Calculate the enthalpy change in kJ/mol (delta H) for the following reaction using the data table.

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Calculate the enthalpy change in kJ/mol (delta H) for the following reaction using the data table.

Below is a transcription and explanation of the information presented in the image, which is suitable for an educational website on chemistry:

---

### Bond Dissociation Energies

The diagram shows bond dissociation energies in kilojoules per mole (kJ/mol) for various types of chemical bonds. Bond dissociation energy is the measure of bond strength in a chemical bond and is defined as the energy required to break the bond between two atoms.

#### Left Section

- **Bonds and Energies:**
  - C–I: 240 kJ/mol
  - CH₃–C–I: 208 kJ/mol
  - H₂C═CH–Cl: 433 kJ/mol
  - (other C and halogen bonds listed in parallel)

- **Diatomic Bonds:**
  - H–I: 295 kJ/mol
  - H–Br: 367 kJ/mol
  - H–Cl: 431 kJ/mol
  - H–F: 565 kJ/mol

#### Right Section

- **Common Bonds and Energies:**
  - C–C: 346 kJ/mol
  - C–H: 412 kJ/mol
  - C–OH: 360 kJ/mol

- **Alcohol and Phenol Bonds:**
  - CH₃–OH: 463 kJ/mol
  - CH₃–O–CH₃: 377 kJ/mol
  - C₆H₅–OH: 460 kJ/mol

### Description of Graph Structure

- **Vertical Axis:** Denoted as \( D \) in kJ/mol, showing the bond dissociation energy.
- **Horizontal Axis:** Represents different chemical bonds.

The graph is divided into sections for different categories of bonds, listed from higher to lower energy. Each bond is linked to its energy value, showing variations in bond strength between different atoms and functional groups.

### Educational Interpretation

This diagram helps in understanding how bond strength varies between different types of bonds. For instance, the C–H bond is stronger than the C–I bond due to its higher dissociation energy. Understanding these energies is fundamental in predicting reaction pathways and stability in organic and inorganic chemistry.

--- 

This content provides foundational knowledge for students and educators in chemistry, illustrating the concept of bond dissociation energies with practical examples.
Transcribed Image Text:Below is a transcription and explanation of the information presented in the image, which is suitable for an educational website on chemistry: --- ### Bond Dissociation Energies The diagram shows bond dissociation energies in kilojoules per mole (kJ/mol) for various types of chemical bonds. Bond dissociation energy is the measure of bond strength in a chemical bond and is defined as the energy required to break the bond between two atoms. #### Left Section - **Bonds and Energies:** - C–I: 240 kJ/mol - CH₃–C–I: 208 kJ/mol - H₂C═CH–Cl: 433 kJ/mol - (other C and halogen bonds listed in parallel) - **Diatomic Bonds:** - H–I: 295 kJ/mol - H–Br: 367 kJ/mol - H–Cl: 431 kJ/mol - H–F: 565 kJ/mol #### Right Section - **Common Bonds and Energies:** - C–C: 346 kJ/mol - C–H: 412 kJ/mol - C–OH: 360 kJ/mol - **Alcohol and Phenol Bonds:** - CH₃–OH: 463 kJ/mol - CH₃–O–CH₃: 377 kJ/mol - C₆H₅–OH: 460 kJ/mol ### Description of Graph Structure - **Vertical Axis:** Denoted as \( D \) in kJ/mol, showing the bond dissociation energy. - **Horizontal Axis:** Represents different chemical bonds. The graph is divided into sections for different categories of bonds, listed from higher to lower energy. Each bond is linked to its energy value, showing variations in bond strength between different atoms and functional groups. ### Educational Interpretation This diagram helps in understanding how bond strength varies between different types of bonds. For instance, the C–H bond is stronger than the C–I bond due to its higher dissociation energy. Understanding these energies is fundamental in predicting reaction pathways and stability in organic and inorganic chemistry. --- This content provides foundational knowledge for students and educators in chemistry, illustrating the concept of bond dissociation energies with practical examples.
The image depicts a chemical equation representing a halogenation reaction of an alkene with hydrogen iodide (HI).

**Chemical Equation:**

1. **Reactants:**
   - On the left, there is an alkene represented by the "H" attached to a double bond and an R group (indicating the rest of the molecule).
   - Hydrogen iodide (HI).

2. **Products:**
   - On the right, the iodine (I) atom attaches to the carbon that was part of the double bond, forming an alkyl iodide.
   - A molecule of H–I is shown as a product, indicating the addition of hydrogen to the other carbon atom of the former double bond. 

**Reaction Type:**
- This is an example of an electrophilic addition reaction, where the pi bond of the alkene is broken and new single bonds are formed. 

This type of reaction is commonly used in organic chemistry to convert alkenes into more complex molecules with halogen atoms.
Transcribed Image Text:The image depicts a chemical equation representing a halogenation reaction of an alkene with hydrogen iodide (HI). **Chemical Equation:** 1. **Reactants:** - On the left, there is an alkene represented by the "H" attached to a double bond and an R group (indicating the rest of the molecule). - Hydrogen iodide (HI). 2. **Products:** - On the right, the iodine (I) atom attaches to the carbon that was part of the double bond, forming an alkyl iodide. - A molecule of H–I is shown as a product, indicating the addition of hydrogen to the other carbon atom of the former double bond. **Reaction Type:** - This is an example of an electrophilic addition reaction, where the pi bond of the alkene is broken and new single bonds are formed. This type of reaction is commonly used in organic chemistry to convert alkenes into more complex molecules with halogen atoms.
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