### Users Who Are Viewing This Thread (Users: 0, Guests: 1)

#### lorka150

I am not positive if I did this correctly, but I was wondering if someone could check and then, potentially, offer ideas.

The question asked to use bond energies and estimate the energy change deltaH (in kJ/mol) for

N=N + 2H2 --> H2N-NH2

(that first N=N is triple)

I think I just realized I did this wrong, because I didn't use a triple for the first one, but I'll write down what I did anyway, and maybe someone can help.

N=N = 418 kJ
H2 = 872.8 kJ
total = 1290.8 kJ

Then, I did
4 H2 bonds = 4x436.4 = -1745.6
2 N-H bonds = 2 x 393 = -786
total = -2531.6

Therefore, 1290.8 + (-2531.6) = -1240.8 kJ/mol

### The Physics Forums Way

We Value Quality
• Topics based on mainstream science
• Proper English grammar and spelling
We Value Civility
• Positive and compassionate attitudes
• Patience while debating
We Value Productivity
• Disciplined to remain on-topic
• Recognition of own weaknesses
• Solo and co-op problem solving