1 Consider the process by which potassium sulfate dissolves in water and dissociates into its individual ions a Write a balanced equation for this process, indicating all relevant phases b Using values from Appendix 4 in your textbook, calculate the standard enthalpy change associated with this process Gas a Molar Mass (g mol) Delta H S Delta G page APP 18 H 2 O 18 015 285 8 69 9 273 2 c If the potassium sulfate comes out of the drying oven at a temperature of 68 75C and is immediately mixed into a beaker of water at 18 50C, will its dissolution be spontaneous Please provide relevant work to support your answer d What is the change in Gibbs free energy for the dissolution described in part c

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Question: 1.Consider the process by which potassium sulfate dissolves in water and dissociates into its individual ions. a. Write a balanced equation for this process, indicating

1.Consider the process by which potassium sulfate dissolves in water and dissociates into its individual ions.

a. Write a balanced equation for this process, indicating all relevant phases.

b. Using values from Appendix 4 in your textbook, calculate the standard enthalpy change associated with this process.

Gas^a

Molar Mass (g/mol)

Delta H

Delta G

page APP-18

H₂O

18.015

-285.8

69.9

-273.2

c. If the potassium sulfate comes out of the drying oven at a temperature of 68.75C and is immediately mixed into a beaker of water at 18.50C, will its dissolution be spontaneous? Please provide relevant work to support your answer.

d. What is the change in Gibbs free energy for the dissolution described in part c?

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