Search found 57 matches
- Wed Mar 14, 2018 3:24 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 15.63
- Replies: 4
- Views: 542
Re: 15.63
Thank you! Was very confused by this question but this was helpful.
- Wed Mar 14, 2018 3:17 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 15.63 How to know what A is
- Replies: 7
- Views: 913
Re: 15.63 How to know what A is
Update: I saw there's a chart with values for A depending on the reaction. For this reaction (CO2 + OH- → HCO3-), A would be 1.5 x 10^10 L/mol*s. But even then, ln(1.5 x 10^10) does not equal -0.59. So why is -0.59 included in the solutions manual?
- Wed Mar 14, 2018 3:09 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: 15.63 How to know what A is
- Replies: 7
- Views: 913
Re: 15.63 How to know what A is
Not sure what you mean? You don't need A at all in this problem. Given that ln(k 2 /k 1 )=E a /R * (1/T 1 - 1/T 2 ), you just need to plug in values. Additionally, A is just the pre-exponential constant in the Arrhenius equation, so you could find it. What do you mean we could find it? How? How wou...
- Wed Mar 14, 2018 3:07 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: k' reverse reaction constant
- Replies: 6
- Views: 1102
Re: k' reverse reaction constant
Oh, okay, I was reading it as "k prime." Thank you.
- Wed Mar 14, 2018 2:54 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: k' reverse reaction constant
- Replies: 6
- Views: 1102
k' reverse reaction constant
Could someone please clarify why the reaction constant for a reverse reaction is k' (k prime)?
- Wed Mar 14, 2018 2:42 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: HW 15.49
- Replies: 2
- Views: 333
Re: HW 15.49
My guess is that it's okay to write it in the second step rate law as [HOBr] because that step is not rate-limiting (it's not the slower step). Thus the intermediate [HOBr] is still not in the overall rate law.
- Wed Mar 14, 2018 2:40 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: E cell value
- Replies: 2
- Views: 375
Re: E cell value
So because this is a Galvanic cell, we know that we want our Eº(cell) to be positive. We know that we're going to have to reverse one of the reduction half-reactions so that we have one reduction and one oxidation. Since our Eº(cell) needs to be positive, we'll need to make the larger of the two sta...
- Wed Mar 07, 2018 1:02 am
- Forum: General Rate Laws
- Topic: Rate Law
- Replies: 2
- Views: 280
Re: Rate Law
There might be an intermediate step for that last equation, like in the example from lecture on Friday with NO2 + CO → NO + CO2.
- Wed Mar 07, 2018 12:59 am
- Forum: General Rate Laws
- Topic: What equation is this?
- Replies: 1
- Views: 293
Re: What equation is this?
It's a form of the Arrhenius equation. From the textbook: The Arrhenius equation is used to predict the value of a rate constant at one temperature from its value at another temperature. You would take the standard Arrhenius equation for one temperature and the same for the next temperature, then su...
- Wed Mar 07, 2018 12:38 am
- Forum: General Rate Laws
- Topic: 15.19a Order
- Replies: 6
- Views: 762
Re: 15.19a Order
Just to understand what the soln manual is trying to say, how would we determine that increasing the concentration of B by the ratio 3.02/1.25 increases the rate by (3.02/1.25)^2? I'm not sure how we would figure this given how we've gone about solving these kind of problems so far. I personally pre...
- Wed Feb 28, 2018 6:54 pm
- Forum: First Order Reactions
- Topic: Terminology "first-order" [ENDORSED]
- Replies: 5
- Views: 681
Terminology "first-order" [ENDORSED]
Do the terms "first-order" and "second-order" only apply to the reaction as a whole and not to the reactants individually? Like if there were two reactants both with coefficients of 1, would we never call the rxn a 2nd-order rxn with two 1st-order reactants?
- Wed Feb 28, 2018 6:47 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: K2K1/K' Formula
- Replies: 3
- Views: 681
Re: K2K1/K' Formula
I think Dr. Lavelle will go into this on Friday, or at least in coming lectures, since we haven't worked on any of it yet.
