For NH3 (ammonia) and H2O (water)…
a. Use curved arrows to show the most likely acid-base reaction, and draw the resulting products. (Hint: First decide which is the stronger acid, and which is the stronger base.)
b. Mark each curved arrow with a positive (bond-breaking) or negative (bond-forming) number indicating the energy change associated with that arrow (in pKa units).
c. Calculate ΔHrxn, and write this number above a set of reaction arrows that indicate which direction is downhill/favorable (in the example, the reaction is downhill to the right).
d. Sketch an energy diagram for the reaction.
e. Is your energy diagram consistent with the fact that, in this case, the most likely acid-base reaction is endothermic?
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