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Chapter 12 Calculating entropy change from reversible heat flow The heat of fusion AH, of dichloromethane (CH₂Cl₂) is 6.2 kJ/mol. Calculate the change in entropy AS when 35. g of dichloromethane melts at -95.1 °C. Be sure your answer contains a unit symbol and the correct number of significant digits.

Chapter 12 Calculating entropy change from reversible heat flow The heat of fusion AH, of dichloromethane (CH₂Cl₂) is 6.2 kJ/mol. Calculate the change in entropy AS when 35. g of dichloromethane melts at -95.1 °C. Be sure your answer contains a unit symbol and the correct number of significant digits.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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7:32 Blackboard Chapter 12 Recitation Chapter 12 X Read Only - Save a copy to edit. Calculating entropy change from reversible heat flow Using the Second Law to predict spontaneous change - Change The heat of fusion AH, of dichloromethane (CH₂Cl₂) is 6.2 kJ/mol. Calculate the change in entropy AS when 35. g of dichloromethane melts at -95.1 °C. Be sure your answer contains a unit symbol and the correct number of significant digits. During an exothermic chemical reaction, a solid is consumed and a gas produced. Mobile View A gas condenses to a liquid, neither absorbing nor releasing heat. A gas expands without absorbing or releasing heat. Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Q AD Read Aloud .5Gº O Yes. O No. @ Save a copy Is this change spontaneous? O Yes. O No. O Can't decide with information given. O Can't decide with information given. O Yes. O No. O Can't decide with information given. Headings
Transcribed Image Text:7:32 Blackboard Chapter 12 Recitation Chapter 12 X Read Only - Save a copy to edit. Calculating entropy change from reversible heat flow Using the Second Law to predict spontaneous change - Change The heat of fusion AH, of dichloromethane (CH₂Cl₂) is 6.2 kJ/mol. Calculate the change in entropy AS when 35. g of dichloromethane melts at -95.1 °C. Be sure your answer contains a unit symbol and the correct number of significant digits. During an exothermic chemical reaction, a solid is consumed and a gas produced. Mobile View A gas condenses to a liquid, neither absorbing nor releasing heat. A gas expands without absorbing or releasing heat. Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Q AD Read Aloud .5Gº O Yes. O No. @ Save a copy Is this change spontaneous? O Yes. O No. O Can't decide with information given. O Can't decide with information given. O Yes. O No. O Can't decide with information given. Headings
7:32 Blackboard × Read Only - Save a copy to edit. Predicting qualitatively how entropy changes with temperature and volume System 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. A few grams of acetone vapor ((CH3)₂CO). A few moles of helium (He) gas. A few moles of helium (He) gas. System 20. L of pure argon (Ar) gas and 20.0 L of pure krypton (Kr) gas, both at 1 atm and 44°C. Predicting qualitatively how entropy changes with mixing and separation A liter of seawater at 15°C. Change A 0.35 M solution of sucrose in water, and a beaker of pure water, both at 37.°C. The acetone condenses to a liquid at a constant temperature of -12.0 °C. Qualitatively predicting reaction entropy The helium is heated from -19.0 °C to 59.0 °C while the volume is held constant at 10.0 L. The helium is heated from 0.0 °C to 3.0 °C and is also compressed from a volume of 13.0 L to a volume of 10.0 L. The gases are mixed, with the pressure kept constant at 1 atm. The seawater is passed through a reverse-osmosis filter, which separates it into 750. mL of pure water and 250. mL of brine (very salty water). The solution is put into a semipermeable bag immersed in the water, and 50. mL of pure water flows through the bag into the sucrose solution. AS OAS < 0 O AS = 0 O AS > 0 not enough information O 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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. Change O OAS < 0 OAS=0 O AS > 0 O OAS < 0 O AS = 0 OAS 0 AS OAS < 0 OAS = 0 O AS> 0 not enough information ΤΟ ΔS < 0 OAS=0 O AS >0 not enough information not enough information OAS <0 OAS = 0 O AS> 0 not enough information .5Gc Save a copy not enough information || For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS If it's not possible to decide with the information given, check the "not enough information" button in the last column. rxn' Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal.
Transcribed Image Text:7:32 Blackboard × Read Only - Save a copy to edit. Predicting qualitatively how entropy changes with temperature and volume System 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. A few grams of acetone vapor ((CH3)₂CO). A few moles of helium (He) gas. A few moles of helium (He) gas. System 20. L of pure argon (Ar) gas and 20.0 L of pure krypton (Kr) gas, both at 1 atm and 44°C. Predicting qualitatively how entropy changes with mixing and separation A liter of seawater at 15°C. Change A 0.35 M solution of sucrose in water, and a beaker of pure water, both at 37.°C. The acetone condenses to a liquid at a constant temperature of -12.0 °C. Qualitatively predicting reaction entropy The helium is heated from -19.0 °C to 59.0 °C while the volume is held constant at 10.0 L. The helium is heated from 0.0 °C to 3.0 °C and is also compressed from a volume of 13.0 L to a volume of 10.0 L. The gases are mixed, with the pressure kept constant at 1 atm. The seawater is passed through a reverse-osmosis filter, which separates it into 750. mL of pure water and 250. mL of brine (very salty water). The solution is put into a semipermeable bag immersed in the water, and 50. mL of pure water flows through the bag into the sucrose solution. AS OAS < 0 O AS = 0 O AS > 0 not enough information O 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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. Change O OAS < 0 OAS=0 O AS > 0 O OAS < 0 O AS = 0 OAS 0 AS OAS < 0 OAS = 0 O AS> 0 not enough information ΤΟ ΔS < 0 OAS=0 O AS >0 not enough information not enough information OAS <0 OAS = 0 O AS> 0 not enough information .5Gc Save a copy not enough information || For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS If it's not possible to decide with the information given, check the "not enough information" button in the last column. rxn' Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal.
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