Question

4. You will conduct the two solvation reactions and three neutralization reactions in this experiment. In the space provided below, write the balanced net ionic reaction equations from the descriptions. Use the table of thermodynamic data in your text (AHf(NaOH(s)= -425.61 kJ-mol) to calculate the molar enthalpy of the reactions. These will be the accepted values you will compare to the experimental values you calculate using data collected during the experiment. Part I: Solid sodium hydroxide is combined with water to form an aqueous sodium hydroxide solution. Sodium hydroxide dissociates into its hydrated ions. Part II: Solid ammonium chloride is combined with water to form an aqueous ammonium chloride solution. Ammonium chloride dissociates into its hydrated ions. Part III: An aqueous solution of sodium hydroxide reacts with an aqueous solution of hydrochloric acid, yielding water. Part IV: An aqueous solution of sodium hydroxide reacts with an aqueous solution of ammonium chloride, yielding aqueous ammonia, NH3, and water. Part V: An aqueous solution of hydrochloric acid reacts with aqueous ammonia, NH3, yielding aqueous ammonium chloride. Balanced reaction equation AH (kJ/mol) Reaction 1 2 4 5 LO

Answer 1

Σn. a H AHAN Reactant produets Na OH Na OH 240.34 - 23 o kJ mal 34)+230)--4250) 24o |AH - 44.73 kJ mo 2.. NH,CA - 314.4 KT -133-2 kJ mo mol -133-2)+1< -05) -- (-314,) 4.O6 kT mol

NaOe 3. - 230K3 - 28S 83 KJ mol mal C-230-C) 2 85.83) -SS.83 AH N 4. Na OH AH. -133-26 k3 - 285-83 KJ mol AH AH 315 kJ mo A H 3.4

Ht S. NH NH -13 3-2 kJ 133 26)C 80 -9) - 52. 36 KS AH