#20 - Chem 165 Chapter 14: Chemical Equilibrium: Class 20...

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Chem 165 Class 20 Suggested End-of-chapter problems for Chapter 14 (today’s material in bold ) Chapter 14: 6, 7, 9, 14, 15, 18, 20, 21, 23, 25, 29, 31, 40, 41, 42, 43, 45, 53 , 57 , 58 , 59 , 60 , 62 (a, b, c, d, g) , 69 , 77, 78 Chapter 14: Chemical Equilibrium: ARIS: Chapter 14-A: assignment due Friday (3/27) at 6:00 pm CDT ARIS: Chapter 14-B: assignment due Monday (3/30) at 6:00 pm CDT Exam 3: Next Wednesday (4/1); 6:30 – 7:30 pm; same seat/room assignments Covers Lectures 13 – 20 [Ch. 13 (Sec. 5 & 6); Ch. 23 (Sec. 1 – 6); Ch. 14 (all)] bjective today: 1. Consider the effects of changing conditions once equilibrium has been reached: LeChâtelier’s Principle Text: Chapter 14: Sections 5 Next class: Chapter 15 (Dr. Zahariev) Caption : The effects of T on the N 2 O 4 2 NO 2 equilibrium, in which the forward reaction is endothermic, demonstrate LeChâtelier’s Principle associated with temperature changes. Low T : N 2 O 4 dominant High T : NO 2 dominant Increase T : [NO 2 ] increases Review sessions (clickers): Sun. (3/29), 6:00 pm, 1002 Gilman Mon. (3/30), 6:00 pm, Physics 5 (note diff. room)
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Chem 165 Class 20 At 100 o C, K c = 0.078 for the reaction SO 2 Cl 2 (g) ' SO 2 (g) + Cl 2 (g) If a mixture of SO 2 Cl 2 (0.108 M), SO 2 (0.052 M) and Cl 2 (0.052 M) were introduced in to a closed vessel at 100 o C, predict whether the reaction is already at equilibrium. If not, which direction the reaction must proceed to achieve the equilibrium? 1. Yes . The reaction is at equilibrium . 2. No . The equilibrium will shift towards reactant .
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This note was uploaded on 10/21/2010 for the course CHEM 155 taught by Professor Burnett,joe during the Fall '08 term at Iowa State.

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#20 - Chem 165 Chapter 14: Chemical Equilibrium: Class 20...

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