Alright so I have a chemistry exam coming up in a couple days and I'm reviewing old exams as practice. I've come across a question that I believe *should* be easy but I just can't find the right answer to.
Given that the standard molar enthalpy of formation for nitrogen dioxide gas, NO2(g), and for dinitrogen tetraoxide gas, N2O4(g), is 33.85 kJ*mol-1 and 9.66 kJ*mol-1, respectively, the nitrogen-to-nitrogen, N-N, bond dissociation enthalpy in dinitrogen tetraoxide, O2N-NO2 (the dimer of NO2), is
a) 9.7 kj*mol-1
b) 24.2 kj*mol-1
c) 33.8 kj*mol-1
d) 58.0 kj*mol-1
e) 77.4 kj*mol-1
Thanks in advance! Glad I came across this forum, lots of useful info here.