Question 12 WA 5.00 g-sample of KOH(s) at 25.0°C was added to 100.0 g of H2O(1) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, thetemperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process?The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH < 0. Also, the ions become less dispersed as KOH(s) dissolves, thusAS >0. Therefore, AG < 0.less than that released as the ion-dipole attractions form during solvation, thus AH < 0. Also, the ions become moreThe energy required to break the bonds between the ions in the solidwidely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG < 0.The average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore. AG > 0.DThe average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS < 0. Therefore. AG > 0.escQ Search or enter website name@#$%&

Since temperature of the solution is increased means energy is released during dissolution process…

Question 12W A 5.00 g-sample of KOH(s) at 25.0 C was added to 100.0 g of H2O(1) temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process? room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus A AS >0. Therefore, AG < 0. The energy required to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus AH < 0. Also, the ions become more B widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG < 0. The average kinetic energy of the particles increases, resulting in AH >0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG > 0. The average kinetic energy of the particles increases, resulting in AH >0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS < 0. Therefore, AG > 0. D

Question 12W A 5.00 g-sample of KOH(s) at 25.0 C was added to 100.0 g of H2O(1) temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process? room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH < 0. Also, the ions become less dispersed as KOH(s) dissolves, thus A AS >0. Therefore, AG < 0. The energy required to break the bonds between the ions in the solid is less than that released as the ion-dipole attractions form during solvation, thus AH < 0. Also, the ions become more B widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG < 0. The average kinetic energy of the particles increases, resulting in AH >0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore, AG > 0. The average kinetic energy of the particles increases, resulting in AH >0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS < 0. Therefore, AG > 0. D

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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