[Hockey66]

The isomerization of a molecule in the gas phase occurs with a rate constant of 0.0006 at 410 degrees C. Calculate the value of the standard molar Gibbs energy of activation (in J. mol-1) for the reaction.

I have no idea where to start for this question! We're given the formulas: K = [AB]/[A][ B], K= e^(-deltaG/RT) x [A][ B] and rate = k(subB)T/h x e^(-deltaG/RT) x [A][ B].

Any ideas or pointers?  I did it and got 39,351 and the answer was 214,108.  I messed up and used capital K as the rate constant, I think.  It should be k(subB) right?  I get one more attempt at it (it's an online assessment), so if you help me out can you use the numbers given below please?  Thanks for your guys' help.

The isomerization of a molecule in the gas phase occurs with a rate constant of 0.0007 at 432 degrees C. Calculate the value of the standard molar Gibbs energy of activation (in J. mol-1) for the reaction.

[dm164]

k_B would be Boltzmann constant. And make sure to always us Kelvin for temperatures in most energy equations.