🤓 Based on our data, we think this question is relevant for Professor Lehman's class at PDX.

Step 1

$\mathbf{35}\mathbf{.}\mathbf{3}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}\mathbf{}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}{\mathbf{44}\mathbf{.}\mathbf{01}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}}$** = 0.8021 mol CO _{2}**

Step 2

$\overline{){\mathbf{PV}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{nRT}}}\phantom{\rule{0ex}{0ex}}\mathbf{P}\mathbf{\hspace{0.17em}}\mathbf{=}\mathbf{}\frac{\mathbf{nRT}}{\mathbf{V}}$

A 35.3 g sample of solid CO_{2} (dry ice) is added to a container at a temperature of 100 K with a volume of 4.2 L.

If the container is evacuated (all of the gas removed), sealed, and then allowed to warm to room temperature T = 298 K so that all of the solid CO_{2} is converted to a gas, what is the pressure inside the container?

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 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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Lehman's class at PDX.