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1 Exam 2 CHEM Name (print legibly) Seat no. Signed On my honor, I have neither given nor received unauthorized aid on this exam. Date 30 questions/3.33 points each Indicate the BEST answer for the questions in this section by completely filling in the appropriate space on the answer card with a #2 pencil. Mark only one space per question. 1. For the reaction: Ag(s) + NO 3 (aq) Ag + (aq) + NO(g) the oxidizing agent is a. Ag(s), since silver increases in oxidation number b. NO 3 (aq), since nitrogen increases in oxidation number c. NO 3 (aq), since oxygen increases in oxidation number d. NO 3 (aq), since nitrogen decreases in oxidation number e. NO 3 (aq), since oxygen decreases in oxidation number 1 2. The oxidation number of P in H 4 P 2 O 7 is a. +9 b. +7 c. +5 d. +3 e CuCl Cu + CuCl 2 is best classified as what type of reaction? a. metal displacement b. acid/base c. halogen displacement d. disproportionation e. combination 4. How many ml of a 2.00 M HCl solution is needed to prepare 500 ml of a M HCl solution? a b. 250 c. 125 d e. 375

2 2 5. How many ml of a M KMnO 4 solution is needed to titrate g of KNO 2 (molar mass = 85.1). The balanced net ionic equation for this reaction is 5 NO MnO 4 + 6H + 2 Mn NO H 2 O a b c d e An ideal gas at 20 C and 2.0 atm pressure occupies a volume of 5.0 L. Calculate the volume (in L) occupied by this gas at 50 C and the same pressure. a. 5.5 b c. 4.5 d e Which of the following gases will have the greatest density at the same specified temperature and pressure? a. CO b. CO 2 c. SO 2 d. SO 3 e. H 2 8. A 2.00-L sample of pure HCl gas at 300 K and atm was dissolved in water. It took 20.3 ml of a NaOH solution to completely neutralize the aqueous HCl. The molarity of the NaOH solution is a b c d e

3 9. A 2.27-g sample of an unknown gas occupies 1.0 L at 300 K and 1.0 atm. The empirical formula of the compound is CH 2. What is the molecular formula of the compound? 3 a. CH 2 b. C 2 H 4 c. C 3 H 6 d. C 4 H 8 e. C 5 H A sample contains only two gases: nitrogen at 1.6 atm pressure and oxygen at 0.40 atm pressure. The mole fraction of oxygen is a b c d e For the reaction 2NO(g) + O 2 (g) 2NO 2 (g) what volume of oxygen gas at 320 K and atm will react completely with 6.0 L of NO gas at the same temperature and pressure? a. 1.0 b. 3.0 c d. 6.0 e An isolated system a. allows the transfer of both mass and energy. b. allows the transfer of mass but not energy. c. allows the transfer of energy but not mass. d. does not allow the transfer of either mass or energy. e. always operates under conditions of constant pressure. 13. A 100-g block of aluminum (specific heat = J/g C) at C is placed in 1,000 g of a liquid at 20.0 C. If the final temperature of the system is 27.0 C, calculate the specific heat of the liquid. Assume no heat is lost to the surroundings or to the vessel containing the liquid. a b c d e. 4.18

4 4 14. A gas expands in volume from 0.50 L to 0.75 L against a constant pressure of 2.0 atm. The work done in J (1 L atm = J) is a. No work is done, since the pressure is constant. b J, since work is done by the system on the surroundings. c. 51 J, since work is done by the system on the surroundings. d J, since work is done by the surroundings on the system. e. 51 J, since work is done by the surroundings on the system. 15. For which of the following reactions does ΔH o reaction equal ΔH o f? a. H 2 (g) + S(rhombic) H 2 S(g) b. C(diamond) + O 2 (g) CO 2 (g) c. H 2 (g) + CuO(s) H 2 S(g) d. O(g) + O 2 (g) O 3 (g) e. 2H(g) + O(g) H 2 O(g) 16. Use the following equations C(graphite) + O 2 (g) CO 2 (g) ΔH = 394 kj 2CO(g) + O 2 (g) 2CO 2 (g) ΔH = 566 kj to calculate the enthalpy change (in kj) for the reaction 2C(graphite) + O 2 (g) a. 222 b c. 960 d e CO(g) 17. Under what conditions is the heat change in a system the same as the enthalpy change? a. constant volume and constant temperature b. constant pressure c. constant temperature d. No work is done. e. constant volume

