The actual molar enthalpy of solution for calcium chloride is -81.3 kJ/mol, whereas the molar enthalpy of solution of ammonium chloride is 14.8 kJ/mol. Calculate the average molar enthalpy of solution for each chemical based on your data, and then calculate the percentage error for each.
The actual molar enthalpy of solution for calcium chloride is -81.3 kJ/mol, whereas the molar enthalpy of solution of ammonium chloride is 14.8 kJ/mol. Calculate the average molar enthalpy of solution for each chemical based on your data, and then calculate the percentage error for each.
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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- The actual molar enthalpy of solution for calcium chloride is -81.3 kJ/mol, whereas the molar enthalpy of solution of ammonium chloride is 14.8 kJ/mol.
Calculate the average molar enthalpy of solution for each chemical based on your data, and then calculate the percentage error for each.
Percent error is (|Actual – Experimental|/Actual) * 100%
![**Table of Data:**
- **Mass of CaCl₂ (grams):**
- 5
- 10.04
- 15
- **ΔT for CaCl₂ (degrees):**
- 6
- 14
- 19
- **Mass of NH₄Cl (grams):**
- 5
- 10.02
- 15
- **ΔT for NH₄Cl (degrees):**
- -4
- -8
- -11
**Graphs Explanation:**
**Chart #1:**
- **X-axis:** Mass of CaCl₂ (grams)
- **Y-axis:** ΔT for CaCl₂ (degrees)
- The graph shows a positive linear relationship between the mass of CaCl₂ and ΔT.
- The line of best fit has the equation:
\[ y = 1.3008x - 0.0251 \]
- The coefficient of determination, \( R^2 = 0.9837 \), indicates a very strong correlation.
**Chart #2:**
- **X-axis:** Mass of NH₄Cl (grams)
- **Y-axis:** ΔT for NH₄Cl (degrees)
- The graph shows a negative linear relationship between the mass of NH₄Cl and ΔT.
- The line of best fit has the equation:
\[ y = -0.7001x - 0.6607 \]
- The coefficient of determination, \( R^2 = 0.9936 \), indicates a very strong correlation.
**Conclusion:**
The data indicates that as the mass of CaCl₂ increases, the temperature change (ΔT) increases, suggesting an exothermic reaction. Conversely, as the mass of NH₄Cl increases, the temperature change (ΔT) decreases, suggesting an endothermic reaction.
*© 2016 Carolina Biological Supply Company*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa4431abc-b804-490c-9182-b6054ed16985%2F3baa0d55-22b2-4579-a592-b9333328a1b4%2Fsjrlu6p.jpeg&w=3840&q=75)
Transcribed Image Text:**Table of Data:**
- **Mass of CaCl₂ (grams):**
- 5
- 10.04
- 15
- **ΔT for CaCl₂ (degrees):**
- 6
- 14
- 19
- **Mass of NH₄Cl (grams):**
- 5
- 10.02
- 15
- **ΔT for NH₄Cl (degrees):**
- -4
- -8
- -11
**Graphs Explanation:**
**Chart #1:**
- **X-axis:** Mass of CaCl₂ (grams)
- **Y-axis:** ΔT for CaCl₂ (degrees)
- The graph shows a positive linear relationship between the mass of CaCl₂ and ΔT.
- The line of best fit has the equation:
\[ y = 1.3008x - 0.0251 \]
- The coefficient of determination, \( R^2 = 0.9837 \), indicates a very strong correlation.
**Chart #2:**
- **X-axis:** Mass of NH₄Cl (grams)
- **Y-axis:** ΔT for NH₄Cl (degrees)
- The graph shows a negative linear relationship between the mass of NH₄Cl and ΔT.
- The line of best fit has the equation:
\[ y = -0.7001x - 0.6607 \]
- The coefficient of determination, \( R^2 = 0.9936 \), indicates a very strong correlation.
**Conclusion:**
The data indicates that as the mass of CaCl₂ increases, the temperature change (ΔT) increases, suggesting an exothermic reaction. Conversely, as the mass of NH₄Cl increases, the temperature change (ΔT) decreases, suggesting an endothermic reaction.
*© 2016 Carolina Biological Supply Company*
Transcribed Image Text:**Data Table 2**
| | 5g CaCl₂ | 10g CaCl₂ | 15g CaCl₂ | 5g NH₄Cl | 10g NH₄Cl | 15g NH₄Cl |
|-----------|----------|-----------|-----------|----------|-----------|-----------|
| **Mass of water (g)** | 100 | 100 | 100 | 100 | 100 | 100 |
| **Mass of salt (g)** | 5.0 | 10.04 | 15.0 | 5.0 | 10.02 | 15.0 |
| **Moles of salt (g x mol/g)** | 0.045 | 0.090 | 0.135 | 0.093 | 0.187 | 0.280 |
| **Initial Temperature (°C)** | 23 | 23 | 23 | 23 | 23 | 23 |
| **Final Temperature (°C)** | 29 | 37 | 42 | 19 | 15 | 12 |
| **Change in Temperature (°C)** | 6 | 14 | 19 | -4 | -8 | -11 |
| **Heat absorbed by the solution (J)** | -125.5 | -585.8 | -1192.4 | 83.7 | 335.4 | 690.4 |
| **Heat Capacity of the Calorimeter (J/°C)** | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 |
| **Heat absorbed by the calorimeter (J)** | 2510.4 | 5857.6 | 7949.6 | 1673.6 | 3347.2 | 4602.4 |
| **Enthalpy of solution (J)** | -2384.9 | -5271.8 | -6820.2 | 1589.9 | 3011.8 | 391
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