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 ?

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Ideal Gas Law:

PV=nRT

moles (n)=mass (m)molar mass (M)

PV=mRTMPVP=mRTMPV=mRTMP


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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Problem Details

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 ?

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