Would you expect the dissolution of ammoniium nitrate to be spontaneous over all

Question

Would you expect the dissolution of ammoniium nitrate to be spontaneous over all temperatures? if so explain why and if not determine for what temperature ranges the dissolution of ammonium nitrate would be spontaneous? if you can determinea temperature range for non spontaneous disolution of ammoniium nitrate do you think this could be observed experimentally.?

determine the deltaH, delataG^zero ad deltaS^zero values for the dissolution of silver chloride. From this data determine the Ksp for silver chloride. How well does this compare with the Ksp value described in the textbook?

Determine the deltaG^zero for the formation of Cu(NH3)4 ^+2 from copper (II ) ion and ammonia all in aqueous solution. From this calculated value of the standard Gibbs free energy change (deltaGzero rxn) for ths reaction determine the Gibss free energy of formation (deltaGzero f ) of the Cu(NH3)4^+2ION. WOULD you predict that the deltaH zero term or the deltaS zero term is larger if you were to calculate from standard thermodynamic values ( that is from deltaG zero = deltaH zero - TdeltaS zero ? provide a statement that supports your prediction.

Explanation / Answer

NO, we cant expect the dissolution of ammonium nitrate occuring spontaneously at all temperatures.

The dissolution of ammonium nitrate (NH4NO3) occurs spontaneously in water at 25

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