Search found 70 matches
- Sun Mar 17, 2019 3:57 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equlibrium and catalysts
- Replies: 2
- Views: 506
Re: Equlibrium and catalysts
I believe it just speeds up the overall reaction, both forward and backwards. If this is the case then the amount of reactants and products being formed shouldn't change.
- Thu Mar 14, 2019 10:16 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Standard cell potential and equilibrium
- Replies: 3
- Views: 358
Re: Standard cell potential and equilibrium
Positive standard cell potential correlates to K>1 because of the equation Delta G=-nFE. This shows that whenever E is positive, Delta G will be negative (moles are never negative and F is a positive constant). When Delta G is negative this means the reaction will be spontaneous and will favor produ...
- Thu Mar 14, 2019 9:46 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Bronsted Neutralization Reaction
- Replies: 1
- Views: 243
Re: Bronsted Neutralization Reaction
I did the same exact thing and got the same answer. I think as long as everything cancels out correctly it should be the same. On the test there will only be a certain number of reactions to choose from as well so I think it will be more clear which reactions we are supposed to use.
- Mon Mar 11, 2019 6:14 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Slow vs Fast Step
- Replies: 4
- Views: 441
Slow vs Fast Step
How do you tell which step in a multistep reaction is the slow step? Would we be given this information or is there a way to tell by the step itself? I am having trouble figuring out which step is the rate limiting step.
- Mon Mar 11, 2019 9:16 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Test 2 Question
- Replies: 1
- Views: 296
Test 2 Question
Hello, it has been a while since we took test two but I am still really confused about one of the problems. I am sure it varied slightly for other people but a brief outline of how to do this problem would be really helpful. The question was.... 5. The ionic dissociation of water us given by the fol...
- Mon Mar 11, 2019 9:11 am
- Forum: Administrative Questions and Class Announcements
- Topic: Homework week 9
- Replies: 3
- Views: 476
Re: Homework week 9
This is our last out of ten. We don't need to turn in an extra 7 because finals week doesn't technically count towards the quarter.
- Mon Mar 11, 2019 9:09 am
- Forum: Zero Order Reactions
- Topic: Graphs
- Replies: 6
- Views: 871
Re: Graphs
It is probably a good idea to know what these look like just because that knowledge could potentially help you figure out which order a reaction is. It is a useful way to test the order of a reaction.
- Tue Mar 05, 2019 12:40 pm
- Forum: General Rate Laws
- Topic: Table with different Concentration
- Replies: 4
- Views: 450
Re: Table with different Concentration
I would say so. My TA went over a past exam question today which asked for the rate law given a table of reactants and concentrations. It would be a good idea to study this sort of thing as the concept will surely come up even if it's not in that specific form.
- Tue Mar 05, 2019 12:36 pm
- Forum: General Rate Laws
- Topic: Orders
- Replies: 3
- Views: 372
Re: Orders
The order is generally the sum of the exponents of each concentration contributing to the rate law. This information not only helps you calculate the rate law, it gives you a clearer understanding about the mixture and which concentrations effect the rate of the reaction the most.
- Sun Mar 03, 2019 3:31 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Large K value
- Replies: 5
- Views: 587
Re: Large K value
The double >> just means that it is very favorable, it is just a way to express that it is strongly favored.
- Mon Feb 25, 2019 7:55 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Gibbs free energy at equilibrium
- Replies: 2
- Views: 275
Re: Gibbs free energy at equilibrium
Delta G is 0 at equilibrium because the forward and the backward reactions are equivalent which would mean they cancel each other out.
- Mon Feb 25, 2019 11:54 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: trends in standard potential
- Replies: 2
- Views: 335
Re: trends in standard potential
I was wondering the same thing, there doesn't seem to be an actual trend that you can just look at or infer. I think you may actually just need the values to evaluate them.
- Sun Feb 24, 2019 8:19 pm
- Forum: Balancing Redox Reactions
- Topic: Including H2O, H+, and OH- in balanced redox reactions
- Replies: 2
- Views: 293
Re: Including H2O, H+, and OH- in balanced redox reactions
No just like how you add and subtract the electrons that you include in the half reactions you can cancel out H20 in that situation as well.
