Draw an energy diagram of the following reactions. A one step reaction with a positive AG O A one step reaction with a negative AG A two-step reaction with an overall positive-Where the intermediates are lower energy than the reactants and the first transition state is lower in energy than the second.
ΔG of any reaction can be written in terms of energy of reactants and products as,
=> ΔG = Total energy of products - total energy of reactants.
Hence if ΔG is +ve, => Total energy of products > Total energy of reactants
And if ΔG is -ve, => Total energy of products < Total energy of reactants
And the number of steps in reaction basically shows the number of peaks in the energy diagram.
For 3rd case, since the energy of transition state 1 is lower than the energy of transition state 2.
Hence the peak height will be more for the 2nd peak compared to first pick.
And since the energy of intermediate is less than reactants, hence the I i.e intermeidates will be below R i.e reactants and P i.e products will be above R to make ΔG +ve.
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