How Do You Find Volume Using PV=nRT?

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Homework Help Overview

The discussion revolves around calculating the volume of an ideal gas using the ideal gas law, PV = nRT, with specific values for the number of moles, temperature, and the gas constant. Participants are exploring the implications of using different units for pressure and the resulting volume calculations.

Discussion Character

  • Exploratory, Assumption checking, Mathematical reasoning

Approaches and Questions Raised

  • Participants are attempting to calculate volume using the ideal gas law with varying assumptions about pressure units (atm vs. Pascals). There are questions about the appropriate value of the gas constant R in different unit systems and the implications of unit conversions on the final volume result.

Discussion Status

The discussion is active with participants sharing their calculations and questioning the validity of their results based on unit choices. Some guidance has been provided regarding the use of units, but there is no explicit consensus on the correct volume calculation yet.

Contextual Notes

Participants are navigating potential confusion regarding the use of different pressure units and the conversion between cubic meters and liters. There is an acknowledgment that the calculated volume appears large for practical scenarios, prompting further discussion about the assumptions made in the calculations.

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Homework Statement


upload_2015-5-15_0-53-46.png


Homework Equations


PV = nRT

The Attempt at a Solution


n = 5.3 moles
R = 8.31 J/(mol K)
T = 273 K
now, with P, do we use 1 atm or 1.013 x 105

i'll go with the latter, and the answer comes out to be 0.119 liters , does this sound correct?
 
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goonking said:

Homework Statement


View attachment 83502

Homework Equations


PV = nRT

The Attempt at a Solution


n = 5.3 moles
R = 8.31 J/(mol K)
T = 273 K
now, with P, do we use 1 atm or 1.013 x 105

i'll go with the latter, and the answer comes out to be 0.119 liters , does this sound correct?
What is R in terms of liter-atm/mol K ?
 
Raghav Gupta said:
What is R in terms of liter-atm/mol K ?
hmm, it is 0.082

also, do we normally express P in Pascals or atm?
 
goonking said:
hmm, it is 0.082

also, do we normally express P in Pascals or atm?
In SI units it is Pa but normally it is a very small unit.
In our day to day life we use atm.
Remember if you are solving you should keep a track on units.
Your attempt is also good.
You will get answer in m3 and then 1m3 = 1000 liter.
 
Raghav Gupta said:
In SI units it is Pa but normally it is a very small unit.
In our day to day life we use atm.
Remember if you are solving you should keep a track on units.
Your attempt is also good.
You will get answer in m3 and then 1m3 = 1000 liter.
hmmm, is 1.19 L correct?
 
goonking said:
hmmm, is 1.19 L correct?
No, can you show what have you done?
 
Raghav Gupta said:
No, can you show what have you done?

P V = n R T
(1.013x105) V = (5.3 moles )( 0.082 liter-atm/mol K) (273K)

V = 0.00119 , I'm pretty sure this is in liters
 
goonking said:
P V = n R T
(1.013x105) V = (5.3 moles )( 0.082 liter-atm/mol K) (273K)

V = 0.00119 , I'm pretty sure this is in liters
But P should be in atm then.
I said keep track of units.
So take P = 1atm.
 
Raghav Gupta said:
But P should be in atm then.
I said keep track of units.
So take P = 1atm.
so V = (5.3 moles )( 0.082 liter-atm/mol K) (273K) = 118.64 Liters?

thats huge for a bottle
 
  • #10
goonking said:
so V = (5.3 moles )( 0.082 liter-atm/mol K) (273K) = 118.64 Liters?

thats huge for a bottle
Yeah, that was what I was getting.

Yeah, that is huge for a bottle but holding 5.3 moles of an ideal gas is a big thing.
 
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