CHEM 1412 Practice Exam 1 - Chapters Zumdahl

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1 CHEM 1412 Practice Exam 1 - Chapters Zumdahl Some equations and constants: T = Km P = XP = MRT ln[a]t = kt + ln[a]o 1 / [A]t = kt + 1 / [A]o t1/2 = ln(2) / k t1/2 = 1 / k{a]o Kp = Kc(RT) n ln(k1/k2) = (Ea /R) (1/T2 1/T1) R = L atm mole 1 K 1 = J mole 1 K 1 A periodic table is also attached to the end of the exam. For show work problems, you must show your calculations and units clearly for credit or partial credit. Good luck! 1. What is the molarity of a solution prepared by dissolving 10.0 g of KNO3 in 250 ml of solution? 2. What is the molality of a solution made by dissolving 5.00 g of naphthalene, C10H8, in 50.0 ml of ethanol? The density of ethanol is g/ml. 3. How many grams of NaCl are in 250 g of a 15.0% (by weight) solution? 4. A solution of glucose, C6H12O6, has an osmotic pressure of 7.7 atm at 25 C. What is the molarity of this solution?

2 5. Aqueous concentrated nitric acid is 69% HNO3 by weight and has a density of 1.42 g/ml. a) What is the molality of this solution? b) What is the molarity of this solution? 6. The vapor pressure of water at 25 C is torr. What is the vapor pressure at 25 C of a solution prepared by dissolving mole of sucrose in 12.0 moles of water? 7. What pressure of CO2 gas is required to keep a concentration of dissolved CO2 at 0.10 M in a can of soda? The Henry s law constant for CO2 dissolved in water is M/atm at 25 C.

3 8. A saturated solution a) will dissolve additional solute if more solute is added. b) contains no dissolved solute. c) contains dissolved solute in equilibrium with undissolved solid. d) will rapidly precipitate some solid solute if a seed crystal is added. 9. Which one of the following substances will be the most soluble in water? a) KBr b) C10H8 c) CCl4 d) C8H A m solution of which one of the following solutes will have the highest boiling point? a) KNO3 b) Ca(NO3)2 c) Al(NO3)3 d) Na2SO4 11. The freezing point of a 1.0 M solution of NaCl in water is higher than the calculated value that assumes the particle concentration for this solute is 2.0 M. This is due to a) solvation of the ions b) particle concentration greater than 2.0 M c) hydrogen bonding d) occurrence of ion pairing 12. When NaCl dissolves in water, a) the oxygens of the water molecules are attracted to the sodium ions. b) the hydrogens of the water molecules are attracted to the chloride ions. c) the sodium and chloride ions becomes separated due to solvation. d) all of the above are true. 13. What is the freezing point of a solution prepared by dissolving 15 g of KBr in 100 ml of water? The freezing point depression constant, Kf, for water is 1.86 C/m. 14. In the gas phase reaction below, if the rate of formation of NO2 is 8.24 X 10 4 M s 1, what is the rate of disappearance of O2? 4 NH3 + 7 O2 4 NO2 + 6 H2O

4 15. Use the table of data shown below to calculate the value of the rate constant k. The reaction is first order. time (s) [A] (M) The reaction 2NO (g) + Br2 (g) 2NOBr (g) is second order with respect to NO and first order with respect to Br2. Which is the correct rate law for this reaction? a) Rate = k[no][br2] b) Rate = k[no] 2 [Br2] c) Rate = k[nobr] 2 d) Rate = k[no][br2] The correct units for the rate constant k in the rate law Rate = k[a] 2 [B] are a) M s 1 b) M 1 s 1 c) M 2 s 1 d) M 1 s The rate law for the aqueous reaction H2SeO3 + 6 I + 4 H + > Se + 2 I3 + 3 H2O is Rate = k[h2seo3][i ] 3 [H + ] 2. By what factor will the rate increase if we double the concentrations of all three reactants? a) 8 b) 32 c) 64 d) Given the rate data below for the reaction 2A + 3B Products, what is the rate law for this reaction? Exp. [A], M [B], M Rate, M sec X X X 10 5 a) Rate = k[a][b] b) Rate = k[a] 2 [B] c) Rate = k[a] 2 [B] 2 d) Rate = k[a][b] When the concentration of a reactant was M, the rate of the reaction was 8.42 X 10 6 M s -1. When the concentration of the reactant was doubled to M, the rate increased to 1.59 X 10 5 M s 1. What is the order of the reaction with respect to this reactant (the value of x in the rate law) to three significant figures?

