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Chem 202 test 2 study guide

by: Catherine Montz

Chem 202 test 2 study guide Chem 202

Marketplace > University of Louisville > Chemistry > Chem 202 > Chem 202 test 2 study guide
Catherine Montz
U of L

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These are just example problems you may see on the test. As I state in the study guide, these are only problems that cover what you should have learned in the notes or reading the text book. If you...
General Chemistry 2
Dr. Kuta
Study Guide
chem 202, Study Guide, chemistry 2, Test 2
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This 7 page Study Guide was uploaded by Catherine Montz on Saturday February 27, 2016. The Study Guide belongs to Chem 202 at University of Louisville taught by Dr. Kuta in Spring 2016. Since its upload, it has received 58 views. For similar materials see General Chemistry 2 in Chemistry at University of Louisville.


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Date Created: 02/27/16
CHEM 202 STUDY GUIDE TEST 2 PROFESSOR KUTA CHAPTERS 44-53 For the test it is very important you study the notes I posted and READ THE TEXT BOOK. You can’t rely on just notes and a study guide for a test reading is very important, this study guide is simply practice problems. I want you to study the notes and come into this study guide able to answer the questions I give you. I feel that is one of the most effective ways of studying. What you don’t know, go back to your book or notes and review. There are extra problems located in your text book. Answer key will be attached. Practice Problems True or false?  1) When a system is in equilibrium, Q = K 2) Activities of reactions are unitless  3) For every spontaneous reaction, the drive is to reach G = 0 4) The greatest driving force for any exergonic process is at the start of the process 5) The standard molar entropy of every ion is a negative number  6) K and k measure for the same variable 7) Q will tell you the speed of the reaction while K tells you the direction  8) The sign of S of every sublimation is positive  9)  Evaporation has negative  S 10)For equilibrium Suniv= 0  11)All endothermic reactions are spontaneous  12)At equilibrium G is zero  13)A bimolecular elementary step involves a reaction of two particles  14)As E eincreases, k decreases 15)Reverse activation energies are always greater than forward activation energies 16)A catalyst lowers the H for the overall reaction 17)When you double a chemical equation you square the K value  18)At equilibrium, the forward and reverse speeds of a reaction are equal 19)For an exothermic process, the equilibrium constant will increase at higher temperatures  20)Dilution favors that side of an equation that has more gas or solute particles  1. Which of these has the largest S A) O (g2 B) F (2) C) Br (g2 D) Br (l2 2. Calculate S  (J/Krxnor this reaction  2 FeO(s) + Cl (g)2+ 4 H (aq)  2 Fe (aq) + 2 Cl (aq) + 2 H O(l)­  2 3. Using free energies formation calculate G (kj) for this reaction  PCl (3) + 3 H (g)2  PH (g) + 33HCl(g) 4. PCl (g) + 4 H O(l)  H PO (aq) + 5 HCl(aq) 5 2 3 4 What is H in kJ? What is S in J/K? 5. Calculate normal boiling point for methanol in K using H and S 6. Write the Q expression for the following  A) N O 2g)5+ H O(l) 2 2 HNO (aq) 3 7. Find the Q value for the following conditions in the eqution:  2­ +  0.0156 atm CO       28.72 mol H O      0.2723 M CO      0.0406 M H3 CO (2) + H O(l)2 CO (aq) + 2 3 (l) + 8. Find G for the following at 298.15 Kelvin   P(NO ) = 0.351 atm  P2N O ) = 4.52 atm  2 4 2 NO (g)  N O (g) 2 2 4 9. Calculate K at 298.15 K  2 NO(g) + 2 Cl (g) 2 2 Cl O(g) + N2(g) 2 10. The equilibrium vapor pressure of water at 40 degrees C is 55.4 torr, calculate G vap 11. Calculate the speed relationship for the following  (NH ) CO(aq) + 2 OH(aq)  CO (aq) + 2 NH (aq)­ 2 2 3 3 12. Here is the reaction: C H Cl(g)  C H (g) + HCl(g)        k = 4.7s    at 960 K  ­1 2 5 2 4 What is the rate? What is the rate when C H Cl = 0.082 m5l/l? what is the half­life? 13. Here is the reaction: 2 NO (g)  N2(g) + NO (g) 2 Second order in NO  and k = 0.68 (l/mol)/s  at 500 K ­1 2 The reaction begins with NO  = 0.03442mol/l What concentration of NO  remains?2What concentration of NO has formed? What is the percent completion? 14. I want you to take a look at problem 4 page 527 in the book. It involves an RED. I cannot find a good enough diagram online to make my own question for you, so please take a look I guarantee this WILL BE ON THE TEST.  15. A reaction has an overall H  = ­200 kJand this reaction has two elementary steps. The rxn first one has H  = ­10 kJ and forward E = 80 kJ. Thea1econd has a forward E  = 60 kJ, a2 what is the reverse Ea2 for the second step? 5 16. Here’s the reaction: 2 FeCl (s) + C2 (g)  2 2eCl (s)       and3K = 3.42 x 10 What is K for this equation? : 2 FeCl (s)  2 F3Cl (s) + Cl (g) 2 2 17. Equilibrium system: Br (l) + C2 (g)  2 2rCl(g)    K = 2.2 Find the pressures of Cl  and 2rCl if the process begins with Cl (g) and BrCl(g)2at 1.00 atm 18. Equilibrium system: CO (aq) + 2 F (aq) + H O(l)  CO  (a2) + 2 HF(aq)  3 K = 4.2 x 10 ­11 ­ The process begins with 0.028 M CO  and 0.017 M F2. What are the concentrations of each solute at equilibrium?  19. Consider the following reaction: P 4s) + 12 HCl(g)  4 PCl (g) + 63H (g)      2 H = ­47.08 kJ Will the following actions cause a shift to the right, left, or have no affect a. Add more P 4 b. Increase H  pressure 2 c. Add Ne(g) to increase total pressure  d. Decrease volume of system  ANSWER KEY  True/false  1. T 2. T 3. T 4. T 5. F 6. F 7. F 8. T 9. F 10. T 11. F 12. T 13. T 14. T 15. F 16. F 17. T 18. T 19. F 20. T Short answer problem  1. Br (g) 2 2. 287.51 J/K 3. ­9.10 kJ 4. ­620.6 kJ and ­203.4 J/K 5. 336.3 K N O −¿ 2 3 ¿ 2 6. Q =  +¿¿¿¿ H ¿ ¿ 7. 0.00764 8. 4.20 kJ ­10 9. 2.127 x 10 10. 6.81 kJ −¿ O H ¿ ¿ 32−¿ ¿ C O ¿ ∆[N H ] 11.  speed = ­   =  ¿  =  1 3 ∆ ¿ ∆¿ 2 ∆t ¿ ∆¿ −1 ¿ 2 12. a. rate = k [C 2 C5] b. 0.42 (mol/L)/s c. 0.15 s        13. b. 0.00901 mol/L             c. 0.0127 mol/L             d. 73.8%        14. Answer in book         15. 220. kJ        16. a. 2.92 x 10        17. P(C2 ) = 0.83 atm      P(BrCl) = 1.34 atm         18. [C2 ] = 0.028 M    [F] = 0.017 M    [CO ] 3 4.4 x 10  M  [HF] = 8.8 x 10  M ­6        19. a and c  


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