Search found 63 matches
- Tue Feb 14, 2017 2:49 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 2014 Midterm #7
- Replies: 2
- Views: 330
Re: 2014 Midterm #7
Cell structures are written anode on the left and cathode on the right. Since H+ is part of the cathode half reaction, it is written on the right.
- Tue Feb 14, 2017 2:44 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Midterm 2012 Question 3A
- Replies: 1
- Views: 333
Re: Midterm 2012 Question 3A
Draw out the lewis structure of the molecule and see what places the attached atoms can fall into. Its like trading places: the maximum number of positions available for the connected elements to go to. Draw out the molecule and see for yourself.
- Tue Feb 14, 2017 2:41 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Nernst equation
- Replies: 1
- Views: 353
Re: Nernst equation
The two equations are the same. The only reason the log equation exists is because it becomes easier to transcribe your answer to ph, since ph is on a log scale. You can use both formulas for ln and log. Your choice.
- Tue Feb 14, 2017 2:39 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Nernst Equation
- Replies: 1
- Views: 297
Re: Nernst Equation
I believe they are only for aqueous solutions for both galvanic and electrolytic cells
- Tue Feb 14, 2017 2:25 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Winter 2014 Q3B
- Replies: 1
- Views: 306
Re: Winter 2014 Q3B
For the part of your question asking why you don't use 2500K to find you specific heat capacity, since you would only use temperature to find the thermal energy needed to break the shell in part A. For part B, you could use the mcAT method to find the specific heat capacity by doing (thermal energy ...
- Tue Feb 14, 2017 2:17 pm
- Forum: Balancing Redox Reactions
- Topic: Redox
- Replies: 4
- Views: 550
Re: Redox
If you have an acid/base reaction, one of your half reactions will probably be a simple, one element to one element +electron reaction, while another will involve compounds. For the more complicated compound, just write the half reaction with H+ and H20 added to it looking at the main reaction.
- Wed Feb 08, 2017 12:00 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 2007 Midterm Question 7
- Replies: 1
- Views: 245
Re: 2007 Midterm Question 7
I have a step by step attempt at the problem posted as an attachment.
Hope that helps!
Hope that helps!
- Mon Jan 30, 2017 9:46 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Expansion against a vacuum
- Replies: 1
- Views: 288
Re: Expansion against a vacuum
I believe that both Free expansion, or expansion against a vacuum, do not do work. The system must be applying a force over a distance on something to be doing work.
- Mon Jan 30, 2017 9:45 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Quiz 1 Question 11
- Replies: 1
- Views: 311
Re: Quiz 1 Question 11
1) Find what the delta H would be when you have 49.7 g of PbO? -Basically, find the number of moles and multiply that by the delta H to get a new delta H 2) Use the formula q=mCdeltaT to figure out the mass needed. In the workbook, you will only need to go up to 100 degrees, and since there was no i...
- Sat Jan 28, 2017 5:38 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Derivations
- Replies: 1
- Views: 273
Re: Derivations
You will not have to know any derivations for the quiz. Dr. Lavelle goes over the derivation to give students better understanding on how the final formula is obtained and how individual elements of the derivations affect the final formula.
- Sat Jan 28, 2017 5:37 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Chapter 9 Q43
- Replies: 1
- Views: 297
Re: Chapter 9 Q43
The system can't be doing any work if you want to calculate free energy just using q. If a system is kept at constant volume, it can't do any work. That way, delta U =q.
- Sat Jan 28, 2017 5:35 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Entropy and Structure
- Replies: 1
- Views: 268
Re: Entropy and Structure
Sure. The more complex a structure is, the more entropy it will have. With entropy we can have an idea of what kind of orientation a substance can be.
- Sat Jan 28, 2017 5:34 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Residual Entropy 3rd Law of Thermodynamics
- Replies: 4
- Views: 755
Re: Residual Entropy 3rd Law of Thermodynamics
There will always be some small amount of residual entropy, but as the system approaches 0K, the residual entropy will approach 0, but will never actually reach 0. Reaching 0K is currently physically impossible.
- Sat Jan 28, 2017 5:30 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: free energy (G) of a gas at pressure P
- Replies: 1
- Views: 258
Re: free energy (G) of a gas at pressure P
Standard Pressure is 1 atm, so anything under standard pressure will be itself
- Sat Jan 28, 2017 5:29 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Standard Gibbs Free Energy Calculation Discrepancies?
- Replies: 1
- Views: 291
Re: Standard Gibbs Free Energy Calculation Discrepancies?
