When fumes of ammonia and fumes of hydrobromic acid meet, they form a “smoke” of solid ammonium bromide according to the following reaction:                         NH3 (g) + HBr (g) --> NH4Br (s) (a)  Without doing any calculations, do you expect this reaction to occur with an increase or a decrease in entropy?  Explain your answer. (b) Determine ∆Hº, ∆Sº, and ∆

When fumes of ammonia and fumes of hydrobromic acid meet, they form a “smoke” of solid ammonium bromide according to the following reaction:

                        NH3 (g) + HBr (g) --> NH4Br (s)

(a)  Without doing any calculations, do you expect this reaction to occur with an increase or a decrease in entropy?  Explain your answer.

(b) Determine ∆Hº, ∆Sº, and ∆Gº for this reaction.  Is the reaction spontaneous?  Is it exothermic?  Is there an increase or decrease in entropy?

(c) Is there a temperature at which ammonium bromide will spontaneously decompose into ammonia gas and HBr gas?  If yes, what is/are this/these temperature(s)?  If no, why not?