Chapter 12, Problem 12.107CHP

Consider three reactions with different values of E_a and ΔE:

$\begin{array}{lllll}Reaction1.E_{\text{a}}\hfill & =\hfill & 20\text{kJ/mol};\Delta E\hfill & =\hfill & -60\text{kJ/mol}\hfill \\ Reaction2.E_{\text{a}}\hfill & =\hfill & 10\text{kJ/mol};\Delta E\hfill & =\hfill & -20\text{kJ/mol}\hfill \\ Reaction3.E_{\text{a}}\hfill & =\hfill & 40\text{kJ/mol};\Delta E\hfill & =\hfill & +15\text{kJ/mol}\hfill \end{array}$

1. (a) Sketch a potential energy profile for each reaction that shows the potential energy of reactants, products, and the transition state. Include labels that define E_a and ΔE.
2. (b) Assuming that all three reactions are carried out at the same temperature and that all three have the same frequency factor A, which reaction is the fastest and which is the slowest?
3. (c) Which reaction is the most endothermic, and which is the most exothermic?