What is the change in entropy (in JK mol) of the system for the following reaction 2H2 (g) + 2FO (g) 2H20 (1) + F2 (g) 1)-352.4 2)-176.2 3) -790 4) -684
What is the change in entropy (in JK mol) of the system for the following reaction 2H2 (g) + 2FO (g) 2H20 (1) + F2 (g) 1)-352.4 2)-176.2 3) -790 4) -684
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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![**Title: Calculating the Change in Entropy for a Chemical Reaction**
Present the problem as follows:
---
**Question: What is the change in entropy (in J·K⁻¹·mol⁻¹) of the system for the following reaction?**
\[2H_2(g) + 2F_2(g) \rightarrow 2H_2O(l) + F_2(g)\]
---
**Options:**
1. -352.4
2. -176.2
3. -790
4. -684
5. +122.0
---
### Explanation:
In this problem, we are given a chemical reaction and asked to determine the change in entropy (\(ΔS\)) of the system. Entropy is a measure of the disorder or randomness in a system, typically expressed in joules per kelvin per mole (J·K⁻¹·mol⁻¹).
When calculating entropy changes, it is important to consider the standard molar entropy values for each substance involved in the reaction at a given temperature (usually 298 K). Here is a step-by-step approach on how you could compute \(ΔS\) for the given reaction:
1. **Identify the reactants and products**:
- Reactants: 2 moles of H₂ (g) and 2 moles of F₂ (g)
- Products: 2 moles of H₂O (l) and 1 mole of F₂ (g)
2. **Use standard molar entropy (\(S°\)) values**:
- Standard molar entropy values for each substance must be taken from a reference (e.g., H₂(g), F₂(g), H₂O(l)).
3. **Calculate the entropy change**:
\[
ΔS = \sum S°(\text{products}) - \sum S°(\text{reactants})
\]
4. **Substitute the values**:
\[
ΔS = [2S°(H₂O(l)) + S°(F₂(g))] - [2S°(H₂(g)) + 2S°(F₂(g))]
\]
5. **Solve for \(ΔS\)**:
- Perform the algebra using the given entropy values to find the correct option from the list.
**Note:**
The actual numerical values for standard molar entropy](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcc0fe995-7680-4da1-9251-6315116f8ff1%2Fb3bb41d6-150e-4918-98a5-5b4726a0de5d%2Flghtzx_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Calculating the Change in Entropy for a Chemical Reaction**
Present the problem as follows:
---
**Question: What is the change in entropy (in J·K⁻¹·mol⁻¹) of the system for the following reaction?**
\[2H_2(g) + 2F_2(g) \rightarrow 2H_2O(l) + F_2(g)\]
---
**Options:**
1. -352.4
2. -176.2
3. -790
4. -684
5. +122.0
---
### Explanation:
In this problem, we are given a chemical reaction and asked to determine the change in entropy (\(ΔS\)) of the system. Entropy is a measure of the disorder or randomness in a system, typically expressed in joules per kelvin per mole (J·K⁻¹·mol⁻¹).
When calculating entropy changes, it is important to consider the standard molar entropy values for each substance involved in the reaction at a given temperature (usually 298 K). Here is a step-by-step approach on how you could compute \(ΔS\) for the given reaction:
1. **Identify the reactants and products**:
- Reactants: 2 moles of H₂ (g) and 2 moles of F₂ (g)
- Products: 2 moles of H₂O (l) and 1 mole of F₂ (g)
2. **Use standard molar entropy (\(S°\)) values**:
- Standard molar entropy values for each substance must be taken from a reference (e.g., H₂(g), F₂(g), H₂O(l)).
3. **Calculate the entropy change**:
\[
ΔS = \sum S°(\text{products}) - \sum S°(\text{reactants})
\]
4. **Substitute the values**:
\[
ΔS = [2S°(H₂O(l)) + S°(F₂(g))] - [2S°(H₂(g)) + 2S°(F₂(g))]
\]
5. **Solve for \(ΔS\)**:
- Perform the algebra using the given entropy values to find the correct option from the list.
**Note:**
The actual numerical values for standard molar entropy
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