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

10th Edition

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

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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