A container under #2558*"psi"# pressure contains carbon dioxide and whose partial pressure is #54.6*"bar"# and #NO_2#? What is #P_(NO_2)# in atmospheres?

1 Answer
May 25, 2017

Answer:

The sum of the partial pressures is equal to the total pressure.

Explanation:

#"Dalton's Law of partial pressures"# holds that in a gaseous mixture, the total pressure is the sum of the individual partial pressures; i.e. the sum of the pressures of the components if they ALONE occupied the container.

You have a real dog's breakfast of pressure terms here that can only have come from the US of A.

Anyway the total pressure is...................

#P_"Total"=2558*"psi"=(2558*"psi")/(14.7*"psi"*atm^-1)=174*atm=174*"bar................................"#

which is a prodigiously high pressure. (Note that #1*"bar"# is as near as dammit equal to #1*atm#).

Now #P_"Total"=P_(NO_2)+P_(CO_2)#

And thus..................................

#P_(NO_2)=P_"Total"-P_(CO_2)=(174-54.6)*atm=119.4*atm#.

These are exceptionally high pressures, and the vessel containing these gases would be exceptionally sturdy.