Question
The enthalpy of dissociation for hydrogen
H2(g) → 2 H(g)
is ΔH = 436.0 kJ/mol. What is the difference between the bond enthalpy (ΔH) and bond energy (ΔE) for this process under standard conditions at 298.15 K?
H2(g) → 2 H(g)
is ΔH = 436.0 kJ/mol. What is the difference between the bond enthalpy (ΔH) and bond energy (ΔE) for this process under standard conditions at 298.15 K?