Note that delta H and delta S for standard delta G should be standard as well. Both methods should be viable. A question will most likely give you information to do one method over the other.
- Sat Jan 28, 2017 5:26 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Question on Calculating Entropy of Vaporization
- Replies: 1
- Views: 376
Re: Question on Calculating Entropy of Vaporization
There are different R values depending on the units. Double check what kind of R you are using.
- Sat Jan 28, 2017 5:24 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Homework 9.51
- Replies: 1
- Views: 282
Re: Homework 9.51
The Delta S should be for whatever you are calculating delta G in. So if delta G is for the system, delta S would need to be for the system. The same applies for the surroundings. Entropy tends to be a chain reaction. If one reaction is spontaneous, the creation of entropy in the surroundings can cr...
- Sat Jan 28, 2017 5:14 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: About pade 31 of course reader
- Replies: 1
- Views: 332
Re: About pade 31 of course reader
Delta S=q/T only if q is reversible. An adiabatic system does not necessarily have to be reversible, so you wouldn't use that delta S formula in that situation. You might want to use other formulas like delta S=nRlnV2/V1 for example
- Sat Jan 28, 2017 5:11 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Clarification on Quiz 1 Prep - Question 2
- Replies: 2
- Views: 337
Re: Clarification on Quiz 1 Prep - Question 2
The answer should be delta U= 0. Conceptually, if I put 5 kj of energy in a bank, and I didn't touch it for 100 years, I will still have 5 kj of energy in the bank. Since there is no change in energy, then delta U=0
- Sat Jan 28, 2017 5:09 pm
- Forum: Calculating Work of Expansion
- Topic: Homework 8.1
- Replies: 1
- Views: 361
Re: Homework 8.1
Please note that L*atm is NOT joules. 1 L*atm is 101.33 Joules. You want to convert Volume to liters and keep pressure at atm to get your work in units of L*atm. Then you can convert L*atm into Joules
- Sat Jan 28, 2017 5:07 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy Change Relating to Temperature
- Replies: 1
- Views: 330
Re: Entropy Change Relating to Temperature
Entropy is less at smaller temperatures, because the more heat you give to a gas, for example, the more excited and random the atoms become. Think about it like heating popcorn. At low temperatures, you are pretty sure where the popcorn kernels will be. But at higher temperatures, when the popcorn p...
- Tue Jan 24, 2017 2:33 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Formulas to know
- Replies: 3
- Views: 734
Re: Formulas to know
I would highly recommend going to any one of the office hours available. The UAs and the TAs do a great job in reviewing all the essential formulas and material you need to know.
- Tue Jan 24, 2017 2:31 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Degeneracy
- Replies: 1
- Views: 323
Re: Degeneracy
You might conceptually need to understand degeneracy in understanding entropy, but I believe that it is not a big picture topic and will probably not be asked.
- Tue Jan 24, 2017 7:10 am
- Forum: Calculating Work of Expansion
- Topic: Irreversible process
- Replies: 2
- Views: 446
Re: Irreversible process
When something diffuses from high concentration to low concentration, it is not doing work. For example, if it were to push on a piston during diffusion and move it, it would be doing work. Diffusion is an irreversible process. You can go from high to low concentrations but not low to high without t...
- Sat Jan 21, 2017 7:44 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Quiz and Examination Schedule
- Replies: 2
- Views: 344
Re: Quiz and Examination Schedule
You can check on Dr. Lavelle's website and if, you have the course reader, it should be there. First quiz will be week 4 in your discussion section. Midterm is Wednesday Feb 15 from 6 to 8pm. This info is on page 8 of the course reader.
- Fri Jan 20, 2017 7:17 am
- Forum: Calculating Work of Expansion
- Topic: Multi step problems [ENDORSED]
- Replies: 1
- Views: 439
Re: Multi step problems [ENDORSED]
You need to use two formulas 1. q=mC(delta)T (m=mass, C=heat capacity, T=Temp) 2. q=mL (m=mass, L=latent heat) a) You should go in increments and every time you jump temperatures you should calculate q=mC(delta)T b) If that increment also includes a phase change (solid-liquid, or liquid-gas) you nee...
- Fri Jan 20, 2017 7:13 am
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: When to use what equation? [ENDORSED]
- Replies: 1
- Views: 321
Re: When to use what equation? [ENDORSED]
Write down all the "givens" you have on one side and try and determine what formula to use with that information. Other than that I think its just a matter of memorizing formulas and practice to increase familiarity of what formula goes where.
