11. Bonding & Molecular Structure

Consider the following equation:

Determine the bond enthalpy value for the F–S bond.

Use the bond energies to estimate the enthalpy of reaction for the combustion of 5 moles of acetylene:

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)

Calculate the average molar bond enthalpy of the carbon–hydrogen bond in a CH₄ molecule.

Use average bond energies to calculate δHrxn for the following hydrogenation reaction: H₂C=CH₂(g) + H₂(g) → H₃C−CH₃(g)

Calculate δhrxn for the combustion of octane (C₈H₁₈) by using average bond energies.

Use average bond enthalpies to estimate the enthalpy δhrxn of the following reaction: 2 SF₄(g) + O₂(g) → 2 OSF₄(g)

Ethanol is a possible fuel. use average bond energies to calculate δH_rxn for the combustion of ethanol.

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)

2 H₃C−CH₃(g) + 7O₂(g) → 4 CO₂(g) + 6 H₂O(g)