Confused - Pressure in a canister?

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SUMMARY

The discussion centers on the calculation of pressure in a CO2 canister, where a manufacturer claims a standard canister contains 16g of CO2 at a volume of 20cm³. Using the ideal gas law, the calculated pressure is 444 Bar, while the manufacturer states it is 60 Bar. Participants suggest that the discrepancy may arise from the CO2 not behaving as an ideal gas and possibly being in a liquid state, affecting the pressure readings.

PREREQUISITES
  • Understanding of the ideal gas law (P = nRT/V)
  • Basic knowledge of gas properties and states (ideal vs. non-ideal gases)
  • Familiarity with unit conversions (cm³ to m³)
  • Awareness of vapor pressure concepts
NEXT STEPS
  • Research the behavior of non-ideal gases and how they differ from ideal gases
  • Study the phase diagram of carbon dioxide to understand pressure-temperature relationships
  • Learn about vapor pressure and its implications for gases in canisters
  • Explore advanced gas laws and equations for real gases, such as the Van der Waals equation
USEFUL FOR

Chemists, engineers, and anyone involved in the handling or manufacturing of gas canisters, particularly those working with carbon dioxide and pressure calculations.

b.kiddo44
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A manufacturer quotes a standard CO2 canister contains 16g of CO2 at a volume of 20cm^3.

So I need to calculate the pressure in the canister...

Using ideal gas law

P = nRT/V
n = 0.364mol (16 of co2)
R = 8.314 J/Kmol (universal gas constant)
T = 294k (gas is at room temp 21 deg C)
V = 20cm3 (volume of canister as quoted)

P = 444 Bar

However the manufacturer quotes the canister pressure to be 60Bar! This seems a bit more realistic to me but I've no idea how this could be the case.

Any thoughts to clear up the confusion?
 
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Its must be cubic meter.Convert 20 cm3 to meter3
 
Good point, but I already did the conversion to m^3 in the calculation to give 444Bar.
 
I don't know chemical very well but maybe there's another formula to calculate pressure.Maybe CO2 supposed to be non-idel gas.
Your equation seems correct.
 
hum, I don't think it matters if the gas is 'ideal' or not. The manufacturer quoting 16g of CO2 in a 20cm^3 canister stored at room temperature. I'm confused as to where the 60 Bar quote comes from.
 
Perhaps the CO2 is not all a gas under pressure and the pressure is the vapor pressure at a given temperature.
 
You wrote it isn't it ?
 
there's only two option.First option this is not an idel gas.Ideal gas make the equation simpler but maybe there's another type of equation which I said before.
Second think As you said its not 60 bar

there's no other option cause our solution is correct.
 

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