Problem: A piece of dry ice (solid carbon dioxide) with a mass of 28.5 g sublimes (converts from solid to gas) into a large balloon.Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at 23 oC and a pressure of 746 mmHg ?

Ideal Gas Law:

$PV = nRT$

$moles (n) = \frac{mass (m)}{molar mass (M)}$

$PV = \frac{mRT}{M} \frac{P V}{P} = \frac{mRT}{MP} V = \frac{mRT}{MP}$

Calculate the volume of the balloon:

molar mass carbon dioxide (CO₂) = 44.01 g/mol

T = 23°C + 273.15 = 296.15 K

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A piece of dry ice (solid carbon dioxide) with a mass of 28.5 g sublimes (converts from solid to gas) into a large balloon.

Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at 23 ^oC and a pressure of 746 mmHg ?

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 Augustine's class at High Point University.