Final answer:
In the acid-base reaction between HBr and NH3, HBr donates a proton to NH3, forming NH4+ and Br-. Equilibrium favors the formation of these products because a stronger acid and base are producing weaker conjugates. The direction of equilibrium is towards the products NH4+ and Br-.
Step-by-step explanation:
Acid-Base Reaction of HBr and NH3
In an acid-base reaction of HBr (hydrobromic acid) and NH3 (ammonia), we consider HBr as the acid and NH3 as the base according to the Brønsted-Lowry definition. The acid donates a proton (H+) to the base, which accepts it, forming NH4+ (the conjugate acid of NH3) and Br− (the conjugate base of HBr). The curved arrow will be drawn from the hydrogen atom of HBr to the nitrogen atom of NH3 to represent the transfer of the proton.
Regarding the direction of equilibrium, since HBr is a strong acid and NH3 is a weak base, the reaction tends to form a weaker acid (NH4+) and a weaker base (Br−). This means that the equilibrium will lie to the right favoring the formation of the products. The reaction is represented with double arrows to indicate that the reaction can proceed in both the forward and reverse directions, although the forward reaction is favored in this case.
Ultimately, the reaction proceeds to equilibrium in the direction of the weaker acid and base, which in this case is from HBr and NH3 to NH4+ and Br−. This is depicted with a longer equilibrium arrow pointing towards the products, symbolizing their dominance at equilibrium.