- Wed Feb 28, 2018 6:07 pm
- Forum: General Rate Laws
- Topic: 15.3 C
- Replies: 8
- Views: 1622
Re: 15.3 C
The solution manual lists instead of an answer for (c), another answer for (b). And it's solution is +3.3 x 10^-3 instead of -3.3 x 10^-3. Is this another error? Or could someone explain to me why this solution would be positive and not negative, if the formula for unique rate would be -1/a ΔA/Δt.
- Thu Feb 22, 2018 2:04 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 14.55
- Replies: 2
- Views: 442
14.55
How come the anode rxn's Eº = +1.23 V and not -1.23 V? In the book the reaction is written O2 + 4H+ + 4e- → 2H2O with Eº = +1.23 V. Since they've switched the reaction here, why isn't it -1.23?
- Thu Feb 22, 2018 1:28 am
- Forum: Balancing Redox Reactions
- Topic: HW #14.3 d
- Replies: 3
- Views: 501
Re: HW #14.3 d
Still two, it's just that Cl is both the reducing and oxidizing agent.
- Thu Feb 22, 2018 1:26 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 14.13 c
- Replies: 1
- Views: 299
14.13 c
Could someone explain why for 14.13 part c Au^+(aq) \rightarrow Au(s) + Au^{3+}(aq) that one of the half-reactions has Au3+ as a reactant and Au(s) as a product when they are both on the same side in the original equation given? I thought the two half reactions would be Au+(a...
- Mon Feb 12, 2018 8:38 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Units for Gibbs Free Energy
- Replies: 3
- Views: 1294
Re: Units for Gibbs Free Energy
Oh, sorry, I actually meant for ΔGº = RTlnK. because then where would the moles cancel out for the R constant?
- Mon Feb 12, 2018 6:28 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Calculating work and internal energy
- Replies: 2
- Views: 302
Re: Calculating work and internal energy
Thank you. Would we have to deduce on our own what kind of work is occurring or would it most likely say in the question what kind of expansion it is?
- Mon Feb 12, 2018 6:24 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Units for Gibbs Free Energy
- Replies: 3
- Views: 1294
Units for Gibbs Free Energy
So when using difference of sums to calculate something such as enthalpy, we multiplied enthalpies of formation by however many moles of each molecule were present in the equation. Like if there were 2 moles of CO _2 , we would enter 2 mol(-394 kJ/mol), and the mol would cancel out, leaving us with ...
- Mon Feb 12, 2018 6:18 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Calculating work and internal energy
- Replies: 2
- Views: 302
Calculating work and internal energy
I'm having trouble determining when to use which equation. Could someone summarize when to use which equation to calculate work and internal energy? I know that for work it can be calculated with w = -PΔV or w = -nRT(V_2/V_1) so in what instances would we use these, i.e. how would we know us...
- Wed Feb 07, 2018 6:32 pm
- Forum: Balancing Redox Reactions
- Topic: Basic vs. Acidic
- Replies: 6
- Views: 621
Re: Basic vs. Acidic
It affects the way you balance the equations. For a reaction in an acidic soln, you would balance the O's in the half-reactions using H2O and then balance the H's using H+ ions. For a reaction in a basic soln, you would balance the O's in the half-reactions using H2O and then, to balance the H's, ad...
- Wed Feb 07, 2018 6:30 pm
- Forum: Balancing Redox Reactions
- Topic: 14.3
- Replies: 3
- Views: 378
Re: 14.3
Yeah, basically it's reversed when it comes to the agents: The oxidizing agent is the species that is being reduced. The reducing agent is the species that is being oxidized.