5 21. For a first order reaction, a plot of vs. time gives a straight line with a slope of k. For a second order reaction, a plot of 1/[A]t vs. time gives a straight line with a slope of. 22. The half-life of iodine-131, a radioactive isotope of iodine, is 8.04 days. If an iodine-131 solution is initially M, what will the concentration be after 60 days? Radioactive decay is a first order process. 23. A substance that forms in one step and is consumed in another step of a multistep reaction is a) a transition state b) an intermediate c) a catalyst d) a final product 24. Which of the following will lower the activation energy for a reaction? a) increasing the concentrations of reactants b) raising the temperature of the reaction c) adding a catalyst d) increasing the total pressure 25. The reaction NO2 + CO NO + CO2 follows the rate law Rate = k[no2] 2. In the mechanism below, a) which step is the rate-limiting step? b) which substance is an intermediate in the reaction? Step 1 NO2 + NO2 > NO3 + NO Step 2 NO3 + CO > NO2 + CO2 26. In any multistep reaction mechanism, the rate of the overall reaction is determined by the rate of the step in the mechanism. a) first b) last c) slowest d) fastest 27. At equilibrium a) All chemical processes have ceased. b) The rate of the forward reaction equals the rate of the reverse reaction. c) The rate constant for the forward reaction equals the rate constant of the reverse reaction. d) The concentration of the products is greater than the concentration of the reactants.

6 28. The equilibrium constant Kp for reaction (1) has a value of What is the value of the equilibrium constant for reaction (2)? (1) SO2 (g) + 1/2 O2(g) SO3 (g) Kp = (2) 2 SO3 (g) 2 SO2 (g) + O2 (g) Kp =? a) b) 2.24 c) 44.2 d) Kc = 278 for the reaction 2 SO2 (g) + O2 (g) 2 SO3 (g) at 1000 K. What is the value of Kp? a) b) c) 54.7 d) The reaction NH4HS (s) NH3 (g) + H2S (g) has Kc = 1.2 X 10 4 at 22 C. If a solid sample of NH4HS is placed in a closed container and allowed to decompose until equilibrium is reached, what will the equilibrium concentrations of NH3 and H2S be? a) M b) 0.28 M c) M d) 0.14 M 31. Consider the following reaction at equilibrium: N2 (g) + 3 H2 (g) 2 NH3 (g) H = kj The forward ( ) reaction should be favored by using conditions of a) high temperature and high pressure b) high temperature and low pressure c) low temperature and low pressure d) low temperature and high pressure

7 32. Write the equilibrium constant expression for the reactions below: a) CO2 (g) + H2 (g) CO (g) + H2O (l) b) SnO2 (s) + 2 CO (g) Sn (s) + 2 CO2 (g) c) 3 Fe (s) + 4 H2O (g) Fe3O4 (s) + 4 H2 (g) d) 6 CO2 (g) + 6 H2O (l) C6H12O6 (s) + 6 O2 (g)

8 33. Consider the following chemical reaction: H2 (g) + I2 (g) 2 HI (g) Kc = 49.5 at 440 C a) If the equilibrium concentrations of H2 and I2 are 0.25 M each, what is the equilibrium concentration of HI? b) If we start with H2 and I2 at 0.25 M each, what will the HI concentration be at equilibrium? c) If we start with H2 at 0.65 M, I2 at 0.65 M, and HI at 5.00 M, what is the value of Qc? Which way with the reaction go (forward, reverse, or no change) in order to react equilibrium?

9 34. At 25 C a reaction has a rate constant of s 1. What is the value of the rate constant at 100 C? The activation energy for the reaction is 70.0 kj/mol. 35. The molar mass of an unknown molecular solute is determined by dissolving 2.50 g of the compound in 50.0 g of benzene. The freezing point of the solution was 1.50 C lower than that of pure benzene. The freezing point depression constant, Kf, for benzene is 5.00 C/m. What is the molecular weight of the compound?

10 Answers M m g M 5. a) 35.3 m b) 15.5 M torr atm 8. C 9. A 10. C 11. D 12. D C X 10 3 M/s 15. k = s B 17. C 18. C 19. B 20. x = ln[a] t, k X 10 4 M 23. B 24. C 25. a) Step 1 b) NO C 27. B 28. D 29. D 30. C 31. D 32. a) K eq = [CO (g)] / [CO 2 (g)][h 2 (g)] b) K eq = [CO 2 (g)] 2 / [CO (g)] 2 c) K eq = [H 2 (g)] 4 / [H 2 O (g)] 4 d) K eq = [O 2 (g)] 6 / [CO 2 (g)] a) [HI] eq = 1.76 M b) [HI] eq = M c) Q c = > 49.5 The reverse reaction will occur until equilibrium is reached. Q c > K c 34. k 2 = 102 s Molecular weight = 167 g/mol

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