Hand Warmer Chemistry Lab Report
Investigation 12:
Using Thermodynamic Quantities Through Calorimetry to Determine the Ideal Compound for Hand warmer
Author: Jane Kim (B2)
Partners: Jenny Kim, Jeffrey Heo, Eugenia Lee
Experiment date: March 2, 2017 Table of Contents
1. Abstract 3
2. Introduction 3
3. Experimental details 4
3-1. Materials 4
3-2. Apparatus 7
3-3. Procedure 7
3-4. Special Precautions 8
3-5. Lab techniques 9
4. Results 9
5. Discussion 14
6. Conclusion 16
7. References 17
1. Abstract
This lab report discusses an experiment to study thermodynamics and find ideal ionic compound to be used in hand warmer. Calorimetry experiment was conducted by dissolving three ionic compounds, CaCl2, Na2CO3, and NaCl, in distilled water to measure the enthalpy of solution. …show more content…
The broader objective is to study thermodynamics, a study of energy and its interconversion. Three main quantities of thermodynamic — enthalpy, entropy, and Gibbs free energy — was investigated for process of dissolving various ionic compounds in water. Calorimetry lab was conducted using 3 different ionic solids, CaCl2, Na2CO3, and NaCl, to calculate heat (symbolized as q) of reaction when these solids were each dissolved in distilled water. Calorimetry is technique used to experimentally measure the heat change with any process using a calorimeter, an insulated device that prevents heat flow between the vessel and the surrounding (S. Zumdahl and A. Zumdahl 254). By observing change in temperature of the system after the compound was dissolved, relationship between bond formation and energy was studied. In making a solution, the difference between energy released when the bonds of solute and solvent break and energy absorbed when solute particles and solvent particles interact to form solution determines the overall change in enthalpy of that reaction. Enthalpy refers to the total heat content a given system has. Ionic compounds with greatest negative change …show more content…
Characteristics of three ionic solid species
Compound
Formular
Characterization
Molecular Weight (g/mol)
Calcium chloride
CaCl2
Calcium chloride is an ionic salt, and metal halide. It is white crystalline solid at room temperature, with high solubility to water (Pubchem). CaCl2 used for this experiment were in beads form of approximately 10 mesh.
110.978
Sodium carbonate
Na2CO3
Sodium carbonate is a sodium salt, and metal carbonate, that is water-soluble. It most commonly occurs as white hygroscopic powder (Pubchem).
105.988
Sodium chloride
NaCl
Sodium chloride is an ionic salt, and metal halide. It is crystalline white solid at room temperature (Pubchem). NaCl used in this lab were in fine powder form.
58.44
3-2. Apparatus
3-3. Procedure
150.0mL of distilled water was poured into the calorimeter using the 100.0mL and 50.0mL graduated cylinders.
The magnetic stirrer and thermometer were placed in calorimeter until temperature was stabilized
Initial temperature of the water was recorded.
The thermometer was removed.
The calorimeter was placed on the magnetic stirring
Using Thermodynamic Quantities Through Calorimetry to Determine the Ideal Compound for Hand warmer
Author: Jane Kim (B2)
Partners: Jenny Kim, Jeffrey Heo, Eugenia Lee
Experiment date: March 2, 2017 Table of Contents
1. Abstract 3
2. Introduction 3
3. Experimental details 4
3-1. Materials 4
3-2. Apparatus 7
3-3. Procedure 7
3-4. Special Precautions 8
3-5. Lab techniques 9
4. Results 9
5. Discussion 14
6. Conclusion 16
7. References 17
1. Abstract
This lab report discusses an experiment to study thermodynamics and find ideal ionic compound to be used in hand warmer. Calorimetry experiment was conducted by dissolving three ionic compounds, CaCl2, Na2CO3, and NaCl, in distilled water to measure the enthalpy of solution. …show more content…
The broader objective is to study thermodynamics, a study of energy and its interconversion. Three main quantities of thermodynamic — enthalpy, entropy, and Gibbs free energy — was investigated for process of dissolving various ionic compounds in water. Calorimetry lab was conducted using 3 different ionic solids, CaCl2, Na2CO3, and NaCl, to calculate heat (symbolized as q) of reaction when these solids were each dissolved in distilled water. Calorimetry is technique used to experimentally measure the heat change with any process using a calorimeter, an insulated device that prevents heat flow between the vessel and the surrounding (S. Zumdahl and A. Zumdahl 254). By observing change in temperature of the system after the compound was dissolved, relationship between bond formation and energy was studied. In making a solution, the difference between energy released when the bonds of solute and solvent break and energy absorbed when solute particles and solvent particles interact to form solution determines the overall change in enthalpy of that reaction. Enthalpy refers to the total heat content a given system has. Ionic compounds with greatest negative change …show more content…
Characteristics of three ionic solid species
Compound
Formular
Characterization
Molecular Weight (g/mol)
Calcium chloride
CaCl2
Calcium chloride is an ionic salt, and metal halide. It is white crystalline solid at room temperature, with high solubility to water (Pubchem). CaCl2 used for this experiment were in beads form of approximately 10 mesh.
110.978
Sodium carbonate
Na2CO3
Sodium carbonate is a sodium salt, and metal carbonate, that is water-soluble. It most commonly occurs as white hygroscopic powder (Pubchem).
105.988
Sodium chloride
NaCl
Sodium chloride is an ionic salt, and metal halide. It is crystalline white solid at room temperature (Pubchem). NaCl used in this lab were in fine powder form.
58.44
3-2. Apparatus
3-3. Procedure
150.0mL of distilled water was poured into the calorimeter using the 100.0mL and 50.0mL graduated cylinders.
The magnetic stirrer and thermometer were placed in calorimeter until temperature was stabilized
Initial temperature of the water was recorded.
The thermometer was removed.
The calorimeter was placed on the magnetic stirring