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CALCULATIONS/ RESULTS (Show work for Reaction A on the next page) Reaction A Reaction B Reaction C Mass of solution (g) Temperature Change (*C) Heat, q n, moles of NaOH AH (kJ/mol NaOH) Class Average, AH N2OH) (kl/mol YOUR ΔΗΑ + ΔΗ % error between YOUR (AHC) and (AH, + AHg). (use AHç as the "known" value) Classes' AH, + AH, % error between the classes' (AHC) and (AH, + AHs). (use AHc as the "known" value)

CALCULATIONS/ RESULTS (Show work for Reaction A on the next page) Reaction A Reaction B Reaction C Mass of solution (g) Temperature Change (*C) Heat, q n, moles of NaOH AH (kJ/mol NaOH) Class Average, AH N2OH) (kl/mol YOUR ΔΗΑ + ΔΗ % error between YOUR (AHC) and (AH, + AHg). (use AHç as the "known" value) Classes' AH, + AH, % error between the classes' (AHC) and (AH, + AHs). (use AHc as the "known" value)

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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You should compare your report data to documented heat of reaction data, to replace "Class Average"

### Calorimetry Experiment Data #### Mass Measurements - **Mass of empty calorimeter, lid and stir bar:** 85.62 g #### Reaction Data - **Reaction A:** - Mass of NaOH(s): 0.56 g - Mass of calorimeter with solution: 110.94 g - Initial temperature (T₁): 25.1°C - Final temperature (T₂): 29.7°C - **Reaction B:** - Mass of NaOH(s): 0.56 g - Mass of calorimeter with solution: 135.47 g - Initial temperature (T₁): 25.2°C - Final temperature (T₂): 28.6°C - **Reaction C:** - Mass of NaOH(s): 0.49 g - Mass of calorimeter with solution: 135.65 g - Initial temperature (T₁): 24.8°C - Final temperature (T₂): 30.0°C ### Explanation of Data This table summarizes the experimental data for three separate reactions (A, B, and C) using a calorimeter. The masses of NaOH(s), calorimeter with solution, and the initial and final temperatures of the reactions are recorded. This data is crucial for calculating the enthalpy changes of the reactions. To comprehensively analyze the reactions, you might explore: - The calculation of the temperature change (ΔT) for each reaction. - The determination of the heat absorbed or released using the formula \( q = mc\Delta T \), where \( m \) is mass, \( c \) is specific heat capacity, and \( \Delta T \) is the change in temperature. - Understanding the differences in heat transfer and energy changes among the three reactions based on the given measurements.
Transcribed Image Text:### Calorimetry Experiment Data #### Mass Measurements - **Mass of empty calorimeter, lid and stir bar:** 85.62 g #### Reaction Data - **Reaction A:** - Mass of NaOH(s): 0.56 g - Mass of calorimeter with solution: 110.94 g - Initial temperature (T₁): 25.1°C - Final temperature (T₂): 29.7°C - **Reaction B:** - Mass of NaOH(s): 0.56 g - Mass of calorimeter with solution: 135.47 g - Initial temperature (T₁): 25.2°C - Final temperature (T₂): 28.6°C - **Reaction C:** - Mass of NaOH(s): 0.49 g - Mass of calorimeter with solution: 135.65 g - Initial temperature (T₁): 24.8°C - Final temperature (T₂): 30.0°C ### Explanation of Data This table summarizes the experimental data for three separate reactions (A, B, and C) using a calorimeter. The masses of NaOH(s), calorimeter with solution, and the initial and final temperatures of the reactions are recorded. This data is crucial for calculating the enthalpy changes of the reactions. To comprehensively analyze the reactions, you might explore: - The calculation of the temperature change (ΔT) for each reaction. - The determination of the heat absorbed or released using the formula \( q = mc\Delta T \), where \( m \) is mass, \( c \) is specific heat capacity, and \( \Delta T \) is the change in temperature. - Understanding the differences in heat transfer and energy changes among the three reactions based on the given measurements.
