[odicon]

The isomerization of a molecule in the gas phase occurs with a rate constant of 0.0007 at 372 degrees C. Calculate the value of the standard molar Gibbs energy of activation (in J. mol-1) for the reaction.

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Hello everyone,

So for this question, I understand that you need to use transition-state theory to solve it. But I do not know how to get started because I have never used the equation before. How would you even start? I think this should be the right equation but I do not understand what the question is looking for. k(T) = k_BT/h e^(Delta G_o/RT)

It would be very appreciated if you could show me how you would go about setting up the equation (to begin solving the problem). Thank you so much!

[tamim83]

The question is asking you to find the  :delta:G_o in your equation.  You have everything you need, remember to put your temperature in Kelvins.  K_b is 1.38 x 10^-23 J/K, h is6.63 x 10^-34,  and R is 8.314 J/mol*K.  

To solve for the free energy of activation, you will need some properties of logarithms.  Taking the natural log (ln) of an exponential will get rid of e.  I would move the pre-exponent (k_bT/H) to the other side first and then take the ln of each side to start.  

Hope that helps.