How Do You Find Volume Using PV=nRT?

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SUMMARY

The discussion centers on calculating the volume of an ideal gas using the ideal gas law equation PV = nRT. The values provided include n = 5.3 moles, R = 0.082 liter-atm/(mol K), and T = 273 K. The pressure P was debated between using 1 atm and 1.013 x 105 Pa, with the consensus leaning towards using 1 atm for practical calculations. The final calculation yielded a volume of approximately 118.64 liters, which was acknowledged as substantial for a single container.

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  • Understanding of the ideal gas law (PV = nRT)
  • Knowledge of unit conversions between atmospheres and Pascals
  • Familiarity with the concept of moles in chemistry
  • Basic proficiency in algebra for solving equations
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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
 
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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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