Chem Chemistry 111: Penn State Altoona Name: _________________ Report Form: Expt.8 Calorimetry Date: __________________ XXXXXXXXXXPartners Name: _________________ Fill in the table below Type of...

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Chem Chemistry 111: Penn State Altoona Name: _________________ Report Form: Expt.8 Calorimetry Date: __________________ Partners Name: _________________ Fill in the table below Type of Reaction Observation Sign of q ∆H PROCEDURE: Part A: Heat of Neutralization of NH3(aq) and HCl(aq) 1. Chemical Equation for ∆Hneut: _________________________________________________ 2. Units for Molarity: Molarity = ____________________________________ Chemical Name Chemical Formula Volume (mL) Molarity Acid or Base or Neutral Ammonia Hydrochloric Acid Ammonia Chloride XXXXXXX Calculation of ∆Hneut from graphs Show Calculation here for ∆Hneut-(Tfinal – Tinitial) from graphs Show Calculation here for Mass of Final solution of NH4Cl:(Final vol. X Density of water) : Show Calculation w/ units here for (convert to KJ) ( )( )final initial 4.184 J Amont of heat _____ g combined solutions g C   = =  = −    q sm T T T Determination of the limiting reactant and moles of product Show Calculation with units for H neut system neut moles product q H = Is this exothermic or endothermic? ____________________ Should this value positive or negative?_______________ Part B. Heat of Solution of NH4Cl(s) Calculation of qsystem Solution reaction: NH4Cl (s) → NH4Cl (aq) 100.0 mL Calculation of ∆H(solution) from graphs Show Calculation here for T(Tfinal – Tinitial) from graphs Show Calculation here for Mass of Final solution of NH4Cl:(Final vol. X Density of water) : Show Calculation here for Average: Amount of heat = ? = ??Δ? = ( 4.184 J g °? ) (_____ g combined solutions + 8.XXXXg)(?final − ?initial) Show Sample Calculation for Moles of NH4Cl? Use mass of ammonium chloride and molar mass Show Sample Calculation H(solution) = q / moles of NH4Cl (experiment) Part C. Calculation of Standard Enthalpy of Formation of Solid Ammonium Chloride using Hess’s Law Reaction (kJ mol-1) I. NH3 (aq, ____M) + HCl (aq, _____M) → NH4Cl (aq, ____M) ∆H(neut) ______ II. NH4Cl(s) → NH4Cl (aq, _____M) ∆H(soln) ______ III. 1/2 N2(g) + 3/2 H2(g) → NH3(g) ∆H – 45.77 IV. 1/2 H2(g) + 1/2 Cl2(g) → HCl(g) ∆H – 92.31 V. NH3(g) → NH3(aq, 1.5M) ∆H – 35.40 VI. HCl(g) → HCl (aq, 1.5M) ∆H –72.84 Final Reaction : ∆Hf  : ½ N2 (g) + ½ Cl2 (g) + 2 H2 (g) → NH4Cl (s) Reorder steps below using Hess’s Law to find ∆Hf of NH4Cl (s) IV. Error Analysis True: Accepted value of ∆Hf [NH4Cl (s)] DH f o = –313.29 kJ mol-1 Reference CRC Handbook of Chemistry and Physics, Robert C Weast p D-67