O ENTROPY AND FREE ENERGY Predicting qualitatively how entropy changes with temperature . jem 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. For eac System Change AS O AS < 0 The nitrogen expands from a volume of 8.0 L to a volume of 10.0L while O AS = 0 A few moles of nitrogen (N,) gas. the temperature is held constant at 55.0 °C. O AS > 0 not enough information O AS < 0 O AS = 0 The ammonia evaporates at a constant temperature of 63.0 °C. A few grams of liquid ammonia (NH3). O AS > Q not enough information O AS <0 The carbon dioxide is heated from -7.0 °C to 61.0 °C and is also compressed from a volume of 7.0 L to a volume of 6.0 L. O AS = 0 A few moles of carbon dioxide (Co,) gas. O AS > 0 not enough
O ENTROPY AND FREE ENERGY Predicting qualitatively how entropy changes with temperature . jem 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. For eac System Change AS O AS < 0 The nitrogen expands from a volume of 8.0 L to a volume of 10.0L while O AS = 0 A few moles of nitrogen (N,) gas. the temperature is held constant at 55.0 °C. O AS > 0 not enough information O AS < 0 O AS = 0 The ammonia evaporates at a constant temperature of 63.0 °C. A few grams of liquid ammonia (NH3). O AS > Q not enough information O AS <0 The carbon dioxide is heated from -7.0 °C to 61.0 °C and is also compressed from a volume of 7.0 L to a volume of 6.0 L. O AS = 0 A few moles of carbon dioxide (Co,) gas. O AS > 0 not enough
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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