A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 19.1 oC before mixing and 29.2 oC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔH for the process:
A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 19.1 oC before mixing and 29.2 oC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔH for the process:
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.2: Specific Heat Capacity: Heating And Cooling
Problem 5.1CYU: You did an experiment in which you found that 59.8 J was required to raise the temperature of 25.0 g...
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A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 19.1 oC before mixing and 29.2 oC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔH
for the process:
CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)
(Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.)
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