- Sun Feb 24, 2019 8:18 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Predicting Standard Potential of Cells
- Replies: 3
- Views: 789
Re: Predicting Standard Potential of Cells
Is the reverse given? I couldn't find the values anywhere, I wasn't sure if you are maybe supposed to derive them from the ones that are given? I am not sure how to go about that though.
- Sun Feb 24, 2019 5:10 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Predicting Standard Potential of Cells
- Replies: 3
- Views: 789
Predicting Standard Potential of Cells
So in the 7th edition in section 6M there are several questions including 6M.3. which ask you to predict the standard potential of different galvanic cells. In the book there is a tabel containing many of the E/V values which you use plug into the formula Ecell=E(cathode)-E(anode) but in some cases ...
- Sun Feb 24, 2019 3:49 pm
- Forum: Balancing Redox Reactions
- Topic: Oxidizing and Reducing Agents
- Replies: 2
- Views: 870
Re: Oxidizing and Reducing Agents
Yes they will be as long as it is a forward reaction because nothing would be reduced or oxidized before a reaction even happens. The oxidizing agent would become the reduced product and the reducing agent would become the oxidized product.
- Sun Feb 24, 2019 3:47 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagram
- Replies: 1
- Views: 191
Cell Diagram
When constructing your cell diagram I know that the anode portion goes on the left of the salt bridge and the cathode goes on the right but within those limits does the order of the species matter? For example if the anode half reaction is H2(g) --> 2H+(aq) + 2e- would it matter when you are drawing...
- Mon Feb 18, 2019 5:12 pm
- Forum: Administrative Questions and Class Announcements
- Topic: 14BL and 14C
- Replies: 5
- Views: 1047
14BL and 14C
Hello, I am trying to plan my classes for next quarter and as of right now I am planning on taking Math 3C and Chem 14C for sure. For the sake of units I need to take a GE as well and I was thinking of maybe taking 14BL also. I know 14BL is only worth three units but does anyone know how time consum...
- Wed Feb 13, 2019 1:13 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Homework
- Replies: 1
- Views: 244
Re: Homework
Yes we still have homework due regardless of the midterm.
- Wed Feb 13, 2019 12:56 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Question 4F.11.
- Replies: 2
- Views: 447
Question 4F.11.
" During the test of an internal combustion engine, 3.00L of nitrogen gas at 18.5 degrees C was compressed suddenly (and irreversibly) to .500L by driving in a piston. In the process the temperature of the gas increased to 28.1 degrees C. Assume ideal behavior and 1.00 mole of nitrogen gas. Wha...
- Mon Feb 11, 2019 11:52 pm
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Assume Ideal Behavior
- Replies: 3
- Views: 1040
Assume Ideal Behavior
I noticed that a couple problems in the book ask you to "assume ideal behavior". After looking at the solutions manual it looks like this means assume there is 1 mole of the given substance? I am not familiar with this phrase and I am hoping someone can maybe shed some light on the subject.
- Sun Feb 10, 2019 8:11 pm
- Forum: Calculating Work of Expansion
- Topic: Work sign convention
- Replies: 3
- Views: 380
Re: Work sign convention
When work is done by the system the value you are going to get will be negative and when work is done on the system the value you will get will be positive. You shouldn't really have to worry about whether or not to put a negative because the determining sign will be a part of your equation you use....
- Sun Feb 10, 2019 8:06 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: calculation of change in entropy
- Replies: 3
- Views: 414
Re: calculation of change in entropy
Although the both of these seem to be changing at the same time we treat them as though they happen separately. So when calculating volume you act as though your temperature is a constant and when you calculate the temperature you do the same thing. We can take the entropies separately and then add ...
- Sat Feb 09, 2019 8:24 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: When n is not given
- Replies: 3
- Views: 385
Re: When n is not given
If you are referring to the q=nCm(Delta T) then usually it will give you specific heat or another value for C that you can plug into the equation q=C(Delta T) or q=mCs(Delta T) if it does not give you the moles.
- Sun Feb 03, 2019 2:12 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Expansion Work and Nonexpansion Work
- Replies: 2
- Views: 294
Re: Expansion Work and Nonexpansion Work
Expansion work is work dealing with pressure-volume while non expansion work is pretty much everything else. I believe Gibbs helps you find the maximum amount of non expansion work that can potentially be done, but I am not sure how this relates to reversibility so hopefully someone else can answer ...
