, 2023 10:29 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: A - Arrhenius Equation
- Replies: 3
- Views: 102
Re: A - Arrhenius Equation
Yes it is the frequency of the molecules colliding!
- Wed Mar 15, 2023 6:09 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing in Basic Condition
- Replies: 7
- Views: 382
Re: Balancing in Basic Condition
Hi! So yeah you do the exact same thing as you would do with acidic conditions which is where you get the H+. But you are going to add OH- to both sides so that this H+ will combine with the OH- to form a water molecule and you are left with the OH- molecules on the other side of the equation since ...
- Wed Mar 15, 2023 5:27 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Week 7- V standard and E standard conditions
- Replies: 2
- Views: 92
Re: Week 7- V standard and E standard conditions
Hi there I am a bit confused as well. What context did he say that E naught is always 0? I dont think this is possible since this means that there would be no cell potential and no reaction would take place. But I am not sure.
- Wed Mar 15, 2023 2:54 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: intermediates
- Replies: 16
- Views: 546
Re: intermediates
Yes, and they will never be in the overall reaction. So it is just something that is needed in the in-between processes to get the final products.
- Fri Mar 10, 2023 11:37 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: Study Video Suggestions
- Replies: 3
- Views: 134
Study Video Suggestions
Hey yall I was wondering if anyone has some good videos for practicing kinetics problems including the Arrhenius equation, I think I need to watch people work out some problems. Thank you!!
- Wed Mar 08, 2023 6:45 pm
- Forum: Balancing Redox Reactions
- Topic: Writing redox rxn
- Replies: 5
- Views: 143
Re: Writing redox rxn
No, I think as long as the correct terms cancel out and you are left with the equation that you need it doesn't matter :)
- Wed Mar 08, 2023 6:37 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: galvanic vs concentration cells
- Replies: 8
- Views: 184
Re: galvanic vs concentration cells
In the examples we looked at galvanic cells use spontaneous reactions to generate the current flow whereas with concentration cells have similar compositions of each of the products and solutions and as they reach equilibrium I believe they generate the current of energy.
- Wed Mar 08, 2023 6:33 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: electrolysis
- Replies: 2
- Views: 93
Re: electrolysis
Electrolysis is the process of using energy to drive a nonspontaneous reaction, so I think this would just be used when we want to push a reaction to occur when it wouldn't typically do it on its own (ex maybe the activation energy is too high for the rxn to occur naturally)
- Wed Mar 08, 2023 6:30 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: voltage vs potential
- Replies: 4
- Views: 116
Re: voltage vs potential
I think voltage is the same as potential difference since it's like the sum energy of the reaction.
- Thu Mar 02, 2023 11:18 am
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Pre-Equilibrium
- Replies: 9
- Views: 474
Re: Pre-Equilibrium
I believe they may be referring to any reaction that is not yet in equilibrium? Not sure though what was the context for this?
- Thu Mar 02, 2023 11:13 am
- Forum: Balancing Redox Reactions
- Topic: Achieve (W7-W8) #17
- Replies: 3
- Views: 90
Re: Achieve (W7-W8) #17
^^ I think we typically find that in this class partial pressure is equated to molarity for gases since it also is relating to its concentration
- Thu Mar 02, 2023 11:10 am
- Forum: Balancing Redox Reactions
- Topic: Achieve Week 7&8 #5
- Replies: 2
- Views: 103
Re: Achieve Week 7&8 #5
Hi there. So for this problem you don’t need to include the water in balancing the half reaction. You can first balance the half reactions on their own and figure out everything first. Then after this you can add in the waters to balance out the equations and then add H+ to balance out any extra Hs ...
- Tue Feb 28, 2023 1:37 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagram Format
- Replies: 2
- Views: 110
Cell Diagram Format
Hi y’all I just wanted to confirm the cell diagram. I know that the anode is all the way to the left and is then separated by | but what determines what goes closest to the salt bridge? I know we separate the phases with | I just am not sure when there’s the solution and the other molecules in conta...
