Problem: A 1.25 -g sample of dry ice is added to a 765 -mL flask containing nitrogen gas at a temperature of 25.0 oC and a pressure of 735 mm Hg . The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 oC.What is the total pressure in the flask?

FREE Expert Solution

We’re being asked to calculate for the total pressure in the flask.


We’re going to calculate the pressure of each gas first using the ideal gas equation:

PV=nRT

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

Rearranging the ideal gas equation:

PVV=nRTVP=nRTV

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Problem Details

A 1.25 -g sample of dry ice is added to a 765 -mL flask containing nitrogen gas at a temperature of 25.0 oC and a pressure of 735 mm Hg . The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 oC.

What is the total pressure in the flask?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.