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@Rushwr @taramgrant0543664 @Empty
I'm thinking D, D and then C I think I have it in the right order
condensation is \[(g) \rightarrow (l)\] So i thought kinetic energy would have to go down. for the second one
For the 1st one I'll go with B
@Rushwr why not D? can you explain..
not saying you're wrong
Yep sorry kinetic energy does decrease
cuz HCl has dipole dipole interactions
ok so for the first one it is B
for the second one I'll go with D or b
not sure though
|dw:1438060894240:dw| isn't this covalent bonding?
Non polar covalent?
it is but they have asked us for the intermolecular interaction not the bonding type right?
C2H6 is covalent bonding
oh yeah... true !
wouldn't that be london dispersion forces/ vanderwalls forces for c2H4?
for the last question I'll go with D
I'm pretty sure D is right for that last one
yes that is london dispersion forces @Photon336
Yeah I think the last one is D. let me check
oh.. wait.. it's E whaaat...
Phase 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)
I can't explain why Potential energy decreases.
Condensation is gas to liquid so you're creating order and energy decreases
OK, 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.
maybe 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.
something like that would do right?
Yes it would
forcing something into a smaller volume would imply a decrease in entropy
But i wonder if that's the case during any phase change
b/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?
Sounds 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!
will post one more question after this then I g2g
I'm not sure about the vapor pressure question @Empty thoughts?
Hmmm 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.
I'm going to re-post the vapor pressure question tomorrow
so as you go from say (s) to liquid the kinetic energy increases but PE decreases right?
We didn't get to the vapor pressure question
Ok 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.
7 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
I 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.
Only other thing would be if you changed the external pressure ..