A 50.0-mL sample of a 1.00 M solution of is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 20.4 ∘C∘C before mixing and 26.3 ∘C∘C after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data calculate ΔH (in kJ/mol) for the process: CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M) Assume the specific heat and density of the solution after mixing are the same as those of pure water.
A 50.0-mL sample of a 1.00 M solution of is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 20.4 ∘C∘C before mixing and 26.3 ∘C∘C after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data calculate ΔH (in kJ/mol) for the process: CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M) Assume the specific heat and density of the solution after mixing are the same as those of pure water.
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 50.0-mL sample of a 1.00 M solution of is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 20.4 ∘C∘C before mixing and 26.3 ∘C∘C after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data calculate ΔH (in kJ/mol) for the process:
CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)
Assume the specific heat and density of the solution after mixing are the same as those of pure water.
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