5 18. The frequency of light (in s 1 ) having a wavelength of 456 nm is 5 a x b x 10 5 c x 10 4 d x e x What is the frequency of light (in s 1 ) having an energy content of 500 kj/mol? a x b x c x d x e x The spectral region associated with light of 500 nm is the a. ultraviolet b. visible c. infrared d. microwave e. radiowave 21. Which of the following changes in electron configuration would result in emission of a photon? a. 1s 2 2s 2 2p 4 changes to 1s 2 2s 1 2p 5 b. 1s 2 2s 2 2p 3 changes to 1s 2 2s 0 2p 5 c. 1s 2 2s 2 changes to 1s 2 2s 1 d. 1s 2 2s 2 2p 6 3s 2 3p 0 changes to 1s 2 2s 2 2p 6 3s 1 3p 1 e. 1s 2 2s 2 2p 6 3s 1 3p 4 changes to 1s 2 2s 2 2p 6 3s 2 3p The ground state electron configuration of Ti is a. [Ar]4s 2 3d 2 b. [Ar]3d 4 c. [Ar]4s 2 4p 2 d. [Ar]3s 2 3d 2 e. [Ar]4s 2 4d 2

6 23. Which of the following is not an allowed set (n, l, m l, m s ) of quantum numbers? 6 a. 1, 1, 0, 1 2 b. 2, 1, 0, 1 2 c. 3, 2, 1, 1 2 d. 3, 0, 0, 1 2 e. 2, 1, 1, Which of the following pairs are isoelectronic? a. V 5+, Cl b. B 3+, F c. Se +, Br + d. Cu 2+, Zn + e. P 3+, S The orbitals pictured above are best described (from left to right) as a. d xz, p y, s b. d xz, p z, s c. p y, p x, s d. d xz, p x, s e. d xz, p xy, s 26. Which of the following has the most unpaired electrons? a. C b. C c. C 2 d. C 3 e. C 4

7 7 27. For an orbital with m l = 4, what is the minimum value allowed for n? a. 6 b. 5 c. 4 d. 3 e An element with the electron configuration [Xe]6s 2 4f 9 is a(n) a. noble gas. b. halogen. c. alkali metal. d. lanthanide (Z = 57 71). e. actinide (Z = ). 29. The ground state electron configuration of Fe 3+ is a. [Ar]4s 2 3d 3 b. [Ar]4s 2 4p 3 c. [Ar]4p 5 d. [Ar]3d 5 e. [Ar]3d Of the following, which has the largest radius? a. O 2 b. O c. S 2 d. Se 2 e. Se

8 8 1A 8A (1) (18) 1 R = L atm/mol K 2 1 H 2A 62.4 L torr/mol K 3A 4A 5A 6A 7A He (2) (13) (14) (15) (16) (17) h = 6.63 x J s Li Be B C N O F Ne c = 3.00 x 10 8 m/s Na Mg 3B 4B 5B 6B 7B.....8B. 1B 2B Al Si P S Cl Ar (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe (98) Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn (209) (210) (222) Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg (223) (226) (227) (261) (262) (266) (264) (277) (268)? (272) Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (145) Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262)

1s 1. [He]2s 1. [He]2s 2. [He]2s 2 2p 2. [He]2s 2 2p 1. [He]2s 2 2p 4. [He]2s 2 2p 3. [He]2s 2 2p 6. [He]2s 2 2p 5

1s 1. [He]2s 1. [He]2s 2. [He]2s 2 2p 2. [He]2s 2 2p 1. [He]2s 2 2p 4. [He]2s 2 2p 3. [He]2s 2 2p 6. [He]2s 2 2p 5 Symbol: He Atomic Number: 2 Molar Mass: 4.003 g/mol Electronegativity: - 1s 2 Symbol: H Atomic Number: 1 Molar Mass: 1.008 g/mol Electronegativity: 2.20 1s 1 Symbol: Be Atomic Number: 4 Molar Mass: 9.012

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