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Based off of the portfolio I'm doing there is an inverse relationship between the pressure and volume.
Not really sure I comprehend your question, particularly this part: What conclusions can you make about the PV product with Ideal Gas 1, MW = 4 g/mol? what do you mean by Ideal Gas 1 Anyways, I will try to help. PV = nRT Where, P = pressure (atm) V = volume (L) n = moles R = 0.082L*atm/(mol*K) T = Temperature (K) Lets see if there really is an inverse relationship between pressure and volume using simple algebra PV = nRT P = nRT/V Seems like there is, assuming moles, Temperature and R are constants. Pressure is proportional to the inverse of Volume
This makes sense if you think about it higher pressure means that the gas is more condensed (bouncing off the sides of the container more) Thus as pressure increase volume Decrease Alternatively, As volume increases pressure decreases
7.336 1.000 7.336 2.445 3.000 7.335 1.223 6.000 7.338 815.1 9.000 7335.9
Well the first column going downward is Volume & then the second is pressure & the third is PV
I'm not sure what you are asking? Can you please clarify your question. Know that PV is just Pressure*Volume
The numbers I just gave you are ideal gas 1 so how do I use that to answer the question being asked up above?
It is asking you to look at the data and draw conclusions from it. What does this graph tell you about pressure in relation to volume and vice versa. I just went over it with you :)
That's what doesn't make sense to me I already answered a similar question I'lls how you. :P
Well does the value of PV change much, when the ratio of Volume to Pressure is changed?
I'm so retarded, I was making things seem way harder than they actually were. u_u
I understand what the question is asking me. :P
Don't be so hard on yourself, we are all guilty of over thinking things :) If you have any other questions feel free to ask me.
But what can I conclude when all of the PV products have no real relation? The first three PV products are 7. something but the last one is 7###. something.
The units of PV are Pressure*Volume or atm*L Ignore the slight deviations, ultimately PV is a constant "PV = k1 which means that pressure multiplied by volume gives you a constant, k. This is not the same constant for every reaction; it differs from gas to gas." Source: http://www.wyzant.com/Help/Science/Chemistry/Gas_Laws/ Read the portion on Boyle's law
So would that be my answer? I did read a little I'm opening my book right now. xP Oh, and thank you for helping me!!!! :) <3
You should also comment on the observed deviations in the PV constant, why do you think that there are deviations?
I'm reading about the constant etc. right now. I shoul dhave read my book maybe cakes. xP
What does that mean? :P
What does what mean?
deviations in the PV constant, why do you think that there are deviations?
Sorry tired I should rephrase that, You should also comment on the observed deviations in the PV constant, why do you think there are deviations in the results?
No need to apologize, what's deviations?
notice how the values of PV are not the same for every result and that they differ, why do you think that they differ? Remember you are measuring these values in a lab.
It might be good to include a reason for the deviations in PV, if it is a constant shouldn't every value observed be the same?
They differ because of the fact that there are different pressure and volume amounts?
I'm sorry for all of these questions you have been a big help!!! <3
Ahhh nvm I'm tired and not making any sense sorry if I confused you. I just wanted to say that if these values were measured experimentally there could be error inherent in the results which could be a reason for seeing slight differences in PV value
but I dont think that makes any sense so disregard it.
Alright, well thanks for all your help! :)
Yeah No problem if you have any other questions feel free to message me