A 17.5-g quantity of dry ice (solid carbon dioxide) is allowed to sublime (evaporate) in an apparatus like the one shown in the figure below. Calculate the expansion work done against a constant external pressure of 0.975 atm and at a constant temperature of 26Â°C. Assume that the initial volume of dry ice is negligible and that CO2 behaves like an ideal gas.

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Tod ThielLv2

17 Dec 2019

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A 65.56 g quantity of dry ice (solid carbon dioxide) is allowed to sublime (evaporate) in a position like apparatus. Calculate the expansion work done against external pressure of 0.956 atm and at a constant temperature of 22C. Assume that the initial volume of dry ice id negligible and the CO2 behaves as an ideal gas (1Lâ¢atm=101.3J)

Dry ice is simply frozen carbon dioxide (carbon dioxide in the solid state) and is pretty cold with a temperature of -109.3 degrees F (-78.5 degrees C). For comparison, liquid nitrogen is MUCH colder at -321 degrees Fahrenheit (-196 degrees Celsius).The carbon dioxide in dry ice will also go directly from the solid state (frozen carbon dioxide) to the gaseous state. This process is called sublimation.

You have likely seen examples of sublimation in your own freezers on food items, such as meat, that are kept for long times in the freezer, and/or not well sealed from the air. This is often called âfreezer burnâ, and it is caused by the sublimation of water molecules from ice crystals present on the surface of meat into the dry freezer air.

You have 2.44 grams of dry ice in a 6.0 Liter container maintained at 31.2⁰C. What is the pressure in the container after ALL the dry ice has sublimated (transformed to the gaseous state)?

-You will use the Ideal Gas Law here, and you must determine which specific value to use for the constant âRâ

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