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 answer question 11 part A and B
![**Part B: Calculating Enthalpy of Reaction**
*Objective:*
Calculate the enthalpy of the reaction:
\[ 4\text{B(s)} + 3\text{O}_2\text{(g)} \rightarrow 2\text{B}_2\text{O}_3\text{(s)} \]
*Given Information:*
1. \(\text{B}_2\text{O}_3\text{(s)} + 3\text{H}_2\text{O(g)} \rightarrow 3\text{O}_2\text{(g)} + \text{B}_2\text{H}_6\text{(g)}, \quad \Delta H^{\circ}_A = +2035 \text{ kJ}\)
2. \(2\text{B(s)} + 3\text{H}_2\text{(g)} \rightarrow \text{B}_2\text{H}_6\text{(g)}, \quad \Delta H^{\circ}_B = +36 \text{ kJ}\)
3. \(\text{H}_2\text{(g)} + \frac{1}{2}\text{O}_2\text{(g)} \rightarrow \text{H}_2\text{O(l)}, \quad \Delta H^{\circ}_C = -285 \text{ kJ}\)
4. \(\text{H}_2\text{O(l)} \rightarrow \text{H}_2\text{O(g)}, \quad \Delta H^{\circ}_D = +44 \text{ kJ}\)
*Instruction:*
Express your answer with the appropriate units.
[**ΔH° =** **Value** **Units**]
**Note:** Click "View Available Hint(s)" for assistance with the calculation steps.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded90a0e-1aa2-42d3-8902-387fb21746ad%2F5a5d7fbb-5bbe-4c58-b564-ea8ba56b3a90%2Fpswiqbb_processed.png&w=3840&q=75)
Transcribed Image Text:**Part B: Calculating Enthalpy of Reaction**
*Objective:*
Calculate the enthalpy of the reaction:
\[ 4\text{B(s)} + 3\text{O}_2\text{(g)} \rightarrow 2\text{B}_2\text{O}_3\text{(s)} \]
*Given Information:*
1. \(\text{B}_2\text{O}_3\text{(s)} + 3\text{H}_2\text{O(g)} \rightarrow 3\text{O}_2\text{(g)} + \text{B}_2\text{H}_6\text{(g)}, \quad \Delta H^{\circ}_A = +2035 \text{ kJ}\)
2. \(2\text{B(s)} + 3\text{H}_2\text{(g)} \rightarrow \text{B}_2\text{H}_6\text{(g)}, \quad \Delta H^{\circ}_B = +36 \text{ kJ}\)
3. \(\text{H}_2\text{(g)} + \frac{1}{2}\text{O}_2\text{(g)} \rightarrow \text{H}_2\text{O(l)}, \quad \Delta H^{\circ}_C = -285 \text{ kJ}\)
4. \(\text{H}_2\text{O(l)} \rightarrow \text{H}_2\text{O(g)}, \quad \Delta H^{\circ}_D = +44 \text{ kJ}\)
*Instruction:*
Express your answer with the appropriate units.
[**ΔH° =** **Value** **Units**]
**Note:** Click "View Available Hint(s)" for assistance with the calculation steps.
![### Understanding Hess's Law
Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." Here are important rules to remember:
1. **Addition of Reactions:** When two reactions are added, their enthalpy values are also added.
2. **Reversing a Reaction:** If a reaction is reversed, the sign of its enthalpy value is changed.
3. **Multiplying Reaction Coefficients:** If the coefficients of a reaction are multiplied by a factor, the enthalpy value is multiplied by the same factor.
### Problem Statement
**Part A:** Calculate the enthalpy of the reaction:
\[ 2\text{NO}(g) + \text{O}_2(g) \rightarrow 2\text{NO}_2(g) \]
Using the following reactions and enthalpies of formation:
1. \(\frac{1}{2}\text{N}_2(g) + \text{O}_2(g) \rightarrow \text{NO}_2(g)\), \(\Delta H_A^\circ = 33.2 \text{ kJ}\)
2. \(\frac{1}{2}\text{N}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{NO}(g)\), \(\Delta H_B^\circ = 90.2 \text{ kJ}\)
**Task:** Express your answer with the appropriate units.
**Input Box:** Calculate and enter the value for \(\Delta H^\circ\).
```plaintext
\(\Delta H^\circ = \text{Value} \quad \text{Units}\)
```
Click to view available hints if needed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded90a0e-1aa2-42d3-8902-387fb21746ad%2F5a5d7fbb-5bbe-4c58-b564-ea8ba56b3a90%2Fd94v62n_processed.png&w=3840&q=75)
Transcribed Image Text:### Understanding Hess's Law
Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." Here are important rules to remember:
1. **Addition of Reactions:** When two reactions are added, their enthalpy values are also added.
2. **Reversing a Reaction:** If a reaction is reversed, the sign of its enthalpy value is changed.
3. **Multiplying Reaction Coefficients:** If the coefficients of a reaction are multiplied by a factor, the enthalpy value is multiplied by the same factor.
### Problem Statement
**Part A:** Calculate the enthalpy of the reaction:
\[ 2\text{NO}(g) + \text{O}_2(g) \rightarrow 2\text{NO}_2(g) \]
Using the following reactions and enthalpies of formation:
1. \(\frac{1}{2}\text{N}_2(g) + \text{O}_2(g) \rightarrow \text{NO}_2(g)\), \(\Delta H_A^\circ = 33.2 \text{ kJ}\)
2. \(\frac{1}{2}\text{N}_2(g) + \frac{1}{2}\text{O}_2(g) \rightarrow \text{NO}(g)\), \(\Delta H_B^\circ = 90.2 \text{ kJ}\)
**Task:** Express your answer with the appropriate units.
**Input Box:** Calculate and enter the value for \(\Delta H^\circ\).
```plaintext
\(\Delta H^\circ = \text{Value} \quad \text{Units}\)
```
Click to view available hints if needed.
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