- Wed Feb 07, 2018 3:44 pm
- Forum: Balancing Redox Reactions
- Topic: 14.1 [ENDORSED]
- Replies: 1
- Views: 229
14.1 [ENDORSED]
For this one, I'm confused how we determine that C was oxidized from -2 to -1? Would we have to draw the Lewis structure of the molecule and calculate formal charge of each atom? I ask because while calculating formal charge of the carbons, I got 0 for both, so how do we know C originally had a char...
- Wed Jan 31, 2018 6:02 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: 9.11
- Replies: 2
- Views: 264
Re: 9.11
You don't need the units atm at all because the atm in the ln part of the equation cancel out. For example ln(4 atm/2 atm) is just ln 2, not ln 2 atm. You want your answer to be in J/K. If you were to use 0.0826 L*atm/K*mol, you would have a leftover L and atm in your answer, and no J.
- Wed Jan 31, 2018 5:45 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: 9.13
- Replies: 2
- Views: 310
9.13
Could someone explain why for this problem we assume n = 1.00 mol? Is it because the problem says to assume this is happening under ideal conditions? And as a role of thumb, what do ideal conditions mean for a reaction?
- Wed Jan 31, 2018 4:38 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.1 [ENDORSED]
- Replies: 3
- Views: 412
9.1 [ENDORSED]
Could someone explain to me why to find change in entropy we would calculate negative q/T as opposed to positive q/T for this problem? I'm also confused because even though the calculation is –(100. J.s^-1)/(293 K), the solutions manual still has a positive number as the solution. Why would it be po...
- Thu Jan 25, 2018 7:59 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.1 Entropy Higher or Lower at Higher Temperatures
- Replies: 2
- Views: 228
Re: 9.1 Entropy Higher or Lower at Higher Temperatures
yes, in this case ΔS would be inversely proportional to T.
- Thu Jan 25, 2018 7:57 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: change in enthalpy
- Replies: 2
- Views: 375
Re: change in enthalpy
for the second part of your question, i believe w = -PΔV when work is done BY the system and w = +PΔV when work is done ON the system.
- Tue Jan 23, 2018 7:32 pm
- Forum: Phase Changes & Related Calculations
- Topic: Phase Changes and Energy
- Replies: 2
- Views: 345
Phase Changes and Energy
Do all phase changes require energy? Or just the "backward" ones like condensation, solidification, etc?
- Wed Jan 17, 2018 5:15 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 8.19 heating water in a copper kettle
- Replies: 3
- Views: 550
8.19 heating water in a copper kettle
For this one, I thought we only had to determine how to heat up the water, but it looks like we need to determine the same for the copper kettle itself. Will we always need to do this whenever it is a question concerning heating up something in a container? For example, would we need to do the same ...
- Wed Jan 17, 2018 5:08 pm
- Forum: Calculating Work of Expansion
- Topic: 8.17 Work done by a system
- Replies: 6
- Views: 702
8.17 Work done by a system
I'm confused about work in general for a couple reasons. Why is it that when a system does work, its work value is negative? Also during condensation, how is it that work is done ON the system rather than by it?
- Wed Jan 17, 2018 4:49 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Standard Temperature
- Replies: 2
- Views: 331
Re: Standard Temperature
I think it's just the standard temperature because that's the temperature of most rooms. Like it's the typical room temperature.
- Thu Jan 11, 2018 5:25 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 8.51
- Replies: 3
- Views: 239
Re: 8.51
The answer is positive because you can't have negative values for density. Like an object like TNT can't be -1 g/mL, just as you can't have negative grams of something.
- Thu Jan 11, 2018 5:21 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Can homework be written in pencil?
- Replies: 6
- Views: 620
Re: Can homework be written in pencil?
I think it depends on your TA! I know tests have to be written in pen.
- Thu Jan 11, 2018 5:20 pm
- Forum: Phase Changes & Related Calculations
- Topic: Intensive vs. Extensive
- Replies: 5
- Views: 2172
Intensive vs. Extensive
Could someone explain the difference between intensive and extensive values/properties? We went over this briefly in my discussion but I was a little lost in how it pertained to our course...
