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Suggest some ways in which the calorimeter or lab protocol could be improved to have lower percentage of errors.

Suggest some ways in which the calorimeter or lab protocol could be improved to have lower percentage of errors.

Chemistry
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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  1. Suggest some ways in which the calorimeter or lab protocol could be improved to have lower percentage of errors.
**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) \[ΔT = Tf - Ti\] | 6 | 14 | 19 | -4 | -8 | -11 | | Heat absorbed by the solution (J) \[qₓ = \[-q⁰ₓ = -mcΔT\]\] | -125.5 | -585.8 | -1192.4 | 83.7 | 335.4 | 690.4 | | Heat Capacity of the Calorimeter (J/°C) \[C\] | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | | Heat absorbed by the calorimeter (J) \[qₑ = C x ΔT\] | 2510.4 | 5857.6 | 7949.6 | 1673.6 | 3347.2 | 4602.4 | | Enthalpy of solution
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) \[ΔT = Tf - Ti\] | 6 | 14 | 19 | -4 | -8 | -11 | | Heat absorbed by the solution (J) \[qₓ = \[-q⁰ₓ = -mcΔT\]\] | -125.5 | -585.8 | -1192.4 | 83.7 | 335.4 | 690.4 | | Heat Capacity of the Calorimeter (J/°C) \[C\] | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | 418.4 | | Heat absorbed by the calorimeter (J) \[qₑ = C x ΔT\] | 2510.4 | 5857.6 | 7949.6 | 1673.6 | 3347.2 | 4602.4 | | Enthalpy of solution
### Transcription for Educational Website #### Data Table | Mass (g) | CaCl₂ ΔT (°C) | NH₄Cl Mass (g) | NH₄Cl ΔT (°C) | |----------|--------------|----------------|--------------| | 5 | 6 | 5 | -4 | | 10.04 | 14 | 10.02 | -8 | | 15 | 19 | 15 | -11 | #### Graph Descriptions **Chart #1: Mass of CaCl₂ vs. ΔT** - **X-axis:** Mass of CaCl₂ (in grams) - **Y-axis:** Change in Temperature (ΔT, in °C) - **Description:** The chart presents a linear relationship between the mass of calcium chloride (CaCl₂) and the change in temperature (ΔT). - **Equation of the Line:** \( y = 1.3008x - 0.0251 \) - **Coefficient of Determination (R²):** 0.9837 - **Observation:** As the mass of CaCl₂ increases, the change in temperature also increases, indicating a direct proportionality. **Chart #2: Mass of NH₄Cl vs. ΔT** - **X-axis:** Mass of NH₄Cl (in grams) - **Y-axis:** Change in Temperature (ΔT, in °C) - **Description:** This chart displays a linear inverse relationship between the mass of ammonium chloride (NH₄Cl) and the change in temperature (ΔT). - **Equation of the Line:** \( y = -0.7001x - 0.6607 \) - **Coefficient of Determination (R²):** 0.9936 - **Observation:** As the mass of NH₄Cl increases, the change in temperature decreases, reflecting an inverse proportionality and indicating an endothermic reaction. #### Source Data provided by © 2016 Carolina Biological Supply Company.
Transcribed Image Text:### Transcription for Educational Website #### Data Table | Mass (g) | CaCl₂ ΔT (°C) | NH₄Cl Mass (g) | NH₄Cl ΔT (°C) | |----------|--------------|----------------|--------------| | 5 | 6 | 5 | -4 | | 10.04 | 14 | 10.02 | -8 | | 15 | 19 | 15 | -11 | #### Graph Descriptions **Chart #1: Mass of CaCl₂ vs. ΔT** - **X-axis:** Mass of CaCl₂ (in grams) - **Y-axis:** Change in Temperature (ΔT, in °C) - **Description:** The chart presents a linear relationship between the mass of calcium chloride (CaCl₂) and the change in temperature (ΔT). - **Equation of the Line:** \( y = 1.3008x - 0.0251 \) - **Coefficient of Determination (R²):** 0.9837 - **Observation:** As the mass of CaCl₂ increases, the change in temperature also increases, indicating a direct proportionality. **Chart #2: Mass of NH₄Cl vs. ΔT** - **X-axis:** Mass of NH₄Cl (in grams) - **Y-axis:** Change in Temperature (ΔT, in °C) - **Description:** This chart displays a linear inverse relationship between the mass of ammonium chloride (NH₄Cl) and the change in temperature (ΔT). - **Equation of the Line:** \( y = -0.7001x - 0.6607 \) - **Coefficient of Determination (R²):** 0.9936 - **Observation:** As the mass of NH₄Cl increases, the change in temperature decreases, reflecting an inverse proportionality and indicating an endothermic reaction. #### Source Data provided by © 2016 Carolina Biological Supply Company.
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