Bond Enthalpy
Chemistry ⇒ Thermochemistry and Energetics
Bond Enthalpy starts at 11 and continues till grade 12.
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Arrange the following bonds in order of increasing bond enthalpy: C–C, C=C, C≡C.
Define bond enthalpy.
Describe how resonance affects bond enthalpy values.
Describe the relationship between bond length and bond enthalpy.
Calculate the enthalpy change for the reaction:
CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g)
Given: Bond enthalpies (kJ mol–1): C–H = 413, Cl–Cl = 243, C–Cl = 328, H–Cl = 431.
Calculate the enthalpy change for the reaction:
H2(g) + Cl2(g) → 2HCl(g)
Given: Bond enthalpies (kJ mol–1): H–H = 436, Cl–Cl = 243, H–Cl = 431.
Given the following bond enthalpies: H–H = 436 kJ mol–1, O=O = 498 kJ mol–1, O–H = 463 kJ mol–1. Calculate the enthalpy change for the reaction:
2H2(g) + O2(g) → 2H2O(g)
Given the following bond enthalpies: N≡N = 945 kJ mol–1, H–H = 436 kJ mol–1, N–H = 391 kJ mol–1. Calculate the enthalpy change for the reaction:
N2(g) + 3H2(g) → 2NH3(g)
Which of the following bonds has the highest bond enthalpy?
(1) H–H
(2) O=O
(3) N≡N
(4) Cl–Cl
Which of the following bonds is expected to have the lowest bond enthalpy?
(1) C–C
(2) C=C
(3) C≡C
(4) C–H
Which of the following bonds is the weakest?
(1) F–F
(2) Cl–Cl
(3) Br–Br
(4) I–I
Which of the following factors does NOT affect bond enthalpy?
(1) Bond order
(2) Atomic size
(3) Temperature
(4) Isotopic mass
Bond enthalpy is also known as _______ energy.
Bond enthalpy is measured per _______ of bonds.
Bond enthalpy values are typically reported in units of _______.
Bond enthalpy values are usually determined for molecules in the _______ phase.
Bond enthalpy is always a positive value. True or False?
Bond enthalpy values are always measured under standard conditions. True or False?
Bond enthalpy values can be used to compare the stability of molecules. Yes or No?
The bond enthalpy of a C–C single bond is 348 kJ mol–1. Is the bond enthalpy of a C=C double bond expected to be exactly twice this value? Yes or No.
