For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few grams of water vapor (H₂O). A few moles of nitrogen (N₂) gas. Change The carbon dioxide is heated from -18.0 °C to 79.0 °C and also expands from a volume of 2.0 L to a volume of 12.0 L. The water condenses to a liquid at a constant temperature of 10.0 °C. The nitrogen is compressed from a volume of 13.0 L to a volume of 1.0 L while the temperature is held constant at 9.0 °C. O ΔS AS < 0 OAS >0 AS = 0 not enough information O AS<0 O AS = 0 OAS >0 O not enough information ΔS < 0 OAS = 0 OAS >0 Ο not enough information

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few grams of water vapor (H₂O). A few moles of nitrogen (N₂) gas. Change The carbon dioxide is heated from -18.0 °C to 79.0 °C and also expands from a volume of 2.0 L to a volume of 12.0 L. The water condenses to a liquid at a constant temperature of 10.0 °C. The nitrogen is compressed from a volume of 13.0 L to a volume of 1.0 L while the temperature is held constant at 9.0 °C. O ΔS AS < 0 OAS >0 AS = 0 not enough information O AS<0 O AS = 0 OAS >0 O not enough information ΔS < 0 OAS = 0 OAS >0 Ο not enough information

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section16.3: Measuring Dispersal Of Energy: Entropy

Problem 16.3CE

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