- Fri Jan 20, 2017 7:10 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Compression and Work, Heat [ENDORSED]
- Replies: 1
- Views: 305
Re: Compression and Work, Heat [ENDORSED]
Compression means work is being done on the system. Since the system is not exerting energy to do work and is getting free work, the value for work is positive. In the formula U=q+w, w is positive. If q is constant, you can say that the system gains energy. Work is affected by compression.
- Fri Jan 20, 2017 7:03 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Work is not a state function [ENDORSED]
- Replies: 3
- Views: 1542
Re: Work is not a state function [ENDORSED]
A state function can be defined by a start and end point. Work is quantified based on the pathways you take. For example, if two people exert a force over a certain distance to the same destination, but take different paths with varying distances, the path matters. So you can't quantify work with on...
- Wed Jan 18, 2017 6:53 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Problem 8.19
- Replies: 2
- Views: 410
Re: Problem 8.19
Yes, for these types of problems, you have to assume that the temperature change is the same for both.
- Tue Jan 17, 2017 9:00 am
- Forum: Phase Changes & Related Calculations
- Topic: Enthalpy
- Replies: 1
- Views: 250
Re: Enthalpy
Based on the question, it should be clear which methods for solving Enthalpy you should use. For example, uses hess's law will be based on the question and whether or not you use enthalpy of formation or bond enthalpy will also be dependent on the problem.
- Tue Jan 17, 2017 8:57 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Eq. 20?
- Replies: 1
- Views: 185
Re: Eq. 20?
Check Appendix 2A in the back of the book. Also, you could go online to check enthalpies of formation.
- Tue Jan 17, 2017 8:56 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Systems Chemistry
- Replies: 1
- Views: 188
Re: Systems Chemistry
Internal energy= q+w
Internal energy is 982 and heat absorbed is 492. This means that the work will be positive, suggesting that work is done on the system. Negative work suggests that the system does work and thus expends energy.
Internal energy is 982 and heat absorbed is 492. This means that the work will be positive, suggesting that work is done on the system. Negative work suggests that the system does work and thus expends energy.
- Sat Jan 14, 2017 9:59 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Clarifying Enthalpy As A State Function
- Replies: 1
- Views: 282
Re: Clarifying Enthalpy As A State Function
Enthalpy changes are additive, because they only depend on the final and initial conditions. Nothing else. In fact it can be extremely difficult to map out the middle and even requires calculus to try. But in essence, state functions have deltas which represents the final state minus the initial sta...
- Sat Jan 14, 2017 9:43 am
- Forum: Administrative Questions and Class Announcements
- Topic: Weekly posts
- Replies: 3
- Views: 467
Re: Weekly posts
From what I have heard, every week ends on Sunday and starts Monday. So if you post on Saturday, it will belong to the same week you posted on.
- Sat Jan 14, 2017 9:41 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: heat q(sys)+ q(surr) =0
- Replies: 3
- Views: 779
Re: heat q(sys)+ q(surr) =0
Given an exothermic reaction, for example, the system releases heat to its surroundings after product formation. If the heat released by the reaction is -q, then the heat absorbed by the surroundings can be +q. Conversely, an endothermic reaction will take heat from its surroundings to supplement a ...
- Fri Jan 13, 2017 7:12 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Problem 8.63c typo?
- Replies: 2
- Views: 301
Re: Problem 8.63c typo?
I would stick with the appendix value for the problem. On future quizzes and exams, there will be a table of enthalpy values for you to reference.
- Fri Jan 13, 2017 7:04 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Most Stable Form
- Replies: 4
- Views: 1618
Re: Most Stable Form
All elements have their natural, most stable state. Look at the periodic table to see the state of matter each element is at room temperature. Metals will generally be solids, and Bromine and Mercury are liquids at room temperature. In terms of having an enthalpy of formation value of 0, all single ...
- Wed Jan 11, 2017 7:32 am
- Forum: Administrative Questions and Class Announcements
- Topic: Random Enrollment Checks
- Replies: 9
- Views: 1531
Re: Random Enrollment Checks
I believe they are to make sure people who don't have the lecture for that time (or none at all) come into the halls and take up seats. The scene at the lecture hall on Monday was packed, with people outside of the enrolled lecture coming in. You should probably have a copy of your study list if you...
- Wed Jan 11, 2017 7:26 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Internal Energy Changes in a Closed System
- Replies: 1
- Views: 289
Re: Internal Energy Changes in a Closed System
A positive delta E would correlate to an increase in energy, while a negative delta E would be a decrease in energy. Different permutations of q and w can contribute to this, but if both q and w are positive, then the system gains energy. If q and w are both negative, the system gains energy. This m...
