VCAA 2009 Exam 2 Q5 or Checkpoints Industrial Chemistry Multiple Choice Q27

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at 298 K

I must ask...what the? Can hydrogen fluoride really react with itself to form hydrogen and fluorine gas? From http://en.wikipedia.org/wiki/List_of_standard_Gibbs_free_energies_of_formation, the change in Gibbs energy is -275.4 kJ mol^-1 = -275400 J mol^-1.
Now, the standard change in Gibbs free energy = -RT * ln K, where R = 8.3145 J K^-1 mol^-1 and T is 298 K here.
So we have -275400 J mol^-1 = -8.1345 J mol^-1 K^-1 * 298 K * ln K
Rearranging, and as all the units drop off, ln K = 111.15, K = 1.87 * 10^48

Now this is for at 298 K
So for the given reaction, K is the square of this quantity, or 3.5 * 10^96. That is a monstrous K value; are you telling me that an equilibrium actually exists?

I might be being too picky, but I feel as if the question is seriously flawed.