Topic: Partial pressure problem (Read 4763 times)

StillLearning · « **on:** October 04, 2008, 06:03:58 PM »

Here's the problem:

A 1.25 g sample of dry ice is added to a 750 flask containing nitrogen gas at a temperature of 25.0 C and a pressure of 720 mmHg. The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 C. What is the total pressure in the flask?

I'm not sure where to start. It seems to me that I need to know how much gas a 1.25 g sample of dry ice will produce, but that's way over my head at this point. Hopefully i'm approaching the problem wrong....otherwise i'm in trouble.

StillLearning · « **Reply #1 on:** October 04, 2008, 06:10:04 PM »

Ok, I just looked up the formula for dry ice. Apparently it's just solidified CO2. So, with that, can I just calculate the molecular mass, then convert that to moles, and plug the values into the ideal gas law formula, PV=nRT?

StillLearning · « **Reply #2 on:** October 04, 2008, 06:18:33 PM »

Nevermind.....that didnt work either. I'm still lost. Does anyone know how to do this?

Borek · « **Reply #3 on:** October 04, 2008, 06:32:19 PM »

Total pressure is given by pV=nRT, but you have two gases in the flask.

StillLearning · « **Reply #4 on:** October 04, 2008, 06:38:34 PM »

I got it. Just calculated the pressure from the sublimed CO2 and added that to the 720mmHg that was already in there.

Topic: Partial pressure problem (Read 4763 times)

StillLearning

Partial pressure problem

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