- Mon Nov 28, 2016 7:14 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: When to use atm v. bar units [ENDORSED]
- Replies: 4
- Views: 1243
Re: When to use atm v. bar units [ENDORSED]
I think that you can use either bar or atm. I would use atm since the problems we have encountered thus far use atm for solutions.
- Thu Nov 24, 2016 11:30 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: 11.59
- Replies: 1
- Views: 390
Re: 11.59
You need to calculate Q in order to know which way the reaction will go in order to reach equilibrium. That way, when you are setting up your ice box, you will know whether to put + or - x for reactants and products for the change (c).
- Wed Nov 16, 2016 9:05 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: MO diagrams for ions
- Replies: 3
- Views: 706
Re: MO diagrams for ions
Lewis structures can really help in these situations to see which atoms lose or gain electrons. Try creating a stable lewis structure for NO+. You will see that oxygen loses an electron and obtains a 1+ charge while being triple bonded to nitrogen. Both have a lone pair of electrons.
- Wed Nov 16, 2016 9:01 am
- Forum: Naming
- Topic: Alphabetizing Ligands
- Replies: 4
- Views: 522
Re: Alphabetizing Ligands
I don't think there is a particular order for writing ligands in a chemical formula. Formulas don't follow the alphabetical rule.
- Wed Nov 16, 2016 8:59 am
- Forum: Naming
- Topic: Convention for naming
- Replies: 2
- Views: 353
Re: Convention for naming
I don't believe order of the ligands matters when writing down the molecular formula from the name. However, when writing the name, ligands appear in alphabetical order.
- Mon Nov 07, 2016 10:09 pm
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Z>8, Z<8
- Replies: 8
- Views: 908
Re: Z>8, Z<8
Z stands for atomic number. So it means that elements that have an atomic number less than 8 or greater than 8 have a certain molecular orbital structure.
- Sun Nov 06, 2016 10:38 am
- Forum: Naming
- Topic: Naming Coordination Compounds
- Replies: 1
- Views: 284
Re: Naming Coordination Compounds
When naming coordination compounds, transition metals will be indicated with roman numerals since they can have more than one oxidation state. If you were to look at a periodic table with labeled oxidation states on the elements, there are some transition metals that stick to a particular oxidation ...
- Tue Nov 01, 2016 7:35 am
- Forum: Administrative Questions and Class Announcements
- Topic: Lewis Structures on the Midterm
- Replies: 2
- Views: 461
Re: Lewis Structures on the Midterm
You should check out previous year midterms as a good indicator of what kind of questions the midterm will be asking. Past midterms have many lewis-structure questions that asks to construct the shape of a molecule and answer some questions about its characteristics. The shape could be lewis, but vs...
- Wed Oct 26, 2016 7:00 am
- Forum: Ionic & Covalent Bonds
- Topic: Double Bonds
- Replies: 1
- Views: 288
Re: Double Bonds
Double bonds can be made if it the formal charge allows for it (ie. makes the atom more stable by doing so) and if the atom has enough electrons to do so. (hydrogen can't double bond) (Period 2 elements can't go over octet) In terms of calculating formal charge, you would have to calculate it every ...
- Wed Oct 26, 2016 6:56 am
- Forum: Electronegativity
- Topic: Electronegativity in Quiz 2 [ENDORSED]
- Replies: 3
- Views: 560
Re: Electronegativity in Quiz 2 [ENDORSED]
You should know general electronegativity trends in order to figure that out.
- Fri Oct 21, 2016 6:53 am
- Forum: Ionic & Covalent Bonds
- Topic: Ionic vs Covalent Bonds
- Replies: 1
- Views: 351
Re: Ionic vs Covalent Bonds
Anything less than 0.5 electronegativity difference is a non-polar covalent bond.
From 0.5 to 2.1, it is a polar-covalent bond.
From 2.1+ is ionic bond.
From 0.5 to 2.1, it is a polar-covalent bond.
From 2.1+ is ionic bond.
- Fri Oct 21, 2016 6:50 am
- Forum: Quantum Numbers and The H-Atom
- Topic: Ch 2.1
- Replies: 1
- Views: 365
Re: Ch 2.1
Ionization energy is the energy required to remove one electron from an element in the periodic table. So the energy required to remove an electron from ground state and the ionization energy is essentially the same thing.
