The equilibrium constant for the reaction from CTQ 47 is given below. [Square brackets]...

The equilibrium constant for the reaction from CTQ 47 is given below. [Square brackets] represent the concentration of that ion or molecule in moles/liter at equilibrium.

a. Is K_eq for this reaction a very large number or a very small number? For this reaction at equilibrium, will there be more reactants or products?

b. Chemical reactions, like water in a riverbed, tend to go downhill. Is your answer in part a consistent with the energy diagram you drew for this reaction in CTQ 47?

c. Which of the following best describes the mathematical relationship between ΔH (in pK_a units) and K_eq?

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 ΔH_rxn, 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?