Which salt did you test Ammonium nitrate Endothermic Salt Trial 1 Mass of Salt Used (g) Moles of Salt Used 6.240 Cs = 4.18 Initial Temperature (°C) Final Temperature (°C) AT = Tf-T₁ *asoln () (see note below table) 9rxn (1) AH (KJ/mol salt) Average AH (kJ/mol salt) *asoln = m* Cs* AT where m = mass in grams of water + salt J 9°C 19.7 15.2 -4.5 the same value as water Trial 2 8.01 19.6 14.3 -5.3
Which salt did you test Ammonium nitrate Endothermic Salt Trial 1 Mass of Salt Used (g) Moles of Salt Used 6.240 Cs = 4.18 Initial Temperature (°C) Final Temperature (°C) AT = Tf-T₁ *asoln () (see note below table) 9rxn (1) AH (KJ/mol salt) Average AH (kJ/mol salt) *asoln = m* Cs* AT where m = mass in grams of water + salt J 9°C 19.7 15.2 -4.5 the same value as water Trial 2 8.01 19.6 14.3 -5.3
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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Please help me complete the chart with the information provided. The mass of water in the Calorimeter is 100 mL.
![### Endothermic Reaction Experiment: Ammonium Nitrate
This educational page provides details from an experiment designed to measure the enthalpy change of an endothermic reaction, specifically the dissolution of ammonium nitrate in water.
#### Experiment Data
| Endothermic Salt | Trial 1 | Trial 2 |
|--------------------------|---------|---------|
| **Mass of Salt Used (g)**| 6.240 | 8.01 |
| **Moles of Salt Used** | | |
| **Initial Temperature (°C)** | 19.7 | 19.6 |
| **Final Temperature (°C)** | 15.2 | 14.3 |
| **ΔT = Tₜ - Tᵢ (°C)** | -4.5 | -5.3 |
| **qₛₒₗₙ (J)** (see note below table) | | |
| **qᵣₓₙ (J)** | | |
| **ΔH (kJ/mol salt)** | | |
| **Average ΔH (kJ/mol salt)** | | |
**Notes:**
- **qₛₒₗₙ (J)**: Calculated using the formula:
\[ qₛₒₗₙ = m \cdot Cₛ \cdot ΔT \]
where \( m \) is the mass in grams of water + salt,
\( Cₛ \) is the specific heat capacity of the solution (assumed to be the same as water, \( 4.18 \, \frac{J}{g°C} \)),
and \( ΔT \) is the change in temperature.
For example:
\[ qₛₒₗₙ^{\text{Trial 1}} = (mass_{solution}) \times 4.18 \times (-4.5) \]
\[ qₛₒₗₙ^{\text{Trial 2}} = (mass_{solution}) \times 4.18 \times (-5.3) \]
This data will help in determining the amount of heat absorbed by the solution (qₛₒₗₙ) and deducing the enthalpy change for the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0f317602-d71b-43c2-a09e-18efcd1b53db%2Fd1936317-28a1-4c39-9515-3ca0c55394c3%2F1wopyrg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Endothermic Reaction Experiment: Ammonium Nitrate
This educational page provides details from an experiment designed to measure the enthalpy change of an endothermic reaction, specifically the dissolution of ammonium nitrate in water.
#### Experiment Data
| Endothermic Salt | Trial 1 | Trial 2 |
|--------------------------|---------|---------|
| **Mass of Salt Used (g)**| 6.240 | 8.01 |
| **Moles of Salt Used** | | |
| **Initial Temperature (°C)** | 19.7 | 19.6 |
| **Final Temperature (°C)** | 15.2 | 14.3 |
| **ΔT = Tₜ - Tᵢ (°C)** | -4.5 | -5.3 |
| **qₛₒₗₙ (J)** (see note below table) | | |
| **qᵣₓₙ (J)** | | |
| **ΔH (kJ/mol salt)** | | |
| **Average ΔH (kJ/mol salt)** | | |
**Notes:**
- **qₛₒₗₙ (J)**: Calculated using the formula:
\[ qₛₒₗₙ = m \cdot Cₛ \cdot ΔT \]
where \( m \) is the mass in grams of water + salt,
\( Cₛ \) is the specific heat capacity of the solution (assumed to be the same as water, \( 4.18 \, \frac{J}{g°C} \)),
and \( ΔT \) is the change in temperature.
For example:
\[ qₛₒₗₙ^{\text{Trial 1}} = (mass_{solution}) \times 4.18 \times (-4.5) \]
\[ qₛₒₗₙ^{\text{Trial 2}} = (mass_{solution}) \times 4.18 \times (-5.3) \]
This data will help in determining the amount of heat absorbed by the solution (qₛₒₗₙ) and deducing the enthalpy change for the
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