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A hyperbaric chamber is an enclosure containing oxygen at higher-than-normal pressures and used in the treatment of certain heart and circulatory conditions. What volume, in L, of O2(g) from a cylinder at 25.2°C and 155 atm, is required to fill a 4.20 x 103-L hyperbaric chamber to a pressure of 2.88 atm at 17.6°C

Argh! I’m so frustrated here…now what equation do I use here?

Use P1V1/T1 = P2V2/T2.

P1 = 155 atm
V1=?
T1= 25.2C+273.15 in Kelvin
P2=2.88 atm
V2=103 L (I am not sure what 4.20 x 103L means, so I ignored the 4.20; if that isn’t right, use the correct volume of the hyperbaric chamber)
T2=17.6C+273.15 in Kelvin.

Solve for V1.

2 Responses

1. Working with 32 characters here! Says:
   November 23rd, 2009 at 1:55 pm

   Use the ideal gas law!

   PV/nRT = 1 for both the cylinder(1) and the chamber(2), so:

   P1V1/nRT1 = P2V2/nRT2

   The number of molecules (n) must be conserved and the gas constant (R) doesn’t change, so these cancel in the equation, and rearranging gives:

   V1 = (P2V2/T2)*(T1/P1)

   Now, as soon as you can figure out the volume of the hyperbaric chamber you’re set!
   References :

2. drjackson955 Says:
   November 23rd, 2009 at 2:15 pm

   Use P1V1/T1 = P2V2/T2.

   P1 = 155 atm
   V1=?
   T1= 25.2C+273.15 in Kelvin
   P2=2.88 atm
   V2=103 L (I am not sure what 4.20 x 103L means, so I ignored the 4.20; if that isn’t right, use the correct volume of the hyperbaric chamber)
   T2=17.6C+273.15 in Kelvin.

   Solve for V1.
   References :

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