nandrol
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Pressure inside a heated, closed bottle
Can someone help me a bit.
Let's say I've got 3, 500ml glass bottles filled to 1/4th, half and 3/4th of their volume respectively with 25% ammonium hydroxide. How can I estimate
what will be their internal pressure?
EDIT: I'm sorry but I wrote it all wrong. I forgot that the bottles were suppose to be heated. The question was aboutl pressure in heated closed
bottles. What would be their internal pressure at 20 C, 100 C and 160 C. It's all theoretical, I don't want to experiment with exploding bottles.
Thanks for replies guys!
[Edited on 5-1-2013 by nandrol]
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Siggebo
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The pressures in the three bottles will be the same.
Current air pressure + vapor pressure of ammonia.
Edit: Wait, didn't think before I posted. Disregard second statement; it applies to an ideal system only.
The necessary data can be found at http://en.wikipedia.org/wiki/Ammonia_%28data_page%29#Vapor-L.... The calculation is analogous.
[Edited on 2013-1-4 by Siggebo]
[Edited on 2013-1-4 by Siggebo]
[Edited on 2013-1-4 by Siggebo]
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AndersHoveland
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On a somewhat related topic, a plastic soda bottle can hold between 3 to 5 atmospheres of pressure.
I'm not saying let's go kill all the stupid people...I'm just saying lets remove all the warning labels and let the problem sort itself out.
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nandrol
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I'm trying to count it but I'm not sure how to.
I assume I should first calculate the vapor pressure of ammonia, water and air using the Antoine Equation:
http://www.ehow.com/how_4479034_calculate-vapor-pressure.htm...
What next?
Should I count the mole fraction and multiply that by the vapor pressure like here:
http://www.ehow.com/how_6201518_calculate-vapor-pressure-sol...
or should I calculate each components mass fraction and multiply by vapor pressure:
http://www.ehow.com/how_12028243_calculate-vapor-pressure-pr...
[Edited on 5-1-2013 by nandrol]
[Edited on 5-1-2013 by nandrol]
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