CO2 -- Pressure of an ideal gas vs. what is measured on this pressure gauge

  • Thread starter havenly
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  • #1
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Homework Statement:
CO2
Relevant Equations:
vanderwaals equation p=nrt/V
A container of 0.5l containing 6 moles of CO2 are heated to 200 ° C on is interested in explaining the pressure variations between the pressure of a perfect gas and the actual value measured on a pressure gauge. The coefficients of the real gas a=3.59 [atm l2/mol2-] b=0.0427 [l /mol] indicate the only proposal that is fully true:
a. in this specific case the measured pressure and the pressure of the perfect gas are the same, it has no deviation
b.la actual gas pressure is 438.7 atm this pressure is lower than the pressure calculated by considering the gas how perfect this negative difference is due to the the fact that CO2 molecules have a real volume.
c. the pressure difference between the perfect gas and real 155.3 atm this deviation is due to the fact that CO2 molecules interact with each other and their shocks are inelastic
d. the error is of the order 6% this negative deviation is due to the fact that the molecules of CO2 have a real volume
e. la pressure difference between the perfect and real gas is 27.26 atm this deviation negative is due to the fact that CO2 molecules interact with each other and their shocks are inelastic

for the vanderwaals equation I get 437.57atm and by p=nrt/V =465.432 atm
I think a is false
 

Answers and Replies

  • #2
mjc123
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a is trivially false. What about the other statements? You are asked to identify the one which is true.
 
  • #3
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I think that c is also false because I don't get 155.3 B and E make me doubt How do I calculate the deviation?
 
  • #4
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CO2 can have a negative deviation?
 
  • #5
mjc123
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CO2 can have a negative deviation?
Well you calculated it (correctly)
 
  • #6
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Have you tried any other equation of state model (e.g., corresponding states) for comparison?
 

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