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Two moles of oxygen gas, which can be regarded as ideal with Cp=29.4 J/(K*mol) (independent of temperature), are initially at 298K in a volume of 12.5 dm^3. The gas is expanded reversibly to 353K at constant pressure. Calculate the final volume and q, w, delta U, and delta H.
Suppose that the gas in the previous question is reversibly compressed to half its volume at constant temperature (298K). Calculate the final pressure and q, w, delta U, and delta H.
Two moles of oxygen gas, which can be regarded as ideal with Cp=29.4 J/(K*mol) (independent of temperature), are initially at 298K in a volume of 12.5 dm^3. The gas is expanded reversibly to 353K at constant pressure. Calculate the final volume and q, w, delta U, and delta H.
Suppose that the gas in the previous question is reversibly compressed to half its volume at constant temperature (298K). Calculate the final pressure and q, w, delta U, and delta H.
Deanna HettingerLv2
17 Jul 2019
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