- Tue Dec 05, 2017 7:11 pm
- Forum: Bronsted Acids & Bases
- Topic: 12.25
- Replies: 2
- Views: 437
12.25
Could someone explain why we know for sure that the concentration of OH- will be twice the amount of Ba(OH)2? Like I get that it will be twice an amount because of the coefficient of 2, but why do we assume it's twice the concentration of Ba(OH)2?
- Tue Dec 05, 2017 7:07 pm
- Forum: Bronsted Acids & Bases
- Topic: Chemical equation for dissociation of strong acids
- Replies: 2
- Views: 578
Re: Chemical equation for dissociation of strong acids
i think right now we're allowed to do both, but if it's strong, i would just put the forward one, and if it's weak, do the double arrows.
- Tue Nov 28, 2017 9:25 pm
- Forum: Hybridization
- Topic: Bond Angles [ENDORSED]
- Replies: 4
- Views: 7568
Re: Bond Angles [ENDORSED]
As far as I know, the orbitals being hybridized has no effect on bond angles. For example a tetrahedral with sp3 hybridization still has 109.5 bond angles. I wouldn't think of hybridization as a separate entity from molecular shape. The shape is the same. Hybridization just goes into WHY it is the s...
- Tue Nov 28, 2017 9:24 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Question 17.33(c)
- Replies: 1
- Views: 250
Re: Question 17.33(c)
That would be my guess as to why it's like that, since it has more than one bonding site.
- Tue Nov 21, 2017 7:12 pm
- Forum: Naming
- Topic: Naming and Polyatomic Ions
- Replies: 6
- Views: 1021
Naming and Polyatomic Ions
1) Can we use something like cyano- and cyanido- interchangeably? I've seen both used in the solutions manual.
2) For the test, are we expected to know the charge of various polyatomic ions like sulfate, oxalate, etc.?
2) For the test, are we expected to know the charge of various polyatomic ions like sulfate, oxalate, etc.?
Re: Naming
If the coordination compound has an overall charge like -1 or +1, it would then be an ion. For example, hexacyanoferrate(II) ion is an ionic compound because it has a charge of -4. But a compound like potassium hexacyanidochromate(III) is a neutral compound: three potassiums with a charge of -1 boun...
- Tue Nov 21, 2017 7:08 pm
- Forum: Naming
- Topic: Oxidation Numbers 17.29
- Replies: 2
- Views: 531
Re: Oxidation Numbers 17.29
I think for the ligands we're meant to know what charge they have? I'm not sure if we need to memorize polyatomic ions... And as far as I know I don't know an easier way to compute it :/
- Tue Nov 14, 2017 8:40 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone Pairs and Bond Angle
- Replies: 3
- Views: 498
Re: Lone Pairs and Bond Angle
There's a difference between molecular geometry and electron geometry. Lone pairs are included in electron geometry but not in molecular geometry. For example for something like NH3, the electron geometry is tetrahedral (including the lone pair) and the molecular geometry (how the molecule itself wi...
- Tue Nov 14, 2017 8:36 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Chapter 4 #25
- Replies: 1
- Views: 689
Chapter 4 #25
Could someone explain to me why 1) you wouldn't arrange CH2Cl2 with H's and Cl's opposite to each other and 2) it's a polar molecule? I thought it might be nonpolar if you arrange them symmetrically...
- Tue Nov 07, 2017 5:57 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angle of OCLO
- Replies: 2
- Views: 519
Re: Bond Angle of OCLO
No it's not trigonal planar cuz there's only 2 things bound to the central atom, rather than three. It would be linear.
- Tue Nov 07, 2017 5:51 pm
- Forum: Lewis Structures
- Topic: 3.97
- Replies: 2
- Views: 333
Re: 3.97
I think it's just drawn this way because that's what it says white phosphorous is, four phosphorouses each connected to three others. I wouldn't worry too much about it.
