Ammonium chloride (NH_4CI) is readily soluble in water. Dissolution of this salt

Question

Ammonium chloride (NH_4CI) is readily soluble in water. Dissolution of this salt in water is an endothermic process (the mix gets cold). Assume that the solution of NH_4CI is formed in a covered glass (closed, but not isolated system), and the glass is located in a very large room with the constant temperature T. After the salt is dissolved, and the system reaches thermodynamic equilibrium (solution warms up to the room T), characterize the change in the enthalpy of the solution, and using the 2nd law of thermodynamics make a suggestion regarding the sign and relative magnitude of the entropy changes and DeltaS_soln, DeltaS_room and DeltaS_universe (where universe = glass with the solution + room).

Explanation / Answer

The enthalpy change is zero because the solvent was at initially temperature T and after the dissolution of ammonium chloride the solution reaches a temperature T. There is no change in temperature which means no change in enthalpy.

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