Questions: Calculate the bond dissociation energy needed to break all the bonds in a mole of carbon dioxide, CO2. Express your answer as an integer and include the appropriate units.

Calculate the bond dissociation energy needed to break all the bonds in a mole of carbon dioxide, CO2. Express your answer as an integer and include the appropriate units.

Transcript text: Calculate the bond dissociation energy needed to break all the bonds in a mole of carbon dioxide, $\mathrm{CO}_{2}$. Express your answer as an integer and include the appropriate units.

Solution

Solution Steps

Step 1: Identify the bonds in a carbon dioxide molecule

A carbon dioxide ($\mathrm{CO}_2$) molecule consists of one carbon atom double-bonded to two oxygen atoms. Therefore, each $\mathrm{CO}_2$ molecule has two C=O double bonds.

Step 2: Determine the bond dissociation energy for a C=O double bond

The bond dissociation energy for a C=O double bond is typically around 799 kJ/mol.

Step 3: Calculate the total bond dissociation energy for one $\mathrm{CO}_2$ molecule

Since there are two C=O double bonds in one $\mathrm{CO}_2$ molecule, the total bond dissociation energy for one molecule is: \[ 2 \times 799 \, \text{kJ/mol} = 1598 \, \text{kJ/mol} \]

Step 4: Calculate the bond dissociation energy for 3 moles of $\mathrm{CO}_2$

To find the bond dissociation energy needed to break all the bonds in 3 moles of $\mathrm{CO}_2$, multiply the energy for one mole by 3: \[ 3 \times 1598 \, \text{kJ/mol} = 4794 \, \text{kJ} \]

Final Answer

\[ \boxed{4794 \, \text{kJ}} \]

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