Question

Solid ammonium nitrate, NH4NO3 (s), dissolves spontaneously in water at 25oC,

NH4NO3 (s) → NH4+ (aq) + NO3- (aq)

If this process is endothermic, which of the following is most likely TRUE?

Answer 1

A) ΔG > 0

B) ΔG = 0

C) ΔS > 0

D) ΔS < 0

E) ΔS = 0

F) ΔH < 0

Answer 2

Well, delta H is >0
And spontaneous the reaction delta G must be < 0.

H-TDeltaS that means t delta s has to be larger than H for delta G to be negative so delta S has to be >0

Answer 3

In an endothermic reaction Delta H is positive ( the products in an endothermic reaction absorbs heat from the surrounding therefore the heat from products increases resulting the Delta H to be positive. )
In an exothermic reaction the delta H is negative ( here it is the other way round)

Answer 4

G>0 non spontaneous reactions
G<0 spontaneous reactions
G=0 reactions which are in equilibrium.
Since this says that the reaction is spontaneous G<0

Answer 5

\[\Delta G = \Delta H - T \Delta S\]
We have already found that delta G is negative and delta H is positive therefore delta S is positive