Chem-2 Gas Laws?

Been working on this question for a bit and I seem to be just off.

4.2g of dry ice (CO2) is placed in a baggie at 22 degrees C. Can the baggie hold all of the CO2 gas if the baggie can expand to a volume of 1.0L at a pressure of 1200 mmHg without bursting?

Answer:
4.2g of CO2 => 4.2g / 44 (g/mole) = 0.0954 moles of CO2.
22 ºC => 273 + 33 = 306 ºK
R = 62.3637 (L mmHg) / (K mole)

So, using the ideal gas equation:
PV = nRT
P = nRT/V
P = 0.0954 * 62.3637 * 306 / 1 = 1820.5 mmHg
which is more than the baggie can handle, meaning it will burst.

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