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PART II. PROBLEM SOLVING A student was asked to determine the enthalpy of solution of KCIO, in water us Styrofoam calorimetry. Calibration was performed by mixing 8.00 mL 0.050 M H with 2.00 mL 0.200 M NaOH. The neutralization reaction (AH = -55.85 kJ/mol) w accompanied by a temperature change from 25.0 to 28.3°C. Using the sal calorimeter, 0.300 g KCIO3 (MW: 122.55) was dissolved in water and temperature was observed to change from 23.6 to 17.3°C. (Assume that the to volume of the mixture in calibration is the same in the enthalpy measurement) %3D A. What is the calorimeter constant? B. What is the enthalpy of dissolution of KCIO3 in kJ/mol? C. Is the dissolution endothermic or exothermic? Explain.

PART II. PROBLEM SOLVING A student was asked to determine the enthalpy of solution of KCIO, in water us Styrofoam calorimetry. Calibration was performed by mixing 8.00 mL 0.050 M H with 2.00 mL 0.200 M NaOH. The neutralization reaction (AH = -55.85 kJ/mol) w accompanied by a temperature change from 25.0 to 28.3°C. Using the sal calorimeter, 0.300 g KCIO3 (MW: 122.55) was dissolved in water and temperature was observed to change from 23.6 to 17.3°C. (Assume that the to volume of the mixture in calibration is the same in the enthalpy measurement) %3D A. What is the calorimeter constant? B. What is the enthalpy of dissolution of KCIO3 in kJ/mol? C. Is the dissolution endothermic or exothermic? Explain.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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PART II. PROBLEM SOLVING A student was asked to determine the enthalpy of solution of KCIO, in water using Styrofoam calorimetry. Calibration was performed by mixing 8.00 mL 0.050 M HCI with 2.00 mL 0.200 M NaOH. The neutralization reaction (AH = -55.85 kJ/mol) was accompanied by a temperature change from 25.0 to 28.3°C. Using the same calorimeter, 0.300 g KCIO3 (MW: 122.55) was dissolved in water and the temperature was observed to change from 23.6 to 17.3°C. (Assume that the total volume of the mixture in calibration is the same in the enthalpy measurement) A. What is the calorimeter constant? B. What is the enthalpy of dissolution of KCIO3 in kJ/mol? C. Is the dissolution endothermic or exothermic? Explain.
Transcribed Image Text:PART II. PROBLEM SOLVING A student was asked to determine the enthalpy of solution of KCIO, in water using Styrofoam calorimetry. Calibration was performed by mixing 8.00 mL 0.050 M HCI with 2.00 mL 0.200 M NaOH. The neutralization reaction (AH = -55.85 kJ/mol) was accompanied by a temperature change from 25.0 to 28.3°C. Using the same calorimeter, 0.300 g KCIO3 (MW: 122.55) was dissolved in water and the temperature was observed to change from 23.6 to 17.3°C. (Assume that the total volume of the mixture in calibration is the same in the enthalpy measurement) A. What is the calorimeter constant? B. What is the enthalpy of dissolution of KCIO3 in kJ/mol? C. Is the dissolution endothermic or exothermic? Explain.
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