**Chemical Reaction and Energy Calculation in Solutions** **Chemical Equation:** \[ \text{3 NaOH}_{(aq)} + \text{H}_3\text{PO}_4_{(aq)} \rightarrow \text{Na}_3\text{PO}_3_{(aq)} + \text{3 H}_2\text{O}_{(l)} \] \[ \Delta H = -173.7 \, \text{kJ} \] --- **1. Heat Produced Calculation** If 31.2 mL of 0.45 M sodium hydroxide is mixed with 65.4 mL of 0.088 M phosphoric acid, how many kJ of heat are produced? **Solution:** - Moles of sodium hydroxide: \[ 31.2 \, \text{mL} \times 0.45 \, \text{M} = 0.0140 \, \text{mol} \] - Moles of phosphoric acid: \[ 65.4 \, \text{mL} \times 0.088 \, \text{M} = 0.00575 \, \text{mol} \] - Limiting reagent: Phosphoric acid (0.00575 mol) is the limiting reagent. - Heat Calculation: \[ 0.00575 \, \text{mol} \times (-173.7 \, \text{kJ/mol}) = -1 \, \text{kJ} \] --- **2. Expected Final Temperature** When the solutions are mixed, what final temperature should we expect the solution to reach? Assume the combined solution has the same density (1 g/mL) and heat capacity (4.184 J/g°C) as water and that it is initially at 22.4 °C. - Use the equation for heat transfer: \[ q = m \cdot c \cdot \Delta T \] Where \( q \) is the heat change, \( m \) is the mass, \( c \) is the heat capacity, and \( \Delta T \) is the change in temperature. --- **3. Experimental Observations** Notice that for Part A of this lab, the temperature of the system and the surroundings both increased; however, for Part B, the temperature of the system decreased while that of
**Chemical Reaction and Energy Calculation in Solutions** **Chemical Equation:** \[ \text{3 NaOH}_{(aq)} + \text{H}_3\text{PO}_4_{(aq)} \rightarrow \text{Na}_3\text{PO}_3_{(aq)} + \text{3 H}_2\text{O}_{(l)} \] \[ \Delta H = -173.7 \, \text{kJ} \] --- **1. Heat Produced Calculation** If 31.2 mL of 0.45 M sodium hydroxide is mixed with 65.4 mL of 0.088 M phosphoric acid, how many kJ of heat are produced? **Solution:** - Moles of sodium hydroxide: \[ 31.2 \, \text{mL} \times 0.45 \, \text{M} = 0.0140 \, \text{mol} \] - Moles of phosphoric acid: \[ 65.4 \, \text{mL} \times 0.088 \, \text{M} = 0.00575 \, \text{mol} \] - Limiting reagent: Phosphoric acid (0.00575 mol) is the limiting reagent. - Heat Calculation: \[ 0.00575 \, \text{mol} \times (-173.7 \, \text{kJ/mol}) = -1 \, \text{kJ} \] --- **2. Expected Final Temperature** When the solutions are mixed, what final temperature should we expect the solution to reach? Assume the combined solution has the same density (1 g/mL) and heat capacity (4.184 J/g°C) as water and that it is initially at 22.4 °C. - Use the equation for heat transfer: \[ q = m \cdot c \cdot \Delta T \] Where \( q \) is the heat change, \( m \) is the mass, \( c \) is the heat capacity, and \( \Delta T \) is the change in temperature. --- **3. Experimental Observations** Notice that for Part A of this lab, the temperature of the system and the surroundings both increased; however, for Part B, the temperature of the system decreased while that of
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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![**Chemical Reaction and Energy Calculation in Solutions**
**Chemical Equation:**
\[ \text{3 NaOH}_{(aq)} + \text{H}_3\text{PO}_4_{(aq)} \rightarrow \text{Na}_3\text{PO}_3_{(aq)} + \text{3 H}_2\text{O}_{(l)} \]
\[ \Delta H = -173.7 \, \text{kJ} \]
---
**1. Heat Produced Calculation**
If 31.2 mL of 0.45 M sodium hydroxide is mixed with 65.4 mL of 0.088 M phosphoric acid, how many kJ of heat are produced?
**Solution:**
- Moles of sodium hydroxide:
\[ 31.2 \, \text{mL} \times 0.45 \, \text{M} = 0.0140 \, \text{mol} \]
- Moles of phosphoric acid:
\[ 65.4 \, \text{mL} \times 0.088 \, \text{M} = 0.00575 \, \text{mol} \]
- Limiting reagent: Phosphoric acid (0.00575 mol) is the limiting reagent.
- Heat Calculation:
\[ 0.00575 \, \text{mol} \times (-173.7 \, \text{kJ/mol}) = -1 \, \text{kJ} \]
---
**2. Expected Final Temperature**
When the solutions are mixed, what final temperature should we expect the solution to reach? Assume the combined solution has the same density (1 g/mL) and heat capacity (4.184 J/g°C) as water and that it is initially at 22.4 °C.
- Use the equation for heat transfer:
\[ q = m \cdot c \cdot \Delta T \]
Where \( q \) is the heat change, \( m \) is the mass, \( c \) is the heat capacity, and \( \Delta T \) is the change in temperature.
---
**3. Experimental Observations**
Notice that for Part A of this lab, the temperature of the system and the surroundings both increased; however, for Part B, the temperature of the system decreased while that of](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6720f477-d171-4017-aeea-4a98f198692e%2F9945114a-951b-41f6-aded-d14c5a15a92c%2Fzd7bf1j.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction and Energy Calculation in Solutions**
**Chemical Equation:**
\[ \text{3 NaOH}_{(aq)} + \text{H}_3\text{PO}_4_{(aq)} \rightarrow \text{Na}_3\text{PO}_3_{(aq)} + \text{3 H}_2\text{O}_{(l)} \]
\[ \Delta H = -173.7 \, \text{kJ} \]
---
**1. Heat Produced Calculation**
If 31.2 mL of 0.45 M sodium hydroxide is mixed with 65.4 mL of 0.088 M phosphoric acid, how many kJ of heat are produced?
**Solution:**
- Moles of sodium hydroxide:
\[ 31.2 \, \text{mL} \times 0.45 \, \text{M} = 0.0140 \, \text{mol} \]
- Moles of phosphoric acid:
\[ 65.4 \, \text{mL} \times 0.088 \, \text{M} = 0.00575 \, \text{mol} \]
- Limiting reagent: Phosphoric acid (0.00575 mol) is the limiting reagent.
- Heat Calculation:
\[ 0.00575 \, \text{mol} \times (-173.7 \, \text{kJ/mol}) = -1 \, \text{kJ} \]
---
**2. Expected Final Temperature**
When the solutions are mixed, what final temperature should we expect the solution to reach? Assume the combined solution has the same density (1 g/mL) and heat capacity (4.184 J/g°C) as water and that it is initially at 22.4 °C.
- Use the equation for heat transfer:
\[ q = m \cdot c \cdot \Delta T \]
Where \( q \) is the heat change, \( m \) is the mass, \( c \) is the heat capacity, and \( \Delta T \) is the change in temperature.
---
**3. Experimental Observations**
Notice that for Part A of this lab, the temperature of the system and the surroundings both increased; however, for Part B, the temperature of the system decreased while that of
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