11. Bonding & Molecular Structure

Bond Energy

Multiple Choice
Use bond energies to estimate the enthalpy change for the formation of HBr(g) from H2(g) and Br2(g). Given: BE(H-H) = 436 kJ/mol, BE(Br-Br) = 192 kJ/mol, BE(H-Br) = 366 kJ/mol.
Multiple Choice
Consider the following equation:
Determine the bond enthalpy value for the F–S bond.
Multiple Choice
Use the bond energies to estimate the enthalpy of reaction for the combustion of 5 moles of acetylene:
Multiple Choice
Calculate the enthalpy of the following reaction based on average bond enthalpies.
Multiple Choice
Which of the following bonds is the strongest?
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)
Open Question
Calculate the average molar bond enthalpy of the carbon–hydrogen bond in a CH₄ molecule.
Open Question
Use average bond energies to calculate δHrxn for the following hydrogenation reaction: H₂C=CH₂(g) + H₂(g) → H₃C−CH₃(g)
Open Question
Calculate δhrxn for the combustion of octane (C₈H₁₈) by using average bond energies.
Open Question
Use average bond enthalpies to estimate the enthalpy δhrxn of the following reaction: 2 SF₄(g) + O₂(g) → 2 OSF₄(g)
Open Question
Ethanol is a possible fuel. use average bond energies to calculate δH_rxn for the combustion of ethanol.
Open Question
Predict whether the following reactions will be exothermic or endothermic.
Open Question
Calculate δh° for the reaction using the given bond dissociation energies.
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)
Open Question
2 H₃C−CH₃(g) + 7O₂(g) → 4 CO₂(g) + 6 H₂O(g)