Search found 11 matches
- Thu Mar 16, 2017 10:22 pm
- Forum: Balancing Redox Reactions
- Topic: Winter 2016 final Q3A [ENDORSED]
- Replies: 5
- Views: 1113
Re: Winter 2016 final Q3A [ENDORSED]
My bad, Mn would have a charge of 7+ and gain 5 electrons, apparently I can't add lol
- Thu Mar 16, 2017 2:01 pm
- Forum: *Haloalkanes
- Topic: Priority when Naming
- Replies: 2
- Views: 1456
Re: Priority when Naming
You are correct. There is priority within the functional groups, but I'm not sure if Dr. Lavelle would give us two different functional groups attached to the same parent chain.
- Thu Mar 16, 2017 1:56 pm
- Forum: *Cyclopropanes and Cyclobutanes
- Topic: Torisonal vs. Steric Strain
- Replies: 2
- Views: 1513
Re: Torisonal vs. Steric Strain
Steric strain is the result of nonbonded interaction. On page 107 of the course reader you can see that the strain arises from hydrogens bonded to different carbons trying to occupy the same space. Torsional strain comes from electron repulsion when a molecule is rotating between staggered and eclip...
- Thu Mar 16, 2017 1:48 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Winter 2016 Final Exam Q2A [ENDORSED]
- Replies: 7
- Views: 1508
Re: Winter 2016 Final Exam Q2A [ENDORSED]
Last quarter in 14A, Professor Li said that it is common practice to use bar as the unit of pressure, but I'm not sure if Dr. Lavelle specified using bar or atm. Just be sure that you are consistent with units when doing calculations so that you don't lose points for conversions.
- Thu Mar 16, 2017 1:38 pm
- Forum: Balancing Redox Reactions
- Topic: Winter 2016 final Q3A [ENDORSED]
- Replies: 5
- Views: 1113
Re: Winter 2016 final Q3A [ENDORSED]
Fe initially has a charge 2+ and loses electrons to have a final charge of 3+ (lose electrons = oxidation) The molecule MnO4 has a net charge of 1-. If you break it up into Mn and O you will see that Mn has a 6+ charge because O is 8- (oxygen is almost always 2-). The given information says that Mn ...
- Thu Mar 16, 2017 1:30 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: How to tell if you're dealing with an ideal gas?
- Replies: 3
- Views: 2031
Re: How to tell if you're dealing with an ideal gas?
Argon and Neon are both noble gases, and I believe it is standard to treat noble gases like ideal gases.
- Thu Mar 16, 2017 1:23 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3673802
Re: Post All Chemistry Jokes Here
If you're not part of the solution, you're part of the precipitate.
- Sun Feb 05, 2017 7:12 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Potential Difference vs. EMF
- Replies: 2
- Views: 530
Re: Potential Difference vs. EMF
Standard reduction potential (E°) is an intensive property that gives the voltage difference between the anode and cathode (see course reader page 47). EMF is the cell potential, which is the maximum voltage actually generated; it is denoted by Ecell.
- Sat Jan 28, 2017 4:35 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy=enthalpy/T
- Replies: 2
- Views: 602
Re: Entropy=enthalpy/T
You can also think of that equation as ΔS = q/T as given by the second law of thermodynamics. ΔS will always be positive for a spontaneous reaction, meaning any reaction/change that happens on its own (i.e. volume of a gas expanding when the volume of the container increases). Any non-spontaneous ch...
- Thu Jan 19, 2017 6:09 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Specific heat capacity [ENDORSED]
- Replies: 1
- Views: 586
Re: Specific heat capacity [ENDORSED]
The specific heat capacity of water is on the formula sheet given with the course reader. I would assume that any other values needed for a problem would be given.
- Sat Jan 14, 2017 12:25 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Definition of bond enthalpy
- Replies: 1
- Views: 434
Re: Definition of bond enthalpy
That is correct! On page 16 of the course reader Dr. Lavelle discusses bond enthalpies, highlighting that energy is required to break bonds (+ΔH) and that energy is released when a bond is formed (- ΔH).