- Sun Feb 03, 2019 2:02 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy of Complicated Molecule
- Replies: 1
- Views: 216
Enthalpy of Complicated Molecule
How do we find the enthalpy for a complicated molecule? I know some of them are listed in the book but are we expected to figure out complicated enthalpies during a test or will those generally be given?
- Wed Jan 30, 2019 5:39 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Thermo Test/Midterm
- Replies: 9
- Views: 786
Re: Thermo Test/Midterm
I am pretty sure that we don't get the lewis structure because my TA broke the process of calculating this down in steps and one of the first steps was to draw out the lewis structures to make sure that we account for all of the bonds.
- Sun Jan 27, 2019 12:38 pm
- Forum: Phase Changes & Related Calculations
- Topic: closed vs isolated system
- Replies: 3
- Views: 801
Re: closed vs isolated system
In both of these the number of particles is fixed and there is no exchange with outside systems in either of them. I am pretty sure the only difference is that a closed system can have a fluctuation in energy but the isolated system cannot. Could anyone explain why? I am still confused how that is a...
- Sun Jan 27, 2019 12:33 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 3 Methods
- Replies: 3
- Views: 363
Re: 3 Methods
Just as with any other problem it is good to have more than one way to solve it. That being said, the information you are given will dictate which one of the three options you can or cannot use. For example if you are only given the total Delta H of the reactions you would have to use the first meth...
- Sun Jan 27, 2019 12:22 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Accuracy of Enthalpy Calculation
- Replies: 3
- Views: 473
Accuracy of Enthalpy Calculation
In my notes from lecture on January 25th I wrote that bond enthalpies of diatomic molecules are accurate but other bond enthalpies are not as accurate and I was wondering why? I didn't write an explanation so I was struggling to make sense of what this means.
- Sat Jan 19, 2019 9:22 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: X Value
- Replies: 3
- Views: 360
Re: X Value
I believe this rule is actually anything below 10 to the -3 not -5 so if you had a number to the -4 you should be alright to leave it out. I am not 100% sure that is correct but the 5% rule at the end will always let you know if it was okay to round it a bit.
- Sat Jan 19, 2019 5:36 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Delta H
- Replies: 2
- Views: 1450
Delta H
During the last bit of class we talked about exo- and endothermic reactions and how this is determined by delta H. What is delta H and if it is positive does that mean it is always going to endothermic and favor the products when heat is added? If it is negative does it always mean it is exothermic ...
- Sat Jan 19, 2019 5:29 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Pressure
- Replies: 4
- Views: 560
Pressure
Would the products or the reactants be favored when volume of a system is compressed if there was an equal number of moles on both sides? What else would determine which is favored if not the number of moles?
- Fri Jan 11, 2019 11:43 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Solids and Liquids in K Expression
- Replies: 2
- Views: 220
Re: Solids and Liquids in K Expression
Thank you that is actually very helpful!
- Fri Jan 11, 2019 11:42 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE Tables
- Replies: 1
- Views: 198
ICE Tables
In class the example we did for ice tables involved the equation H2o + ATP = ADP +P. When finding the solutions we found that the change in molarity for ATP was about -8.435 so in turn we added 8.435 to both ADP and P. Do we add the same amount to both because there is a 1-1 ratio between them or wo...
- Fri Jan 11, 2019 11:32 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Charles’s Law
- Replies: 4
- Views: 224
Re: Charles’s Law
I am not sure I can explain as in depth as you are looking for, but I believe Charle's law describes how gasses expand when they are heated up. Basically the experiment showed that when pressure is constant, the volume of the gas will be directly proportional to the temperature of the gas (in Kelvin).
- Fri Jan 11, 2019 11:21 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Solids and Liquids in K Expression
- Replies: 2
- Views: 220
Solids and Liquids in K Expression
So if you have a chemical equation that you want to find the equilibrium constant for, you do not include solids or liquids at all? I understand that this means that you do not include them in the K equation but if they are a part of the reaction shouldn't they affect the equilibrium? I am just a li...
