The dissolution of ammonium nitrate occurs spontaneously in water at 25°c. as nh4no, dissolves, the temperature of the water decreases. what are the signs of ah, as, and ag for this process? a. ah> 0, as > 0, ag > 0 b. ah> 0, as > 0, ag

ΔG <0 , ΔH > 0 , ΔS > 0 .

Explanation:

From the data given in question , the reaction is a spontaneous process , hence , the value of change in gibbs free energy would be negative , ΔG <0

And , on dissolution process , the temperature of the water decreases , i.e. , it is an endothermic process , i.e. , the change in enthalphy value is positive , ΔH > 0

And , during the process of dissolution , the ammonia salt break does to ions , i.e. , the randomness increases , hence the ΔS > 0

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