11. Bonding & Molecular Structure

Bond Energy

Multiple Choice
What is the bond order of the molecule O_2^+?
Open Question
Ethanol is a possible fuel. use average bond energies to calculate δH_rxn for the combustion of ethanol. CH₃CH₂OH(g) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(g)
Multiple Choice
Consider the following equation:
Determine the bond enthalpy value for the F–S bond.
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Multiple Choice
Which of the following is the bond order of the diatomic molecule with 10 valence electrons, such as O2?
Multiple Choice
Given that ΔH° = -311 kJ for the hydrogenation of acetylene, C₂H₂: H-C≡C-H(g) + 2 H₂(g) → CH₃-CH₃(g) and the following bond dissociation energies: H-H = 436 kJ/mol, C-H = 413 kJ/mol, and C-C = 348 kJ/mol, estimate a value for the C≡C triple bond dissociation energy?
Multiple Choice
Use the bond energies in Chemistry 2e of your textbook to determine the approximate enthalpy change for the following reaction: H2(g) + 1/2 O2(g) → H2O(g). What is the approximate enthalpy change (ΔH) for this reaction?
Multiple Choice
What is the bond order of the diatomic molecule B_2?
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Multiple Choice
Given the bond energies: Br-Br = 192 kJ/mol, C≡C = 839 kJ/mol, C-Br = 276 kJ/mol, estimate ΔH°rxn for the reaction 2 Br2(l) + C2H2(g) → C2H2Br4(l). What is the ΔH°rxn?
Open Question
Calculate δh° for the reaction using the given bond dissociation energies.
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Multiple Choice
Calculate the enthalpy of the following reaction based on average bond enthalpies.
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Open Question
Ethanol is a possible fuel. Use average bond energies to calculate δH_rxn for the combustion of ethanol. CH₃CH₂OH(g) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(g)
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Multiple Choice
Which of the following bonds is the strongest?
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Open Question
Ethanol is a possible fuel. use average bond energies to calculate δH_rxn for the combustion of ethanol.
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Multiple Choice
Use the bond energies to determine the approximate enthalpy change for the following reaction: H2(g) + 1/2 O2(g) → H2O(g). Given the bond energies: H-H = 436 kJ/mol, O=O = 498 kJ/mol, and O-H = 463 kJ/mol.
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Multiple Choice
Use the bond energies to estimate the enthalpy of reaction for the combustion of 5 moles of acetylene:
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