Write the balanced chemical equation for the dissolution of ammonium chloride in

Question

Write the balanced chemical equation for the dissolution of ammonium chloride in water. In the experiment, identify the system and the surroundings Which one gains heat in this experiment? Is the system endothermic or exothermic? Explain how the observed temperature change verifies your answer to #4. From the temperature change obtained for the system in the calorimeter, what must be the sign for delta Hr_rxn? Based on observing the solution in the coffee-cup calorimeter, is the dissolution of ammonium chloride spontaneous or non-spontaneous at room temperature? Based on observing the solution, is delta G > 0 or

Explanation / Answer

Thermodynamics of dissolution of salt in water.

1. Balanced equation, NH4Cl(s) --> NH4+(aq) + Cl-(aq)

2. System : NH4Cl(s) ; surrounding : H2O

3. System gains heat

4. Heat is absorbed : Endothermic

5. The temperature of the initial solution is higher than the temperature after dissolution, such that heat is absorbed in the reaction. This proves reaction is endothermic in nature.

6. Sign of dHrxn (enthalpy) = +ve

7. a) The dissolution reaction is spontaneous

b) dG for the system = < 0

8. Dissolution of 1 NH4Cl(s) produces two NH4+ and Cl- ions, so disorder has increased.

9. The solubility of NH4Cl would decrease with decreasing temperature and increase with increasing temperature.

dHrxn = +ve

dSrxn = +ve

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