Problem 4. Calcium chloride is a salt used in a number of food and medicinal applications and in fluid for refrigeration systems. Its most distinctive property is its affinity for water: in its anhydrous form it efficiently absorbs water vapour from gases, and from aqueous liquid solutions it can form (under different conditions) calcium chloride hydrate (CaCl2-H20), dihydrate (CaCl2 2H2O), tetrahydrate (CaCl2-4H2O) and hexahydrate (CaCl2-6H2O). You have been given the task of determining the standard heat of of the reaction in which calcium chloride hexahydrate is formed from anhydrous calcium chloride: AH (k) ? CaCl2(s)6H20 CaCl2-6H20 (s) By definition, the desired quantity is the heat of hydration of calcium chloride hexahydrate. You cannot carry out the hydration reaction directly, so you resort to an indirect moethod. You first dissolve 1 mol of anhydrous (no water) CaCl2 in 10 mol of water in a calorimeter and determine that 64.85 kJ of heat must be transferred away from the calorimeter to keep the solution temperature at 25°C. You next dissolve 1 mol of the hexahydrate salt in 4 mol of water and find that 32.41 kJ of heat must be transferred to the calorimeter to keep the temperature at 25°C Use these results to calculate the desired heat of reaction (Hint: remember Hess' Law)
Problem 4. Calcium chloride is a salt used in a number of food and medicinal applications and in fluid for refrigeration systems. Its most distinctive property is its affinity for water: in its anhydrous form it efficiently absorbs water vapour from gases, and from aqueous liquid solutions it can form (under different conditions) calcium chloride hydrate (CaCl2-H20), dihydrate (CaCl2 2H2O), tetrahydrate (CaCl2-4H2O) and hexahydrate (CaCl2-6H2O). You have been given the task of determining the standard heat of of the reaction in which calcium chloride hexahydrate is formed from anhydrous calcium chloride: AH (k) ? CaCl2(s)6H20 CaCl2-6H20 (s) By definition, the desired quantity is the heat of hydration of calcium chloride hexahydrate. You cannot carry out the hydration reaction directly, so you resort to an indirect moethod. You first dissolve 1 mol of anhydrous (no water) CaCl2 in 10 mol of water in a calorimeter and determine that 64.85 kJ of heat must be transferred away from the calorimeter to keep the solution temperature at 25°C. You next dissolve 1 mol of the hexahydrate salt in 4 mol of water and find that 32.41 kJ of heat must be transferred to the calorimeter to keep the temperature at 25°C Use these results to calculate the desired heat of reaction (Hint: remember Hess' Law)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Transcribed Image Text:Problem 4.
Calcium chloride is a salt used in a number of food and medicinal applications and in fluid for
refrigeration systems. Its most distinctive property is its affinity for water: in its anhydrous form
it efficiently absorbs water vapour from gases, and from aqueous liquid solutions it can form
(under different conditions) calcium chloride hydrate (CaCl2-H20), dihydrate (CaCl2 2H2O),
tetrahydrate (CaCl2-4H2O) and hexahydrate (CaCl2-6H2O).
You have been given the task of determining the standard heat of of the reaction in which calcium
chloride hexahydrate is formed from anhydrous calcium chloride:
AH (k) ?
CaCl2(s)6H20 CaCl2-6H20 (s)
By definition, the desired quantity is the heat of hydration of calcium chloride hexahydrate. You
cannot carry out the hydration reaction directly, so you resort to an indirect moethod. You first
dissolve 1 mol of anhydrous (no water) CaCl2 in 10 mol of water in a calorimeter and determine
that 64.85 kJ of heat must be transferred away from the calorimeter to keep the solution
temperature at 25°C. You next dissolve 1 mol of the hexahydrate salt in 4 mol of water and find
that 32.41 kJ of heat must be transferred to the calorimeter to keep the temperature at 25°C
Use these results to calculate the desired heat of reaction (Hint: remember Hess' Law)
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