The bond enthalpy of N2(g) is 418.0 kJ/mol. Calculate ÄH°f for N(g).?
To calculate ΔH°f for N(g), we need to use the bond enthalpy of N2(g) and the equation:
N2(g) → 2N(g)
The bond enthalpy of N2(g) is given as 418.0 kJ/mol, which represents the energy required to break one mole of N-N bonds in N2(g).
Since the reaction involves breaking one N-N bond in N2(g) and forming two N atoms, we need to consider the bond dissociation energies for both processes.
To find the enthalpy change, we subtract the energy required to break the N-N bond from the energy released when forming two N atoms. The equation would look like this:
ΔH°f for N(g) = (2 × bond enthalpy of N(g)) - bond enthalpy of N2(g)
Substituting the given values:
ΔH°f for N(g) = (2 × bond enthalpy of N(g)) - 418.0 kJ/mol
Now, you just need to know the bond enthalpy of N(g). However, that information is not typically provided directly. It can be determined experimentally or estimated based on other similar compounds.