Chem_30_Unit_1_Module_1_Lesson_8_Assignment

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Chemistry 30: Module 1: Lesson 8 1 Assignment Booklet MODULE 1: LESSON 8 ASSIGNMENT Total /34 Read all parts of your assignment carefully, and record your answers in the appropriate places. If you have difficulty with an assignment, go back to the textbook and review the appropriate lesson. Be sure to proofread your answers carefully before submitting your Assignment. Lesson 8 Assignment: Concepts from Lessons 6, 7, and 8 1. Calculate the enthalpy of reaction (NOT molar enthalpy) for the combustion of ethene (5 marks) . [ -1323 kJ OR -1411 kJ – only one of these is correct ] Answer: C2H4+3O2=2CO2 +H2O 52.4+0-2(-393.5)+2(-241.8) =-1323 kJ 2. Use your answer to question 1 to answer the following questions. a. Express the enthalpy of reaction calculated in question 1 as a molar enthalpy of reaction per mole of carbon dioxide (2 marks) . Answer: -1323 kJ/2mol = =-661.5 b. Express the reaction enthalpy calculated in question 1 by writing it as a term in the balanced chemical equation (2 marks). Answer: C2H4+3O2=2CO2+2H2O+1323kJ c. Draw an energy diagram to describe the change in chemical potential energy that occurs in this reaction. Label important parts of your diagram (4 marks) .
Chemistry 30: Module 1: Lesson 8 2 Assignment Booklet d. Indicate whether the reaction is exothermic or endothermic, and justify your answer by making reference to relevant concepts (2 marks) . Answer: Its an exothermic reactions, since it releases heat 3. Use the information contained in “Lab Exercise 11.B” on page 506 in the textbook to answer the following questions. a. Use the reaction equations and reaction enthalpies shown in the introduction section to calculate the following: a reaction enthalpy for the combustion of pentane (3 marks) a molar enthalpy of combustion for pentane (1 mark) [ 3488.7 kJ and 3488.7 kJ/mol ] Answer: Q= (4.19 J/g )(1.24kg)(37.6-18.4) =99.8 deltarH = -99.8 2.15g x 1/72.17 = 0.0297mol -99.8/0.0297 = -3348.6 kJ/mol b. Use the calorimetric data provided to calculate a molar enthalpy of combustion for pentane (3 marks) . [ 3.35 x10 3 kJ/mol ] Answer: deltahHm = -(1.24kg)(4.19)(19.2)/(0.0297) = 3.35X10^3 kJ/mol c. Calculate the percentage error between the value calculated in question 3.a (theoretical value) and the value calculated in question 3.b (experimental value) . (2 marks) [ 3.98 % ] Answer:
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