1. An $$ \mathrm{O}=\mathrm{O} $$ bond has a bond energy of $$ 498 \mathrm{~kJ} / \mathrm{mol} $$. a. How much energy is required to break the bond?

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To determine the energy required to break an $$ \mathrm{O}=\mathrm{O} $$ bond, we can use the given bond energy.

### Given:
- **Bond Energy of $$ \mathrm{O}=\mathrm{O} $$ bond:** $$ 498 \, \text{kJ/mol} $$

### a. Energy Required to Break the Bond

The bond energy value represents the amount of energy needed to break one mole of bonds in the gas phase. Therefore, to break one mole of $$ \mathrm{O}=\mathrm{O} $$ bonds, the energy required is:

$$
498 \, \text{kJ/mol}
$$

**Summary:**
- **Energy required to break one mole of $$ \mathrm{O}=\mathrm{O} $$ bonds:** $$ 498 \, \text{kJ} $$

If you are interested in the energy required to break a single $$ \mathrm{O}=\mathrm{O} $$ bond (not per mole), you can use Avogadro's number ($$ 6.022 \times 10^{23} $$ mol$$^{-1}$$) to convert:

$$
\text{Energy per bond} = \frac{498 \times 10^3 \, \text{J/mol}}{6.022 \times 10^{23} \, \text{bonds/mol}} \approx 8.27 \times 10^{-19} \, \text{J per bond}
$$

However, for most practical chemistry calculations, the energy per mole ($$ 498 \, \text{kJ/mol} $$) is typically used.

**Answer:**  
a. 498 kilojoules of energy are needed to break each mole of O=O bonds.
To break one mole of $$ \mathrm{O}=\mathrm{O} $$ bonds, 498 kJ of energy is required.

1. An \( \mathrm{O}=\mathrm{O} \) bond has a bond energy of \( 498 \mathrm{~kJ} / \mathrm{mol} \). a. How much energy is required to break the bond?

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