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a) The average kinetic energy of the molecules is greater, thus more molecules can enter the gaseous phase. b) The number of gaseous molecules above the liquid remains constant but these molecules have greater average kinetic energy. c) the faster moving molecules in the liquid exert a greater pressure. d) all the molecules have greater kinetic energies. e) the intermolecular forces between the molecules become less at higher temperatures.
@sweetburger posted a link to an online exam, I got it from there.
I know its not E as thats what happens at lower temperatures
I'm thinking that it could be D possibly
it's definitely not b and c
I'll go with A
I chose A but i was leaning towards E for some reason
A was going to be my second guess
@rushr yeah A was the correct one, why isn't it E?
higher temp = less IMF more particles in gas phase
I'm pretty sure that the intermolecular forces were greater at higher temperatures and lower at lower temperatures
@taramgrant0543664 why? i may have mixed it up
what I thought was When temperature increases definitely the vapor pressure increases right? When temperature increases the Kinetic energy of the molecules increases. the no, of molecules in liquid phase is high so the molecules will start entering the gaseous phase as their kinetic energy now is high
With the higher temperature means higher pressure since the molecules are moving around more. At high pressures, gas particles are forced into close proximity with one another, causing significant intermolecular interactions
I see, because vapor pressure is proportional to temperature, and when one is raised the other is. so the fraction of molecules in the gaseous phase increases. so i guess if i think of it like a sealed container, increasing the temperature increases amount of particles in the gaseous phase and they interact with one another more. But the thing was i considered E because i was thinking about say ideal gas behavior don't know why.. i was considering that at higher temperatures particles are moving around faster and the attractions become negligible while at lower temperature those forces become more relevant.
thing is.. like I get your explanations but i still don't get why E is eliminated.
how far in chemistry have you gone I can explain it another way but it will just confuse you if you haven't reached a specific point
@ higher temperatures aren't the molecules moving around more quickly so IMF goes down
Energy is made up of 4 things the translational energy the rotational energy, the vibrational energy and electrical energy so q= qT+qR+qV+qE The energy associated with the molecules interacting increases when temperature increase as each of the energies are affected by temperature so the increase in temperature increase the intermolecular forces because of each of the different energies
ok, got it, I think I was confusing two completely different terms.
so the idea is that higher pressure caused by greater # of molecules results in greater attractions
I think I confused it with ideal gases
Possibly but it sounds like you got it now
because for an ideal gas like higher temperature means less attraction between particles, but I guess that's under the assumption that there aren't any attractions to begin with.
Yes that makes sense
Thanks a lot I guess we can put this question to rest.