Question

1. A reaction was conducted in 1-butanol at -80 ˚C and took 72 hours to go to completion. How long would you expect it to take if the reaction were run at 0 ˚C? How long would you expect it to take if the reaction were run at 100 ˚C? When the reaction is ran at 0 ˚C, it selectively forms one isomer over the other by a ratio of 100:1. What does that say about the different energies of activation at 0 ˚C? Would you expect that ratio to be greater or smaller at 100 ˚C?

Answer 1

as we increase the temperature for a reaction the number of molecules undergoing effective collisions increases. hence the activation energy barrier can be crossed easily. the rate of reaction increases and the time taken for completion of the reaction decreases. also when we increase the temperature the rearrangement of the intermediate compound decreases and the specific product is formed. at 100 degree celsius we would expect to get a pure product .