Ch.6 - Thermochemistry WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Internal Energy
Calorimetry
Hess's Law
Enthalpy of Formation
End of Chapter 6 Problems
Additional Practice
Units of Energy
Endothermic & Exothermic Reactions
Additional Guides
Enthalpy

Solution: When a solid dissolves in water, heat may be evolved or absorbed. The  heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when  3.50 g of CuSO4 (s) are dissolved in 115.90 g of water, the temperature of the solution  increases from 24.19 to 27.48°C. The heat capacity of the calorimeter (sometimes referred to as the  calorimeter constant) was determined in a separate experiment to be 1.78 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of  CuSO4 (s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. 

Problem

When a solid dissolves in water, heat may be evolved or absorbed. The  heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. 

In the laboratory a general chemistry student finds that when  3.50 g of CuSO4 (s) are dissolved in 115.90 g of water, the temperature of the solution  increases from 24.19 to 27.48°C. 

The heat capacity of the calorimeter (sometimes referred to as the  calorimeter constant) was determined in a separate experiment to be 1.78 J/°C. 

Based on the student's observation, calculate the enthalpy of dissolution of  CuSO4 (s) in kJ/mol. 

Assume the specific heat of the solution is equal to the specific heat of water.