- Sat Dec 08, 2018 5:16 pm
- Forum: *Making Buffers & Calculating Buffer pH (Henderson-Hasselbalch Equation)
- Topic: Final Exam
- Replies: 8
- Views: 2412
Final Exam
Just to be clear we only need to conceptually understand Ka and Kp values and equilibrium constants but we do not actually have to solve for this or use these factors for anything except determining which acid or base is stronger?
- Thu Dec 06, 2018 8:25 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: pH calculation
- Replies: 4
- Views: 569
Re: pH calculation
Usually this value is given to you as the molarity of the solution or you are given moles and volume of a certain solution and you have to find the molarity by dividing moles of solute by liters of solution to find the molarity to in turn plug into the pH equation.
- Thu Dec 06, 2018 8:18 pm
- Forum: Octet Exceptions
- Topic: Sulfur
- Replies: 3
- Views: 664
Re: Sulfur
If you draw the lewis structure for (SO4)2- with only single bonds it would not have an expanded octet but in order to draw the lewis structure with the least amount of formal charges you have to draw the lewis structure with two single bonds and two double bonds so that only two Oxygens have negati...
- Thu Dec 06, 2018 8:08 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Relative Acidity
- Replies: 1
- Views: 260
Re: Relative Acidity
Those rules are only applicable in certain situations. When you have the case where you're looking at two acids that they all have the same configurations such as ClOH, BrOH, and IOH you can't look at the atomic radius because the hydrogens are not directly attached to the differing atoms. In this c...
- Wed Dec 05, 2018 7:51 pm
- Forum: Lewis Acids & Bases
- Topic: Identifying Lewis Acids and Bases
- Replies: 3
- Views: 1173
Re: Identifying Lewis Acids and Bases
I don't fully understand why SO3 is the base but when I draw the lewis structure you can see that there is resonance in its structure and in order to fill the octet rule the Sulfur in the center has to make one double bond. When you draw the lewis structure for H2O2 it is nicely balanced, it is non-...
- Tue Dec 04, 2018 5:08 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: polydentate
- Replies: 2
- Views: 212
Re: polydentate
A ligand is polydentate if it has more than one place where it is binding to a central metal atom. An example of this would be EDTA, which binds to a metal in six different places, also known as a hexadentate ligand.
- Sun Dec 02, 2018 2:03 pm
- Forum: Bronsted Acids & Bases
- Topic: Chelating Ligands
- Replies: 1
- Views: 172
Chelating Ligands
I know that ligands are molecules that bind to a central atom but I am a little confused on what the difference is between a regular ligand and a chelating ligand. Also can ligands ever have double or triple bonds or are they strictly single? I have only seen single bonds so I was curious if they wo...
- Sun Dec 02, 2018 1:55 pm
- Forum: Bronsted Acids & Bases
- Topic: Water with Acids and Bases
- Replies: 3
- Views: 395
Water with Acids and Bases
So i know several elements can act as both an acid and a base such as water but how do you tell when a water should act as an acid or a base. When do you know when it should give up or accept electrons? Also does water affect the likelihood of certain compounds being stronger or weaker acids or bases?
- Sun Dec 02, 2018 1:48 pm
- Forum: Lewis Acids & Bases
- Topic: Weak Acid/Base vs. Strong
- Replies: 7
- Views: 900
Re: Weak Acid/Base vs. Strong
If it does completely dissociate in water how do you actually tell when this happens? Is there a way to tell how much it will dissociate?
- Mon Nov 26, 2018 11:28 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Lone PR and Bonding PR
- Replies: 2
- Views: 247
Re: Lone PR and Bonding PR
I believe we are just supposed to know the different trends that occur as more and more lone pairs are presented on certain types of molecules. This would include the two you have listed above as well as linear, see saw, trigonal bi-pyramidal, t-shaped, among others as the molecules get bigger and b...
- Mon Nov 26, 2018 11:23 pm
- Forum: Dipole Moments
- Topic: Intermolecular Forces
- Replies: 1
- Views: 264
Re: Intermolecular Forces
While Fluorine is a very electronegative atoms, this electronegativity creates very strong Intramolecular bonds which make the molecule itself very hard to break apart. When you are talking about boiling point however the bonds between molecules, or the intermolecular bonds, are what you actually ne...
