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Photon336
 one year ago
Chem question
Photon336
 one year ago
Chem question

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Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Question on vapor pressure

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Condensation: dealing with kinetic/potential energy

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@Rushwr @taramgrant0543664 @Empty

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0I'm thinking D, D and then C I think I have it in the right order

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0condensation is \[(g) \rightarrow (l)\] So i thought kinetic energy would have to go down. for the second one

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1For the 1st one I'll go with B

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0@Rushwr why not D? can you explain..

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0not saying you're wrong

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0Yep sorry kinetic energy does decrease

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1cuz HCl has dipole dipole interactions

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0ok so for the first one it is B

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1for the second one I'll go with D or b

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0dw:1438060894240:dw isn't this covalent bonding?

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1it is but they have asked us for the intermolecular interaction not the bonding type right?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0C2H6 is covalent bonding

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0wouldn't that be london dispersion forces/ vanderwalls forces for c2H4?

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1for the last question I'll go with D

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0I'm pretty sure D is right for that last one

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1yes that is london dispersion forces @Photon336

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Yeah I think the last one is D. let me check

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0oh.. wait.. it's E whaaat...

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Phase change, is an equilibrium process so i'm going to make a stretch and say that at an equilibrium process temperature = constant so KE stays the same. (don't quote me on that)

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I can't explain why Potential energy decreases.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0FYI If you want to see the rest of the questions i attached them here,

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0Condensation is gas to liquid so you're creating order and energy decreases

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0OK, but the way though of it was that if kinetic energy goes down then PE has go up KE + PE + Wf = Mechanical energy. don't know thinking that they have to be conserved. (but i'm working backwards from the answer) the say PE went down. I guess we can go on to the second question about vapor pressure. I attached the PDF to the conversation.

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1maybe it's like this. When a liquid is condensed all he molecules pack in to a smaller volume right? So heat is given out. That heat is given out by the potential energy having the kinetic energy unchanged.

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1something like that would do right?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0Yes it would

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0forcing something into a smaller volume would imply a decrease in entropy

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0But i wonder if that's the case during any phase change

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0b/c a phase change is an equilibrium process, where t is constant, but i think that's probably the best way to explain it.. so the heat is released by the (total potential energy) going down, leaving KE unchanged?

taramgrant0543664
 one year ago
Best ResponseYou've already chosen the best response.0Sounds pretty good to me. I'm going to bed now so good night enjoy the rest of the question and I'll check in again with this tomorrow!

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0will post one more question after this then I g2g

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I'm not sure about the vapor pressure question @Empty thoughts?

Empty
 one year ago
Best ResponseYou've already chosen the best response.1Hmmm Yeah I was a bit confused by this as well I was almost sure it was D but I was also fairly certain potential energy decreased as well since the distances between particles should be less as they start to bond to each other slightly. I guess I need to go look at vapor pressure and all this I'm sort of rusty I guess.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0I'm going to repost the vapor pressure question tomorrow

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0so as you go from say (s) to liquid the kinetic energy increases but PE decreases right?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0We didn't get to the vapor pressure question

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.0Ok so for im assuming question 7 that you posted about the vapor pressure. I am going with answer choice d. Both I and III are correct but II increasing the volume wouldn't have any affect on the vapor pressure.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.07 was A. but i'm not sure as to why though. @sweetburger equilibrium vapor pressure. like I knew increasing temperature, increases vapor pressure, but isn't the equilibrium vapor pressure = external pressure/ boiling point? NOT sure. I "guess" equilibrium = temperature dependent, so if you heat up or cool down something equilibrium will change/shift

sweetburger
 one year ago
Best ResponseYou've already chosen the best response.0I understand how heat affects the equilibrium, but I also thought that pressure would have an affect but thinking about it now If the pressure was increased above the surface there would be no true affect on the number of molecules coming out and the number going back in.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.0Only other thing would be if you changed the external pressure ..
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