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General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.30QP: Enthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room...
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Help with questions 2-3 on work sheet using data please
Questions: You may have noticed that you can dissolve more sugar or table salt in hot water than in cold water. This is because the solubility of these substance increases with temperature. But is it always true that solubility increases with temperature? 1. Is KCl more soluble in hot or cold water? Is this reaction endothermic or exothermic? (See information in step #12) More soluble in cold water. Endothermic 2. Is Ce2(SO4)3 more soluble in hot or cold water? Is this reaction endothermic or exothermic? ore Soluble in hot watir. 3. Can you hypothesize a relationship between endo/exothermicity and the dependence of solubility on temperature based on the results of Parts One and Two?
Transcribed Image Text:Questions: You may have noticed that you can dissolve more sugar or table salt in hot water than in cold water. This is because the solubility of these substance increases with temperature. But is it always true that solubility increases with temperature? 1. Is KCl more soluble in hot or cold water? Is this reaction endothermic or exothermic? (See information in step #12) More soluble in cold water. Endothermic 2. Is Ce2(SO4)3 more soluble in hot or cold water? Is this reaction endothermic or exothermic? ore Soluble in hot watir. 3. Can you hypothesize a relationship between endo/exothermicity and the dependence of solubility on temperature based on the results of Parts One and Two?
BE SURE TO SET THE THERMAL PROPERTIES TO INSULATED SURROUNDINGS. 11. Start by placing 100 mL of water in a beaker and record the starting temperature. 12. Add 20 grams of the KCI, wait until it is dissolved, then record the new temperature. When salts dissolve, energy is always absorbed or released. When energy is absorbed the solution gets colder - this is an endothermic reaction. When energy is released the solution gets warmer - this is an exothermic reaction. 13. Repeat the experiment with the Ce2(SO4)3 using the second beaker. Add the same amount and record the new temperature. 14. Dissolving potassium chlorate (KCIO3) is even more endothermic than potassium chloride. Your final task is to determine how many grams of potassium chlorate you would have to add to 100 mL of water to produce the same temperature change as 5 grams of KCI. Data: Part One 35.7865g : @80°C = 46.52039g Mass of KCI Dissolved: @25°C = Mass of Ce2(SO4)3 Dissolved: @25°C = 6.Z1 957 g; @80°C = 0.919 45 g Part Two New Temperature After Dissolving 20 grams of solid in 100 mL of water: KCI = 1.54 °C; Ce2(SO4)3= 28.44°C Part Three Grams of KCIO3 Needed: 2.
Transcribed Image Text:BE SURE TO SET THE THERMAL PROPERTIES TO INSULATED SURROUNDINGS. 11. Start by placing 100 mL of water in a beaker and record the starting temperature. 12. Add 20 grams of the KCI, wait until it is dissolved, then record the new temperature. When salts dissolve, energy is always absorbed or released. When energy is absorbed the solution gets colder - this is an endothermic reaction. When energy is released the solution gets warmer - this is an exothermic reaction. 13. Repeat the experiment with the Ce2(SO4)3 using the second beaker. Add the same amount and record the new temperature. 14. Dissolving potassium chlorate (KCIO3) is even more endothermic than potassium chloride. Your final task is to determine how many grams of potassium chlorate you would have to add to 100 mL of water to produce the same temperature change as 5 grams of KCI. Data: Part One 35.7865g : @80°C = 46.52039g Mass of KCI Dissolved: @25°C = Mass of Ce2(SO4)3 Dissolved: @25°C = 6.Z1 957 g; @80°C = 0.919 45 g Part Two New Temperature After Dissolving 20 grams of solid in 100 mL of water: KCI = 1.54 °C; Ce2(SO4)3= 28.44°C Part Three Grams of KCIO3 Needed: 2.
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