# 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:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

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:

$\frac{\mathbf{P}\overline{)\mathbf{V}}}{\overline{)\mathbf{V}}}\mathbf{=}\frac{\mathbf{nRT}}{\mathbf{V}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{P}}{\mathbf{=}}\frac{\mathbf{nRT}}{\mathbf{V}}}$

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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?