Use The Following Information To Answer The Next Two Questions A Chemistry Student Wanted To Determine The Molar Enthalp 1 (346.15 KiB) Viewed 72 times
Use The Following Information To Answer The Next Two Questions A Chemistry Student Wanted To Determine The Molar Enthalp 2 (321.07 KiB) Viewed 72 times
Use the following information to answer the next two questions A chemistry student wanted to determine the molar enthalpy of formation for pentan- 1-01 (C5H11OH()). He set out to experimentally determine the molar heat of combustion of pentan-1-ol using calorimetry and then by manipulating known enthalpies he could determine the molar enthalpy of formation for pentan-1-ol. In order to determine the enthalpy change for the combustion of pentan-1-ol, the chemistry student bumed 0.900 g of pentan-1-ol in a homemade calorimeter. The following data was collected. Mass of water (g) Highest Temperature of H₂O(1) (°C) Initial Temperature of H₂O() (°C) Change in Temperature (°C) Your answer. Trial #1 250.0 49.0 21.0 Using the Calorimetry Data above, calculate the molar enthalpy for the combustion of pentan-1-ol as shown in equation 3. (3 marks)
Use the following additional information to answer the next question Overall Equation 5 C(s) + 6 H₂(g) + ½ O2(g) C5H11OH(1) AH = Given equations: Equation 1: C(s) + O₂(g) → CO₂(g) AH = Equation 2: H₂(g) + O2(g) → H₂O(1) AH = ½ Equation 3: C5H11OH(1) + 15/2 O2(g) → 5 CO₂(g) + 6 H₂O(1) AcH = Using Hess' Law and your answer from the previous question, calculate the enthalpy of formation for pentan-1-ol as shown in the overall equation. (3 marks) AƒH = Your answer. KJ
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