If AH° of a mock reaction, H2(g) + X2(g) → 2HX (g) is -184.7 kJ/mol, given the bond energy of H-H is 436 kJ/mol, and X-X is 243 kJ/mol, determine the bond energy of one mole of H-X bond in the product.
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
![### Determining Bond Energy in a Chemical Reaction
**Problem Statement:**
In a mock chemical reaction:
\[ \text{H}_2(g) + \text{X}_2(g) \rightarrow 2\text{HX} (g) \]
The standard enthalpy change (\(\Delta H^0\)) is given as -184.7 kJ/mol. The bond energies for the involved molecules are:
- H-H bond: 436 kJ/mol
- X-X bond: 243 kJ/mol
**Objective:**
Calculate the bond energy of one mole of the H-X bond in the product.
**Calculation Steps:**
1. **Define the Reaction:**
- Breaking of bonds: H-H and X-X
- Formation of bonds: 2 H-X
2. **Using the Enthalpy Formula:**
\[
\Delta H^0 = \left(\text{Bond energies of reactants} - \text{Bond energies of products}\right)
\]
3. **Plugging in the Values:**
\[
\Delta H^0 = [(436 \, \text{kJ/mol} + 243 \, \text{kJ/mol}) - 2 \times \text{H-X}]
\]
\(-184.7 = [436 + 243 - 2 \times \text{H-X}]\)
4. **Solve for H-X:**
\[
-184.7 = [679 - 2 \times \text{H-X}]
\]
\[
2 \times \text{H-X} = 679 + 184.7
\]
\[
2 \times \text{H-X} = 863.7
\]
\[
\text{H-X} = \frac{863.7}{2}
\]
\[
\text{H-X} = 431.85 \, \text{kJ/mol}
\]
Thus, the bond energy of the H-X bond is approximately 431.85 kJ/mol.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bd06d49-1f03-4d83-9ba1-5526279a5db3%2F3b1fefc5-921e-4370-9ba4-f3a8740c927c%2F6vfh6ok_processed.jpeg&w=3840&q=75)
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