- Mon Nov 26, 2018 11:13 pm
- Forum: Lewis Acids & Bases
- Topic: Difference Between Acids and Bases
- Replies: 4
- Views: 500
Difference Between Acids and Bases
When you are trying to decide wether a molecule is an acid or a base is there more ways to determine this other than if the molecule donates or accepts electrons? I know there are some other indicators but what are they and are they as accurate as looking at whether they receive or donate electrons?
- Thu Nov 15, 2018 4:12 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: 109.5 Degrees
- Replies: 4
- Views: 3248
Re: 109.5 Degrees
Bent molecules actually do not have a bond angle of 109.5 degrees because the lone pairs are more electronegative and push the other atoms more closely together. This would cause the bond angle of a bent molecule to be less than 109.5, the exact value i believe was 104.5 degrees. I think the only mo...
- Thu Nov 15, 2018 4:07 pm
- Forum: Dipole Moments
- Topic: Dipoles
- Replies: 2
- Views: 176
Dipoles
I am a little bit confused about what a dipole actually is. When we were talking about interactions in lecture and ion-ion, ion-dipole, and dipole-dipole reactions were brought up how do you determine whether something is a dipole or not?
- Thu Nov 15, 2018 3:42 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Planar vs Pyramidal
- Replies: 3
- Views: 1443
Re: Planar vs Pyramidal
So when considering the shape of a molecule it helps to first look at how many electrons are going to be connected to the central atom. The difference between a trigonal planar and a trigonal pyramidal is the planar has a total of three things connected to the central atom while the pyramidal has fo...
- Sun Nov 11, 2018 11:10 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Bond Angles
- Replies: 4
- Views: 933
Re: Bond Angles
In that instance you would have to consider a 3D model instead of a 2D model. The surrounding atoms want to be as far away from each other as possible so a three dimensional model provides the most space between the atoms.
- Thu Nov 08, 2018 12:39 pm
- Forum: Lewis Structures
- Topic: Exceptions to the octet rule
- Replies: 3
- Views: 463
Re: Exceptions to the octet rule
Group 13 elements only have three electrons available to make bonds. They can only accept three more because once they have six there are no more electrons available to bond with.
- Sun Nov 04, 2018 7:46 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: How to write P and D Orbitals
- Replies: 1
- Views: 378
How to write P and D Orbitals
So when you're writing out the electron configuration for an element such as Bromine would you write this as 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{5} or would you switch the 3d^{10} and 4s^{2} orbitals. I am not sure when to write the d orbital before the s or if I should always writ...
- Fri Nov 02, 2018 2:03 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Exceptions to the Octet Rule
- Replies: 2
- Views: 258
Exceptions to the Octet Rule
So i know that sometimes you can have ten electrons in the valence shell by using the d orbital but is there ever a time when you have even more in the valence shell? Do you ever use the f orbital to accommodate more electrons?
- Fri Nov 02, 2018 1:47 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Diamagnetic/Paramagnetic
- Replies: 1
- Views: 244
Re: Diamagnetic/Paramagnetic
On the class website there are lists of everything you need to know for each subject. The midterm covers "Review of Chemical & Physical Principles", "The Quantum World", and part of "Chemical Bonds" and I don't believe those topics are listed under these subjects. T...
- Fri Nov 02, 2018 1:38 pm
- Forum: Coordinate Covalent Bonds
- Topic: Electronegativity
- Replies: 12
- Views: 1744
Electronegativity
I know that electronegativity is the tendency an atom has to attract a bonding pair of electrons to itself but how do we find the electronegativity of an atom? Why is Fluorine higher than the other halogen elements? I am just a little confused on how the electronegativity trend works and why it decr...
- Fri Oct 26, 2018 5:47 pm
- Forum: Ionic & Covalent Bonds
- Topic: Valence Electrons
- Replies: 3
- Views: 346
Valence Electrons
How do elements actually keep their shape and the same number of electrons as they bond and detach from other elements. Is it just the magnetic pull that keep them together? Once they lose or gain electrons how do they regain or get rid of them after?
