Question

Use the bond energies to answer the question. H–H = 432 H–O = 467 O–O = 146 O=O = 495 H2 (H–H) combines with O2 (O=O) to become hydrogen peroxide (H2O2) bonded as such: H–O–O–H. Which option shows the difference in total bond energy between the reactants and the products? (1 point) Responses 153 153 −153 negative 153 1,080 1 comma 080 \ce\bond−927 ce bond negative 927

Answer 1

To find the difference in total bond energy between the reactants and the products, we will calculate the bond energies for the bonds broken in the reactants and the bonds formed in the products.

Step 1: Calculate the bond energies for the reactants (H2 + O2)

• Reactants:
  • 1 H–H bond from H2: \( 432 , \text{kJ/mol} \)
  • 1 O=O bond from O2: \( 495 , \text{kJ/mol} \)

Total bond energy of reactants: \[ \text{Total energy of reactants} = 432 + 495 = 927 , \text{kJ/mol} \]

Step 2: Calculate the bond energies for the products (H2O2)

• Products:
  • 2 H–O bonds in H2O2: \( 2 \times 467 = 934 , \text{kJ/mol} \)
  • 1 O–O bond in H2O2: \( 146 , \text{kJ/mol} \)

Total bond energy of products: \[ \text{Total energy of products} = 934 + 146 = 1,080 , \text{kJ/mol} \]

Step 3: Calculate the difference in bond energy between products and reactants \[ \Delta E = \text{Total energy of products} - \text{Total energy of reactants} = 1,080 - 927 = 153 , \text{kJ/mol} \]

Therefore, the difference in total bond energy between the reactants and the products is 153 kJ/mol.

The correct answer is 153.