The following reaction: 2HBr(g)
(g) + Br2
The values of the equilibrium constant temperatures are:
What is the :delta: H for this reaction in kJ/mol? (R=8.31*10-3
A) -67.8 kJ/mol B) 16.5 kJ/mol C) 74.0 kJ/mol D) 97.2 kJ/mol
I thought this was a pretty straightforward application of an equation, but I got it wrong, so if anyone could tell me if I did anything wrong, I would really, really appreciate it!
)= :delta: H/R (1/T2
)/(1/300-1/500)= :delta: H=74 kJ, which is C. But the answer key says the answer is D?
Again, thanks soo much!