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:*

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

A 1.25 -g sample of dry ice is added to a 765 -mL flask containing nitrogen gas at a temperature of 25.0 ^{o}C 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 ^{o}C.

What is the total pressure in the flask?

Frequently Asked Questions

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 Partial Pressure concept. You can view video lessons to learn Partial Pressure. Or if you need more Partial Pressure practice, you can also practice Partial Pressure practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Mieszawska's class at BROOKLYN CUNY.