EXPERIMENT #9 DETERMINING THE ENTHALPY OF A CHEMICAL REACTION Used 50ml of NaOH. Reactions are…

EXPERIMENT #9 DETERMINING THE ENTHALPY OF A CHEMICAL REACTION

Used 50ml of NaOH. Reactions are provided in second picture.

Computer 13 14. Conduct this reaction in a fume hood or in a well-ventilated area. Repeat Step 10 to conduct the reaction and collect temperature data. DATA TABLE Reaction 2 Reaction 3 Reaction 1 Maximum temperature ('c) 35.5 C 322.47 35,6C Initial temperature (“C) Temperature change (AT) |1니 13Yoll'ugoC | 03 DATA ANALYSIS 1. Calculate the amount of heat energy, g, produced in each reaction. Use 1.03 g/mL for the density of all solutions. Use the specific heat of water, 4.18 J/(g C), for all solutions. 2 Calculate the enthalpy change, Alf, for each reaction in ge, A/, for each reaction in terms of kJ/mol of each reactant. 3. Use your answers from 2 above and Hess's law to determine the experimental molar enthalpy for Reaction 3. 4. Use Hess's law, and the accepted values of AH in the Pre-Lab Exercise to calculate the AFI for Reaction 3. How does the accepted value compare to your experimental value? 5. Does this experimental process support Hess's law? Suggest ways of improving your results. of the reactions ag ucous solution of sodium hydroxide reacts with an aqueous solution of lution of sodium hydroxide reacts with an aqueous solution of Reaction 1: An s hydrochloric acid, yielding water RC Reaction 2: An áqueous so ammonium chloride, yielding aqueous ammonia, NH3, and water. Reaction 3: An aqueous solution of hydrochloric acid reacts With aqueous ammonia, NHs, yielding aqueous ammonium chloride ΔΗ (kJ/mol) Reaction Balanced reaction equation -58 ke 2 O. -133.3 3 PROCEDURE Computer 13 14. Conduct this reaction in a fume hood or in a well-ventilated area. Repeat Step 10 to conduct the reaction and collect temperature data. DATA TABLE Reaction 2 Reaction 3 Reaction 1 Maximum temperature ('c) 35.5 C 322.47 35,6C Initial temperature (“C) Temperature change (AT) |1니 13Yoll'ugoC | 03 DATA ANALYSIS 1. Calculate the amount of heat energy, g, produced in each reaction. Use 1.03 g/mL for the density of all solutions. Use the specific heat of water, 4.18 J/(g C), for all solutions. 2 Calculate the enthalpy change, Alf, for each reaction in ge, A/, for each reaction in terms of kJ/mol of each reactant. 3. Use your answers from 2 above and Hess's law to determine the experimental molar enthalpy for Reaction 3. 4. Use Hess's law, and the accepted values of AH in the Pre-Lab Exercise to calculate the AFI for Reaction 3. How does the accepted value compare to your experimental value? 5. Does this experimental process support Hess's law? Suggest ways of improving your results.

of the reactions ag ucous solution of sodium hydroxide reacts with an aqueous solution of lution of sodium hydroxide reacts with an aqueous solution of Reaction 1: An s hydrochloric acid, yielding water RC Reaction 2: An áqueous so ammonium chloride, yielding aqueous ammonia, NH3, and water. Reaction 3: An aqueous solution of hydrochloric acid reacts With aqueous ammonia, NHs, yielding aqueous ammonium chloride ΔΗ (kJ/mol) Reaction Balanced reaction equation -58 ke 2 O. -133.3 3 PROCEDURE

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