Please help! Chemistry Question! HARD!?

Question

One of the treatments for gangrene and "the bends," is hyperbaric oxygenation. This occurs in a chamber in which oxygen is used at a higher-than normal pressures. This are the following informations, 3.00 x 10^3 liter hyperbaric chamber at a pressure of 250cm Hg and at 68F?

Consider the hyperbaric cylinder mentioned above. If the cylinder contains 2735 grams of carbon dioxide instead of oxygen, what volume would the gas occupy at 360 Torr and 850F?

Answer 1

I think this might be a trick question unless there is a mistake. They are asking for the volume of the gas (CO2); the volume of the gas would be the volume of the chamber it occupies! which was specified as 3.00 x 10^3 liters! The only exception would be if the temperature was so cold the gas liquified!

We can go ahead and plug the given numbers into the gas equation and see what happens anyway:

First get in proper units:

360torr = 360/760 = 0.474atm

850F = [850 -32] x5/9 + 273 = 727K

2735g/44g/mol = 62.16 moles CO2

Now plug into gas equation (solved for v):

v = [62.16 x 0.08205 x 727]/0.474 = 7822.5 liters

I still think there is a mistake in the question.

Answer 2

If the oxygen is contained in a chamber of x volume, then if it is replaced with CO2, doesn't the volume of the chamber remain the same? Is this a trick question?

Answer 3

Ideal gas law: PV = nRT
P = 360 torr
V = unknown to calculate
n = number of moles of gas (2735 g / 44 g per mol = mol)
R = gas constant (62.36 for torr)
T = 850 F (convert temp to C then add 273 to convert to K)