- Tue Feb 28, 2023 1:25 pm
- Forum: Balancing Redox Reactions
- Topic: Study Video Recommendations
- Replies: 8
- Views: 207
Re: Study Video Recommendations
Omg just realized the person above recommended the same video as me lol, it was really helpful. Also this one below is a bit longer but is very helpful and in depth.
https://youtu.be/YWl4KHsUxuw
https://youtu.be/YWl4KHsUxuw
- Tue Feb 28, 2023 1:24 pm
- Forum: Balancing Redox Reactions
- Topic: Study Video Recommendations
- Replies: 8
- Views: 207
Re: Study Video Recommendations
Hi! This video really helped me out for balancing reactions under acidic or basic conditions which is when we add the water to balance out the equation!
https://youtu.be/N6ivvu6xlog
https://youtu.be/N6ivvu6xlog
- Tue Feb 28, 2023 1:22 pm
- Forum: Balancing Redox Reactions
- Topic: Week 7 and 8 Achieve Question 15
- Replies: 2
- Views: 108
Re: Week 7 and 8 Achieve Question 15
Hi! I struggled with this one too. the equation to find this is e=E0-(RT)/(nF) *lnQ So, you use the molar concentrations to find what Q is and then plug that in to find that part of the equation. To find E0 you would look at the standard reduction potentials page and figure out which part of the rea...
- Tue Feb 28, 2023 12:02 pm
- Forum: Balancing Redox Reactions
- Topic: Electrochemical Cell
- Replies: 6
- Views: 200
Re: Electrochemical Cell
Yes, its the generic term for the cells. There are different types that we discussed in class such as those with the salt bridge or the porous disk, but an electrochemical cell is simply the device that can generate electrical energy from the reactions that are occurring naturally.
- Tue Feb 28, 2023 12:00 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Isothermal
- Replies: 20
- Views: 946
Re: Isothermal
I dont think so, I am pretty sure as long as the temperature change remains 0 then it is isothermal. So while it typically would be a closed system as we have looked at, there can be isothermal systems that are not closed as long as delta t is 0.
- Tue Feb 28, 2023 11:56 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Achieve problem
- Replies: 2
- Views: 97
Re: Achieve problem
^^ also make sure that when accounting for the electrons you take the coefficients into account, but for the E0 you simply just use the standard reduction potentials. This got me last time on this problem. The oxidations numbers are only important in this case to calculate the moles of electrons.
- Tue Feb 28, 2023 11:51 am
- Forum: Balancing Redox Reactions
- Topic: Identifying Charge and Whether an Atom is Reduced/Oxidized
- Replies: 6
- Views: 185
Re: Identifying Charge and Whether an Atom is Reduced/Oxidized
There also is a resource for oxidation numbers in the book that tells you some basic rules. For example, O2 when attached to a nonmetal will have an oxidation number of -2. From this you can figure out the charge for the other atom in the molecule. Also, from the periodic table we can find some of t...
- Mon Feb 27, 2023 4:00 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Delta H and qp
- Replies: 3
- Views: 155
Re: Delta H and qp
OHH ok that makes so much more sense, I think I got a bit confused with it since I would just assume that Qp was given rather than found with that equation. Thank ya'll so much!!
- Sat Feb 25, 2023 12:18 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Delta H and qp
- Replies: 3
- Views: 155
Delta H and qp
Hey yall, I had a question about the relationship between delta h and qp. I know that we learned that they are equal to each other when there is constant pressure, but I also saw another equation where when pressure and temperature are constant then delta h is equal to delta u plus P delta V, so I w...
- Thu Feb 23, 2023 4:11 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Degeneracy and entropy
- Replies: 8
- Views: 613
Re: Degeneracy and entropy
A follow-up question for this, how can we calculate the number of positions? Do we need to draw out every possible structure or is there a formula that we can use to determine this if we are not given the number of positions?
- Tue Feb 21, 2023 8:29 pm
- Forum: Ideal Gases
- Topic: Gas constant R
- Replies: 14
- Views: 1672
Re: Gas constant R
As long as the units cancel out you're good! So definitely just look at those before choosing the R value on the page.
- Tue Feb 21, 2023 8:20 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Cv and Cp for Ideal Gases
- Replies: 15
- Views: 6083
Re: Cv and Cp for Ideal Gases
If both pressure and volume are constant we just use R right?