Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Dissolution of KBr in Water
**Concept: Enthalpy of Solution**
When solid KBr (Potassium Bromide) is dissolved in H₂O (Water), the process involves two main enthalpy changes:
- **ΔH₁: Enthalpy of Solute Dissociation**
\[ ΔH₁ = -690 \, \text{kJ/mol} \]
- **ΔH₂: Enthalpy of Solute-Solvent Interaction**
\[ ΔH₂ = +19.9 \, \text{kJ/mol} \]
The overall enthalpy change of the solution, noted as **ΔH_solution**, is the sum of these two enthalpies:
\[ \Delta H_{\text{solution}} = \Delta H_{1} + \Delta H_{2} \]
**Formula:**
\[ ΔH_{\text{solution}} = (-690 \, \text{kJ/mol}) + (19.9 \, \text{kJ/mol}) \]
**Instructions for Calculation:**
1. Substitute the given values into the formula.
2. Calculate the sum.
3. Enter the result in kilojoules per mole (kJ/mol) to the nearest ones place. For example, 45 kJ.
**Input Fields:**
- The **ΔH_solution** is \( \_\_\_\_\_\_ \text{kJ/mol} \)
- The solution is described as: **\[ \text{Exothermic}/\text{Endothermic} \]**
**Example Calculation:**
\[ \Delta H_{\text{solution}} = -690 + 19.9 = -670.1 \]
So, ΔH_solution is -670 kJ/mol.
**Type of Process:**
- If **ΔH_solution** is negative: The solution is **Exothermic**.
- If **ΔH_solution** is positive: The solution is **Endothermic**.
**Interactive Tool:**
Enter your calculated **ΔH_solution** to the ones place, e.g., 45 kJ, and select the correct description of the solution.](https://content.bartleby.com/qna-images/question/c25f84cd-37fe-4eda-bb3a-0db4abed4038/0340f699-2cae-432b-b425-104a6a1d1b72/k0hjyks_processed.jpeg)
Transcribed Image Text:### Dissolution of KBr in Water
**Concept: Enthalpy of Solution**
When solid KBr (Potassium Bromide) is dissolved in H₂O (Water), the process involves two main enthalpy changes:
- **ΔH₁: Enthalpy of Solute Dissociation**
\[ ΔH₁ = -690 \, \text{kJ/mol} \]
- **ΔH₂: Enthalpy of Solute-Solvent Interaction**
\[ ΔH₂ = +19.9 \, \text{kJ/mol} \]
The overall enthalpy change of the solution, noted as **ΔH_solution**, is the sum of these two enthalpies:
\[ \Delta H_{\text{solution}} = \Delta H_{1} + \Delta H_{2} \]
**Formula:**
\[ ΔH_{\text{solution}} = (-690 \, \text{kJ/mol}) + (19.9 \, \text{kJ/mol}) \]
**Instructions for Calculation:**
1. Substitute the given values into the formula.
2. Calculate the sum.
3. Enter the result in kilojoules per mole (kJ/mol) to the nearest ones place. For example, 45 kJ.
**Input Fields:**
- The **ΔH_solution** is \( \_\_\_\_\_\_ \text{kJ/mol} \)
- The solution is described as: **\[ \text{Exothermic}/\text{Endothermic} \]**
**Example Calculation:**
\[ \Delta H_{\text{solution}} = -690 + 19.9 = -670.1 \]
So, ΔH_solution is -670 kJ/mol.
**Type of Process:**
- If **ΔH_solution** is negative: The solution is **Exothermic**.
- If **ΔH_solution** is positive: The solution is **Endothermic**.
**Interactive Tool:**
Enter your calculated **ΔH_solution** to the ones place, e.g., 45 kJ, and select the correct description of the solution.
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