- Fri Oct 26, 2018 2:27 pm
- Forum: Ionic & Covalent Bonds
- Topic: Bonding Between Cations and Anions
- Replies: 3
- Views: 265
Bonding Between Cations and Anions
When you have an example like the one that professor went over during lecture with 2 cations and 1 anion where do they bond together if they all have full valence shells? I believe the example was ammonium sulfate (NH4)2+ (SO4)2-
- Fri Oct 26, 2018 2:22 pm
- Forum: Ionic & Covalent Bonds
- Topic: Ground State Electron Configurations
- Replies: 7
- Views: 685
Re: Ground State Electron Configurations
Argon and copper both share the exact same beginning of their electron configurations. By putting argon before the rest of the configuration it just makes it shorter to write out. These short cuts make it so that the elements with longer configurations are more easily written.
- Fri Oct 19, 2018 2:39 pm
- Forum: Properties of Light
- Topic: Equations
- Replies: 7
- Views: 552
Re: Equations
We went over this a little bit in our discussion week so hopefully this will help. 1)Energy of a photon: E=hv and c=v(lambda) -These are commonly used in questions concerning the photoelectric effect.These are used for photons only. 2) De Broglie's Equation: lambda=h/p(momentum) -Although this also ...
- Fri Oct 19, 2018 2:06 pm
- Forum: Photoelectric Effect
- Topic: Test 2
- Replies: 16
- Views: 1176
Test 2
Is test 2 on only the the quantum world section or will there be questions on the previous section as well?
- Tue Oct 16, 2018 11:07 pm
- Forum: *Black Body Radiation
- Topic: Stefan-Boltzmann law and Wien's law
- Replies: 2
- Views: 624
Re: Stefan-Boltzmann law and Wien's law
On Lavelle's website under "Lecture Outlines" he has a list of everything you need to know for each subject. Neither one of those subjects are on there so you won't need to know them for the chapter two test.
- Thu Oct 11, 2018 4:44 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: En=-hR/n^2
- Replies: 3
- Views: 230
Re: En=-hR/n^2
I believe the reason that this equation is negative is because all free electrons (when they are not near something) have a value of zero joules and because bound electrons have a lower energy then free electrons the bound electrons have to be less than zero (or negative).
- Thu Oct 11, 2018 4:36 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect
- Replies: 1
- Views: 245
Photoelectric Effect
In any problem where you were using the equation E=1/2(MV2) how would you find M? Is there any way you could find the mass of the actual electrons themselves if you are given what time of element it is from? Does it just have to be given in order for you to use this equation?
- Thu Oct 11, 2018 4:06 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect
- Replies: 2
- Views: 191
Photoelectric Effect
I am taking the post-module test for the photoelectric effect module and I am having trouble with number 28. So the information given is the velocity and the work and the work function. Because it is asking for the Kinetic Energy I assume you would need to use the formula E=1/2(MV2) but I am not sur...
- Tue Oct 02, 2018 6:45 pm
- Forum: General Science Questions
- Topic: Limiting Reactant Calculations
- Replies: 2
- Views: 875
Limiting Reactant Calculations
21. According to the following equation, 0.750 g of C6H9Cl3 is mixed with 1.000 kg of AgNO3 in a flask of water. A white solid, AgCl, completely precipitates out. What is the mass of AgCl produced? C6H9Cl3 + 3AgNO3 ---> AgCl + C6H9(NO3)3. Molar Mass: C6H9Cl3 (187.50 g/mol), 3AgNO3 (169.88 g/mol), Ag...
- Tue Oct 02, 2018 6:17 pm
- Forum: Empirical & Molecular Formulas
- Topic: Formula Mass and Molar Mass
- Replies: 2
- Views: 5273
Re: Formula Mass and Molar Mass
The difference between molar mass and formula mass is that formula mass is the sum of all the atomic weights of the atoms in its empirical formula while molar mass is just the mass of 1 mol of a substance. Molar mass also uses the units g/mol while formula mass uses atomic mass units (amu).
- Tue Oct 02, 2018 6:01 pm
- Forum: Student Social/Study Group
- Topic: Any necessary data booklets?
- Replies: 2
- Views: 345
Re: Any necessary data booklets?
I believe the only necessary materials for this course are the "Chemical Principles The Quest for Insight" (7th edition) textbook and the Student Solutions Manual that accompanies it. The textbook has a periodic table of elements on the first page and the formulas can all be found in the b...