Suppose 1.2 mol of a monatomic ideal gas initially at 11 L and 300 K is heated at constant volume to 590 K, allowed to expand isothermally to its initial pressure, and finally compressed at constant pressure to its original volume, pressure, and temperature. During the cycle, what are (a) the...
ah success! haha that's like the first answer i got completely right XD
ok one more quick question on a different problem, I am pretty sure i know how to do this one only I am a tad bit confused, i don't find it difficult enough to post a new thread so ima post it here an see if it'll get...
In the sample it says
The average kinetic energy of the entire gas is
K = N(3/2 * kT)
I tried it both E / that and E over the thing you posted and both answers were wrong? do i have the value of k right = 1.38e-23?
ohhh ok cool, nevermind i thought there was something to do with the mass of a single molecule...
anyway and then for part be it says the ratio of such and such:
would that be E / Kavg of the gas = E / N([3/2]kT) ?
so E / Kavg = 1.55e-20 / (3.3418e * [3/2] * 1.38e-23 * 302.7) = 7.402e-23?
an incredibly small fraction, then? hmm so
well the problem is asking for E based on n = the number of molecules per gram of sample, so since 3.34e22 is the number of molecules per gram of sample, would then E = 1.55e-20?
or am i somehow supposed to implement the use of a single molecule...
I'm honestly not quite sure
it says En = the heat of vaporization (518cal/g) where n is the molecules per gram. so that means En = 518cal/g, n = 3.3418e22 (whats the unit for this, mols?), then would E = 518cal/g / 3.3418e22 ?
that doesn't sound right seem's like an incredibly small number...
i guess i was trying to find the moles? or something, is it not
n = Msample / M
where M = molecular mass = 18.02g for H2O?
i guess i only got halfway, that would be the number of moles, correct?
then to get the number of molecules you multiply that by Avo's Number
(1/18.02mol) *...
I'm really starting to hate this class, the lecture didn't even begin to explain any of this I have no idea where to begin. We've been working on change in internal energy and work done on/by a gas, etc, and we get a question like this on the homework:
Water standing in the open at 29.7°C...
I don't understand that part, how do you determine if it isn't enough?
using this example, Q for the ice to 0 degrees is 1847040J (for both ice cubes), and Q for the water is 19213740J from 27 to 0 degrees
How do you determine if that is enough heat or not enough heat? Or is my math wrong?
so from what you said here's what I am getting:
C ice * M ice * (0 - [-13]) + L * M ice + C ice * M ice * (Tfinal - 0)
[heat to ice] + (heat of fusion) + [heat to melted ice] ?
and you do that with both cubes of ice?
edit: i just tried that and got the same answer (T0 =...
First of all, hi, and thanks ahead of time... I've been working on this homework for almost a week, even asked the teacher for help but still haven't been able to figure out what I've been doing wrong/missing. its online work so ill copy paste it
Homework Statement
(a) Two 32 g ice cubes...