ep 1. H₂O₂ +J H₂O + 10 slow ep 2. 10 + H₂Qz H₂O + 0₂ + I fast The reaction coordinate diagram for this mechanism is show below. 70 60 40 30 10 Progress of the Reaction What is the AH for the reverse reaction? 50 kJ/mol/30 kJ/mol/none of the answers are correct/20 kJ/mol/-20 kJ/mol Potential Energy (kJ/mol)

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Chapter1: Chemical Foundations
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### Considering the Reaction Mechanism Shown Below

#### Mechanism Steps:
**Step 1**:
\[ \text{H}_2\text{O}_2 + \text{I}^- \rightarrow \text{H}_2\text{O} + \text{IO}^- \] *(slow)*

**Step 2**:
\[ \text{IO}^- + \text{H}_2\text{O}_2 \rightarrow \text{H}_2\text{O} + \text{O}_2 + \text{I}^- \] *(fast)*

#### Explanation:
The reaction mechanism involves two steps. 

1. In the first step, hydrogen peroxide (H₂O₂) reacts with iodide (I⁻) to form water (H₂O) and hypoiodite (IO⁻). This step is slow and is considered the rate-determining step.
2. In the second step, hypoiodite (IO⁻) further reacts with another molecule of hydrogen peroxide to form water, oxygen (O₂), and regenerate the iodide (I⁻) ion. This step proceeds fast.

### Reaction Coordinate Diagram:
Below the reaction mechanism, a reaction coordinate diagram illustrates the potential energy changes throughout the reaction progress.

#### Description of the Graph:
- **X-Axis**: Progress of the Reaction
- **Y-Axis**: Potential Energy (kJ/mol)
- The graph starts at a lower energy level and ascends to a peak around 40 kJ/mol, indicating the activation energy for the first step.
- It then drops to around 30 kJ/mol, showing the formation of an intermediate.
- A second peak at approximately 70 kJ/mol represents the activation energy for the second step.
- Finally, the potential energy decreases drastically to just above 10 kJ/mol as the reaction reaches completion.

### Question:
What is the \( \Delta H \) for the reverse reaction?

### Options:
- 50 kJ/mol
- 30 kJ/mol
- None of the answers are correct
- 20 kJ/mol
- -20 kJ/mol
Transcribed Image Text:### Considering the Reaction Mechanism Shown Below #### Mechanism Steps: **Step 1**: \[ \text{H}_2\text{O}_2 + \text{I}^- \rightarrow \text{H}_2\text{O} + \text{IO}^- \] *(slow)* **Step 2**: \[ \text{IO}^- + \text{H}_2\text{O}_2 \rightarrow \text{H}_2\text{O} + \text{O}_2 + \text{I}^- \] *(fast)* #### Explanation: The reaction mechanism involves two steps. 1. In the first step, hydrogen peroxide (H₂O₂) reacts with iodide (I⁻) to form water (H₂O) and hypoiodite (IO⁻). This step is slow and is considered the rate-determining step. 2. In the second step, hypoiodite (IO⁻) further reacts with another molecule of hydrogen peroxide to form water, oxygen (O₂), and regenerate the iodide (I⁻) ion. This step proceeds fast. ### Reaction Coordinate Diagram: Below the reaction mechanism, a reaction coordinate diagram illustrates the potential energy changes throughout the reaction progress. #### Description of the Graph: - **X-Axis**: Progress of the Reaction - **Y-Axis**: Potential Energy (kJ/mol) - The graph starts at a lower energy level and ascends to a peak around 40 kJ/mol, indicating the activation energy for the first step. - It then drops to around 30 kJ/mol, showing the formation of an intermediate. - A second peak at approximately 70 kJ/mol represents the activation energy for the second step. - Finally, the potential energy decreases drastically to just above 10 kJ/mol as the reaction reaches completion. ### Question: What is the \( \Delta H \) for the reverse reaction? ### Options: - 50 kJ/mol - 30 kJ/mol - None of the answers are correct - 20 kJ/mol - -20 kJ/mol
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