- Thu Nov 02, 2017 2:40 pm
- Forum: Lewis Structures
- Topic: #37 on Chapter 3
- Replies: 2
- Views: 348
#37 on Chapter 3
Could someone explain how to do this problem. Like how would we know which Period 3 element it would be...
- Thu Nov 02, 2017 2:39 pm
- Forum: Ionic & Covalent Bonds
- Topic: #25 on Chapter 3
- Replies: 6
- Views: 992
#25 on Chapter 3
Could someone please explain how to do this problem? I'm confused on how to determine the compound formula when it comes to ions with 2+ and 3- charge, and vice versa.
- Tue Oct 24, 2017 6:45 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Sequen of Orbitals
- Replies: 4
- Views: 545
Re: Sequen of Orbitals
If this is true then why, for elements like tungsten, would it be 4f14 5d4 6s2 instead of 4f14 5s2 5p6 5d4 6s2?
- Tue Oct 24, 2017 6:41 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: HW Question 2.43
- Replies: 4
- Views: 616
HW Question 2.43
For anyone who has done question #2.43 on the homework: Why would tungsten's configuration be [Xe]4f^14 5d^4 6s^2 instead of [Xe]4f^14 5s^2 5p^6 5p^5 5d^4 6s^2?
- Tue Oct 17, 2017 7:12 pm
- Forum: DeBroglie Equation
- Topic: 1.39 Help
- Replies: 5
- Views: 655
1.39 Help
Could someone help me with 1.39? My units don't cancel out properly. I thought J = kg * m^2 * / s^2? But in my equation I have one kg on top, two meters, and only one second. This is what I entered:
wavelength = (6.626 x 10^-34 kg • m^2 • s^-2) / (0.15 kg)(41 m)
wavelength = (6.626 x 10^-34 kg • m^2 • s^-2) / (0.15 kg)(41 m)
- Tue Oct 17, 2017 7:07 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect as Proof of Particle Qualities of Light
- Replies: 3
- Views: 756
Photoelectric Effect as Proof of Particle Qualities of Light
I get that the photoelectric effect proves light is a particle, but how exactly does it prove that? Like how does it prove that it is a particle?
- Wed Oct 11, 2017 7:45 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect: Post Module Assessment Q. 28, 29, and 30
- Replies: 12
- Views: 1454
Re: Photoelectric Effect: Post Module Assessment Q. 28, 29, and 30
will we be given the mass of an e- and planck's constant in a problem or will we have to know them by heart?
- Wed Oct 11, 2017 6:55 pm
- Forum: Photoelectric Effect
- Topic: Units Cancelling Out
- Replies: 3
- Views: 998
Units Cancelling Out
Could someone explain to me how units cancel out in equations like E = hv and E = 1/2mv^2? Do I even need to worry about it?
- Wed Oct 11, 2017 5:57 pm
- Forum: Limiting Reactant Calculations
- Topic: Theoretical Yield [ENDORSED]
- Replies: 6
- Views: 768
Re: Theoretical Yield [ENDORSED]
We've basically been calculating theoretical yields rather than actual yields this whole time, so we would only know the actual yield if it were given to us in the problem. And then you would take the actual yield that is given and divide that over the theoretical yield calculated times 100 to find...
- Sat Oct 07, 2017 10:32 am
- Forum: Limiting Reactant Calculations
- Topic: Theoretical Yield [ENDORSED]
- Replies: 6
- Views: 768
Re: Theoretical Yield [ENDORSED]
We've basically been calculating theoretical yields rather than actual yields this whole time, so we would only know the actual yield if it were given to us in the problem.
- Sat Oct 07, 2017 10:30 am
- Forum: Balancing Chemical Reactions
- Topic: Net Moles Produced [ENDORSED]
- Replies: 5
- Views: 906
Re: Net Moles Produced [ENDORSED]
Add the coefficients of the reactants together and then subtract the sum of the coefficients of the products from that. For example, if the reaction were 2K + 10W --> 5L + 4R, then the net moles produced would be 12 - 9 = 3 net moles.