When 2.53 g of CaCl2 was dissolved in 30.00 g of water in an adiabatic calorimeter at 23.0°C, the temperature of the solution went up to 36.5°C. Find ΔH (in kJ/mol) for the dissolution of one mole of CaCl2 in water. (The molar mass of CaCl2 is 110.978 g/mol.)
When 2.53 g of CaCl2 was dissolved in 30.00 g of water in an adiabatic calorimeter at 23.0°C, the temperature of the solution went up to 36.5°C. Find ΔH (in kJ/mol) for the dissolution of one mole of CaCl2 in water. (The molar mass of CaCl2 is 110.978 g/mol.)
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 82AE: Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the...
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When 2.53 g of CaCl2 was dissolved in 30.00 g of water in an adiabatic calorimeter at 23.0°C, the temperature of the solution went up to 36.5°C.
Find ΔH (in kJ/mol) for the dissolution of one mole of CaCl2 in water. (The molar mass of CaCl2 is 110.978 g/mol.)
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