### CALCULATIONS/ RESULTS (Show work for Reaction A on the next page) | | Reaction A | Reaction B | Reaction C | |----------------------------|------------|------------|------------| | **Mass of solution (g)** | __________ | __________ | __________ | | **Temperature Change (°C)**| __________ | __________ | __________ | | **Heat, q** | __________ | __________ | __________ | | **n, moles of NaOH** | __________ | __________ | __________ | | **ΔH (kJ/mol NaOH)** | __________ | __________ | __________ | | **Class Average, ΔH (kJ/mol NaOH)** | __________ | __________ | __________ | **YOUR ΔH<sub>A</sub> + ΔH<sub>B</sub>** _________________ **% error between YOUR (ΔH<sub>C</sub>) and (ΔH<sub>A</sub> + ΔH<sub>B</sub>)** (use ΔH<sub>C</sub> as the “known” value) _________________ **Classes' ΔH<sub>A</sub> + ΔH<sub>B</sub>** _________________ **% error between the classes' (ΔH<sub>C</sub>) and (ΔH<sub>A</sub> + ΔH<sub>B</sub>)** (use ΔH<sub>C</sub> as the “known” value) _________________ This table is structured to help students document and calculate various thermodynamic properties of three different reactions: A, B, and C, during their lab experiments. 1. **Mass of Solution (g):** The mass of the solution used in each reaction should be recorded here. 2. **Temperature Change (°C):** The change in temperature observed during the reaction. 3. **Heat, q:** The heat absorbed or released during the reaction. 4. **n, moles of NaOH:** The amount of sodium hydroxide involved in the reaction. 5. **ΔH (kJ/mol NaOH):** The enthalpy change per mole of NaOH. 6. **Class Average, ΔH (kJ/mol NaOH):** The average ΔH calculated from the class data. Following the tabulated data: - Students are asked to sum their calculated enthalpies for reactions A and B. - They then calculate the percentage error between their summed enthalpy (
Transcribed Image Text:### CALCULATIONS/ RESULTS (Show work for Reaction A on the next page) | | Reaction A | Reaction B | Reaction C | |----------------------------|------------|------------|------------| | **Mass of solution (g)** | __________ | __________ | __________ | | **Temperature Change (°C)**| __________ | __________ | __________ | | **Heat, q** | __________ | __________ | __________ | | **n, moles of NaOH** | __________ | __________ | __________ | | **ΔH (kJ/mol NaOH)** | __________ | __________ | __________ | | **Class Average, ΔH (kJ/mol NaOH)** | __________ | __________ | __________ | **YOUR ΔH<sub>A</sub> + ΔH<sub>B</sub>** _________________ **% error between YOUR (ΔH<sub>C</sub>) and (ΔH<sub>A</sub> + ΔH<sub>B</sub>)** (use ΔH<sub>C</sub> as the “known” value) _________________ **Classes' ΔH<sub>A</sub> + ΔH<sub>B</sub>** _________________ **% error between the classes' (ΔH<sub>C</sub>) and (ΔH<sub>A</sub> + ΔH<sub>B</sub>)** (use ΔH<sub>C</sub> as the “known” value) _________________ This table is structured to help students document and calculate various thermodynamic properties of three different reactions: A, B, and C, during their lab experiments. 1. **Mass of Solution (g):** The mass of the solution used in each reaction should be recorded here. 2. **Temperature Change (°C):** The change in temperature observed during the reaction. 3. **Heat, q:** The heat absorbed or released during the reaction. 4. **n, moles of NaOH:** The amount of sodium hydroxide involved in the reaction. 5. **ΔH (kJ/mol NaOH):** The enthalpy change per mole of NaOH. 6. **Class Average, ΔH (kJ/mol NaOH):** The average ΔH calculated from the class data. Following the tabulated data: - Students are asked to sum their calculated enthalpies for reactions A and B. - They then calculate the percentage error between their summed enthalpy (
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