When solid `NH_(4)NO_(3)` is dissolved in water at `25^(@)C`, the temperature of the solution decreases. What is true about the signs of `DeltaH and DeltaS` for this process?

When solid CuSO_(4) dissolves in water to make a 1 M solution, the temperature of the system increases When solid NH_(4)NP_(3) dissolves in water to make a 1M solution, the temperature of the system decreases. Which statement(s) mus be correct for these dissolving processes? (P) DeltaH^(@) value for both processes have the same sign. (Q) DeltaG^(@) values for both processes have the same sign.

An ionic compound ha a solublity increases as the temperature is raised. What are the signs of DeltaH^(@) and DeltaS^(@) for the dissolving process?

What will be the signs of DeltaH and DeltaS when NaOH is dissolved in water?

What will be the signs of DeltaH and DeltaS when NaOH is dissolved in water?

The decomposition of solid ammonium carbamate, (NH_(4))(NH_(2)CO_(2)) , to gaseous ammonia and carbon dioxide is an endothermic reaction. 9NH_(4))(NH_(2)CO_(2)))(s)hArr2NH_(3)(g)+CO_(2)(g) (a) When solid (NH_(4))(NH_(2)CO_(2)) is introduced into and evacuated flask at 25^(@)C , the total pressure of gas at equilibrium is 0.3 atm. What is the value of K_(p) "at" 25^(@)C ?

The number of ions formed when [Cu(NH_(3))_(4)]SO_(4) is dissolved in water is