- Sun Oct 16, 2016 7:52 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Naming Elements
- Replies: 1
- Views: 232
Re: Naming Elements
The d orbital should be listed first in the given scenario. The p orbital occurs in the p block, whereas Zr, for example, hasn't reached the p block in the 5th energy level. Zr is in the d block, past the s block. In general, just follow the blocks of the periodic table from left to right, and it sh...
- Tue Oct 11, 2016 7:57 am
- Forum: Properties of Light
- Topic: QUIZ 1 [ENDORSED]
- Replies: 7
- Views: 1128
Re: QUIZ 1 [ENDORSED]
For Quiz 1 the formula and name of all compounds will be provided.
- Sun Oct 09, 2016 7:57 pm
- Forum: Trends in The Periodic Table
- Topic: Up to which topic will the first quiz cover? [ENDORSED]
- Replies: 2
- Views: 386
Re: Up to which topic will the first quiz cover? [ENDORSED]
The Self-Prep Workbook Quiz is a great indicator of what kind of content will be on the quiz. Quiz 1 should be on Fundamentals and Chapter 1. The Heisenberg Uncertainty Equation should be the last concept that will be on the quiz. Talks about, for example, orbital structures will not be on the quiz....
- Thu Oct 06, 2016 2:22 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Workbook - Quiz 1
- Replies: 2
- Views: 487
Re: Workbook - Quiz 1
Page 14 of your course reader should be able to help you out. But to explain, when you purchased your 2016 course reader, it included a tan 2016 workbook that includes practice quizzes and other helpful materials from previous years. Self-Prepatory quiz 1 that does not have the answers in the back n...
- Tue Oct 04, 2016 5:32 pm
- Forum: Ionic & Covalent Bonds
- Topic: Copper (I) Oxide [ENDORSED]
- Replies: 1
- Views: 254
Re: Copper (I) Oxide [ENDORSED]
The Roman Numeral (I) indicates the positive charge of the metal cation. Metals are always positive, so copper will be positive. The (I) will indicate its charge, so copper will be Cu1+. Reason for the Roman Numerals is that some transition metals can have different charges (i.e. 2+ or 3+) and the n...
- Tue Oct 04, 2016 1:51 pm
- Forum: General Science Questions
- Topic: Workbook 2016
- Replies: 1
- Views: 637
Re: Workbook 2016
The workbook comes with the 2016 Course Reader for the class. The workbook will be turned in to the TA before or on the day of your quiz and will be graded in the workbook. That being said, I believe the doing the self-prep quiz directly from a workbook may be the only way to get credit. You may be ...
- Mon Oct 03, 2016 3:51 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Preparatory Self Quizzes [ENDORSED]
- Replies: 3
- Views: 548
Re: Preparatory Self Quizzes [ENDORSED]
Page 14 of the new 2016 Course Reader has a description.
As far as turning them in, they can be turned in on the day of your quiz to your TA.
As far as turning them in, they can be turned in on the day of your quiz to your TA.
- Mon Oct 03, 2016 3:47 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Even numbered textbook solutions?
- Replies: 2
- Views: 426
Re: Even numbered textbook solutions?
I think there might be some select even-numbered textbook problems on Chemistry Community.
I have seen a couple already posted.
I have seen a couple already posted.
- Sun Oct 02, 2016 12:31 pm
- Forum: Significant Figures
- Topic: Sig Figs in a problem with addition & multiplication [ENDORSED]
- Replies: 5
- Views: 1580
Re: Sig Figs in a problem with addition & multiplication [ENDORSED]
I believe that Dr. Lavelle has said to do the sig figs at the end of the problem. I have also talked to a couple TAs and they have said this as well.
Hope this helps!
Hope this helps!
- Thu Sep 29, 2016 1:27 pm
- Forum: Photoelectric Effect
- Topic: Photoelectric effect AV Post assessment #8 and #14
- Replies: 3
- Views: 432
Re: Photoelectric effect AV Post assessment #8 and #14
C=v(lambda) doesn't really describe the photoelectric effect since the photoelectric effect describes light behaving like a particle, not a wave. The equation is applicable to the wave-like nature of light and would explain why scientists performing the photoelectric experiment initially thought tha...
- Mon Sep 26, 2016 2:51 pm
- Forum: Balancing Chemical Reactions
- Topic: H.13 How To Write This Chemical Equation?
- Replies: 4
- Views: 2700
Re: How To Write This Chemical Equation?
I do not think the problem is correct. I may be wrong, but it seems that one part of the problem is from one question and another part is from another. H13, which is the question I think you're referring to, is as follows: When nitrogen and oxygen gases react in the hot exhaust environment of an aut...