Bond Enthalpy
Chemistry ⇒ Thermochemistry and Energetics
Bond Enthalpy starts at 11 and continues till grade 12.
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Describe how bond enthalpy data can be used to estimate the enthalpy change of a chemical reaction.
Describe one limitation of using average bond enthalpies to calculate enthalpy changes of reactions.
Describe the difference between bond enthalpy and lattice enthalpy.
Describe the relationship between bond length and bond enthalpy.
Given the following bond enthalpies: C–H = 413 kJ mol–1, Cl–Cl = 243 kJ mol–1, C–Cl = 338 kJ mol–1, calculate the enthalpy change for the reaction: CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g). Assume H–Cl = 431 kJ mol–1.
Given the following bond enthalpies: C–H = 413 kJ mol–1, O=O = 498 kJ mol–1, C=O = 799 kJ mol–1, calculate the enthalpy change for the reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g). Assume O–H = 463 kJ mol–1.
Given the following bond enthalpies: C–H = 413 kJ mol–1, O=O = 498 kJ mol–1, C=O = 799 kJ mol–1, O–H = 463 kJ mol–1. Calculate the enthalpy change for the reaction: CH3OH(g) + 3/2 O2(g) → CO2(g) + 2H2O(g).
Given the following bond enthalpies: H–H = 436 kJ mol–1, Br–Br = 193 kJ mol–1, H–Br = 366 kJ mol–1. Calculate the enthalpy change for the reaction: H2(g) + Br2(g) → 2HBr(g).
Bond enthalpy is also known as: (1) Lattice energy (2) Bond dissociation energy (3) Ionization energy (4) Electron affinity
Bond enthalpy values are always measured in which state? (1) Solid (2) Liquid (3) Gaseous (4) Aqueous
Which bond is stronger based on bond enthalpy values? (1) C–C (2) C=C (3) C≡C
Which of the following best defines bond enthalpy? (1) The energy required to break one mole of a specific type of bond in a gaseous molecule (2) The energy released when a bond is formed in a solid (3) The energy required to break all bonds in a liquid (4) The energy required to melt one mole of a substance
Fill in the blank: The bond enthalpy of a bond is the energy required to break one mole of the bond in the ______ state.
Fill in the blank: The bond enthalpy of a C–H bond is ______ kJ mol–1 (use the average value 413).
Fill in the blank: The bond enthalpy of a N≡N bond is ______ kJ mol–1 (use the average value 945).
Fill in the blank: The enthalpy change for a reaction is negative if the total energy released in bond formation is ______ than the total energy required for bond breaking.
Bond enthalpy is always a positive value. True or False?
Is the bond enthalpy of a double bond generally greater than that of a single bond between the same two atoms? Yes or No.
True or False: The bond enthalpy of a bond in a polyatomic molecule is always the same as in a diatomic molecule.
True or False: The bond enthalpy of a C–H bond in methane is exactly the same as in ethane.
