`NH_(4)CI(s) + aq rarr NH_(4)^(+)(aq) + CI^(-1)(aq)`
`DeltaH=+15.1 KJ mol^(-1) NH_(4)CI(s)` dissolves in water according to above equation

Consider the reaction for the dissolution of ammonium nitrate : NH_(4)NO_(3)(s) to NH_(4)^(+)(aq) + NO_(3)^(-)(aq) DeltaH = +28.1 kJ mol^(-1), DeltaS = 108.7 J K^(-1)mol^(-1) . Calculate the change in entropy of the surroundings and predict whether the reaction is spontaneous or not at 25^(@)C ?

Consider the reaction for the dissolution of ammonium nitrate: NH_(4)NO_(3)(s) rarr NH_(4)^(o+)(aq) +NO_(3)^(Theta) (aq) DeltaH =+29.8 KJ mol^(-1), DeltaS = 108.0 J K^(-1) mol^(-1) . Calculate the change in entropy of the surroundings and predict whether the reaction is spontaneous or not at 25^(@)C ?

Consider the reaction for the dissolution of ammonium nitrate: NH_(4)NO_(3)(s) rarr NH_(4)^(o+)(aq) +NO_(3)^(Theta) (aq) DeltaH =+29.8 KJ mol^(-1), DeltaS = 108.0 J K^(-1) mol^(-1) . Calculate the change in entropy of the surroundings and predict whether the reaction is spontaneous or not at 25^(@)C ?

Given the equilibrium system NH_(4)Cl(s)hArr NH_(4)^(+)(aq)+Cl^(-)(aq) (DeltaH=+"3.5 kcal/mol"). What change will shift the equilibrium to the right?

Given the equilibrium system NH_(4)Cl(s)hArr NH_(4)^(+)(aq)+Cl^(-)(aq) (DeltaH=+"3.5 kcal/mol"). What change will shift the equilibrium to the right?

Given the equilibrium system NH_(4)Cl(s)hArr NH_(4)^(+)(aq)+Cl^(-)(aq) (DeltaH=+"3.5 kcal/mol"). What change will shift the equilibrium to the right?

Given the equilibrium system : NH_(4)Cl(g) hArr NH_(44)^(+)(aq)+Cl^(-)(aq), (DeltaH = + 35 kcal // mol ). What change will shift the equilibrium to the right ?

NH_(4)Cl(s) +H_(2)O rarr NH_(4) Cl (aq) DeltaH=16.3 kJ DeltaH in the above reaction represents

NH_(4)CI on heating with NaOH liberates