I have often come across reactions where kinetic and thermodynamic processes give completely different outputs. I was told that in such cases check temperature, if temperature controlled, then take thermodynamic product otherwise if reaction is very fast (not temperature controlled) then consider the kinetic product.

I was also told that if there is a case where you can't decide whether it is temperature controlled or speed controlled, then always take the thermodynamic product.

My question is: Why will thermodynamic processes have an upper hand in the latter case? CH2CHC(CH2)CH3 what MAJOR product does it produce on giving 1 equivalent HBr?

  • $\begingroup$ Can you give a specific example? $\endgroup$ – Chet Miller Nov 24 '15 at 0:14
  • $\begingroup$ An example from organic chemistry. $\endgroup$ – Qwerty Nov 24 '15 at 6:07
  • $\begingroup$ I edited the question. $\endgroup$ – Qwerty Nov 24 '15 at 6:10
  • $\begingroup$ I'm having trouble understanding what you are asking. Is it something like: what is the difference between solving a problem using the equilibrium constant and using the reaction kinetics equations? $\endgroup$ – Chet Miller Nov 24 '15 at 12:33
  • $\begingroup$ Not quite. Look at the example that I gave. If we assume CH2CHC(CH2)CH3 to follow temperature controlled reaction when provided with 1 equivalent of HBr, the product it gives (I think) will be different from the one if we assume the reaction to be very fast and not quite affected by temperature. $\endgroup$ – Qwerty Nov 24 '15 at 13:08

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