A 50.0 mL of 0.700 M copper (II) sulfate solution is added to a 50.00 mL of 1.00 M sodium hyroxide solution in a coffee cup calorimeter. The initial temperature of the two solutions is 22.5 °C and the highest temperature reached in the calorimeter after mixing is 25.7 °C. Assume that no heat is transferred to the calorimeter or the surroundings and that the heat capacity of the solutions is 4.18 J/g °C. Assume that density of each solution is 1.00 g/mL. Calculate the molar enthalpy change, in kJ/mol, for the precipitation reaction: CuSO4 (aq) +2 NaOH(aq) -----> Cu(OH)2 (s) + Na2SO4 (aq)
A 50.0 mL of 0.700 M copper (II) sulfate solution is added to a 50.00 mL of 1.00 M sodium hyroxide solution in a coffee cup calorimeter. The initial temperature of the two solutions is 22.5 °C and the highest temperature reached in the calorimeter after mixing is 25.7 °C. Assume that no heat is transferred to the calorimeter or the surroundings and that the heat capacity of the solutions is 4.18 J/g °C. Assume that density of each solution is 1.00 g/mL. Calculate the molar enthalpy change, in kJ/mol, for the precipitation reaction: CuSO4 (aq) +2 NaOH(aq) -----> Cu(OH)2 (s) + Na2SO4 (aq)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![A 50.0 mL of 0.700 M copper (II) sulfate solution is added to a 50.00 mL of 1.00 M
sodium hyroxide solution in a coffee cup calorimeter. The initial temperature of the
two solutions is 22.5 °C and the highest temperature reached in the calorimeter
after mixing is 25.7 °C. Assume that no heat is transferred to the calorimeter or
the surroundings and that the heat capacity of the solutions is 4.18 J/g °C.
Assume that density of each solution is 1.00 g/mL. Calculate the molar enthalpy
change, in kJ/mol, for the precipitation reaction:
CuSO4 (aq)
+2 NaOH(aq) -----> Cu(OH)2 (s) + Na2SO4 (aq)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50197843-120f-40bf-88bf-2951ca6216dd%2Fe2f4073f-8cd2-440b-a203-35df7da32c67%2Fck7vk7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 50.0 mL of 0.700 M copper (II) sulfate solution is added to a 50.00 mL of 1.00 M
sodium hyroxide solution in a coffee cup calorimeter. The initial temperature of the
two solutions is 22.5 °C and the highest temperature reached in the calorimeter
after mixing is 25.7 °C. Assume that no heat is transferred to the calorimeter or
the surroundings and that the heat capacity of the solutions is 4.18 J/g °C.
Assume that density of each solution is 1.00 g/mL. Calculate the molar enthalpy
change, in kJ/mol, for the precipitation reaction:
CuSO4 (aq)
+2 NaOH(aq) -----> Cu(OH)2 (s) + Na2SO4 (aq)
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