= J K. 1. Which sample contains the fewest atoms? a. 10 g of C b. 10 g of Ne c. 10 g of H d. 10 g of O. ANSWER: b

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1 CHEM 101 Fall 07 Final Exam On the answer sheet (scantron) write your Name, Student ID Number, and Recitation Section Number. Choose the best (most correct) answer for each question AND ENTER IT ON YOUR ANSWER SHEET. Potentially useful data: Avogadro s Constant: mol -1 The speed of light is: c = m/s. The Planck constant is: h = J s. The Rydberg constant is: R H = J. 2 ΔE = - R H (1/n f 1/n 2 i ) E = hc/λ = hν q = c m ΔT 1.0 atm = 760 Torr = 760 mm Hg R = L atm K -1 mol -1-1 = J K -1 mol 1. Which sample contains the fewest atoms? a. 10 g of C b. 10 g of Ne c. 10 g of H d. 10 g of O 2. Which of the following is not an ionic compound? a. CaSO 4 b. MgO c. CH 4 d. LiF 3. The Roman numerals in the reaction given represent the coefficients in the balanced chemical equation. What are the values of the coefficients? I II III IV a b c d I Ni(ClO 4 ) 2 + II K 2 S III KClO 4 + IV NiS 4. In the reaction given below, how many grams of C 14 H 9 Cl 5 will be produced by the reaction of 25.0 g of each of the starting materials? Page 1 of 7

2 a g b. 25 g c g d g C 2 HOCl C 6 H 5 Cl C 14 H 9 Cl 5 + H 2 O 5. Which of the following is determined by the limiting reactant? a. percent yield b. theoretical yield c. actual yield d. stoichiometric coefficients 6. Which substance is oxidized in the reaction below? a. Na + b. PbO c. NaNO 3 d. Pb NaNO 3 + Pb 7. What is the oxidation number of N in NH 4 +? a. 3 b. 1 c. 0 d. +1 NaNO 2 + PbO 8. Light has a wavelength of 582 nm. What is its frequency? a Hz b Hz c Hz d Hz 9. A yellow light with a wavelength of 580 nm does not result in the emission of electrons from a metal surface. Which of the following is most likely to eject electrons from the metal? a. light with a wavelength of 450 nm b. light with a wavelength of 650 nm Page 2 of 7

3 c. light with a lower frequency d. light with the same wavelength but higher amplitude 10. Determine the wavelength of yellow light with an energy of J. a nm b. 500 nm c. 573 nm d nm 11. How much energy is released when an electron goes from n = 4 to n = 2 in a hydrogen atom? a J b J c J d J 12. Which statement regarding the Bohr model of the atom is true? a. An element produces a continuous spectrum. b. Electrons cannot be located between energy levels. c. Light is emitted when an electron moves from the ground state to an excited state. d. Electrons in the lowest energy level are in an excited state. 13. How many orbitals are contained in the 4d subshell? a. 2 b. 5 c. 10 d Give the element that has the electron configuration: a. Pd b. Fe c. Ni d. Sr 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 5s 2 Page 3 of 7

4 15. Which of the following elements has the largest atomic radius? a. Mg b. Si c. P d. N 16. If heat is transferred from the system to the surroundings, then a. the process is endothermic b. the process is exothermic c. the system must be doing work d. the surroundings must be doing work 17. The temperature of a 21.6 g sample of a metal rises 6.04 C when 60.0 J of energy is applied to it. What is the identity of the metal? a. silver (specific heat = J g -1 C -1 ) b. copper (specific heat = J g -1 C -1 ) c. iron (specific heat = J g -1 C -1 ) d. aluminum (specific heat = J g -1 C -1 ) 18. What is the molar heat capacity of table salt, NaCl (specific heat = 0.88 J g -1 C -1 )? a J mol -1 C -1 b J mol -1 C -1 c. 117 J mol -1 C -1 d. 245 J mol -1 C Determine the quantity of ice required to absorb exactly 50 kj of energy when the ice warms from C to C (specific heat of ice = 2.06 J g -1 C -1, ΔH fus = 333 J/g, ΔH vap = 2260 J/g). a g b. 485 g c. 607 g d g 20. What is the enthalpy change when 22.5 g of CH 4 are burned in excess O 2? Page 4 of 7

5 a kj b kj c kj d kj CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) H = -890 kj 21. The temperature of 3.50 kg of water is raised by 1.17 C when 1.00 g of hydrazine N 2 H 4 is burned in a bomb calorimeter. The calorimeter has a heat capacity of 883 J/ C. How much heat is given off by the sample? The specific heat of water = 4.18 J g -1 C -1. a kj b kj c kj d kj 22. The standard enthalpies of formation for several substances are given below: CO(g) kj/mol CO 2 (g) kj/mol H 2 O(l) kj/mol H 2 O(g) kj/mol H 2 O 2 (l) kj/mol CH 3 OH(g) kj/mol C 2 H 5 OH(l) kj/mol C 2 H 5 OH(g) kj/mol Determine the H for the reaction below. a kj b kj c kj d kj 2CO(g) + 4H 2 (g) C 2 H 5 OH(g) + H 2 O(g) 23. Write the correct Lewis dot structure for CCl 2 O. Which statement correctly describes the structure? a. The structure contains 3 single bonds, 1 double bond, and 2 lone pairs. b. The structure contains 3 single bonds, 1 triple bond, and 8 lone pairs. c. The structure contains 2 single bonds, 1 double bond, and 2 lone pairs. d. The structure contains 2 single bonds, 1 double bond and 8 lone pairs. 24. Which bond is shortest? a. carbon-oxygen double bond Page 5 of 7

6 b. carbon-oxygen single bond c. carbon-nitrogen single bond d. carbon-carbon double bond 25. Which of the following elements is the most electronegative? a. iodine b. nitrogen c. aluminum d. carbon 26. Which statement properly describes the formal charges on the atoms in SO 4 2, where S obeys the octet rule? a. +2 on sulfur, -2 on oxygen b. +2 on sulfur, -1 on oxygen c. +1 on sulfur, -1 on oxygen d. -1 on sulfur, +2 on oxygen 27. Construct correct Lewis dot structures for the three molecules below. Determine which compounds exceed the octet rule. SF 4 PF 3 O 3 I II III a. I b. II c. III d. I, II, and II 28. How many lone pairs of electrons does the Lewis dot structure of H 2 S have around its central atom and what is the molecular geometry of the molecule? a. 0, linear b. 1, triangular planar c. 2, tetrahedral d. 2, bent 29. In VSEPR Theory, under which of the following conditions will the electron-pair geometry always be the same as the molecular geometry? Page 6 of 7

7 a. in molecules with at least one lone pair of electrons on the central atom b. in molecules with no lone pairs of electrons on the terminal atoms c. in molecules with no lone pairs of electrons on the central atom d. in molecules that exceed an octet around the central atom 30. List whether the following molecules are polar or nonpolar. CH 2 Cl 2 SiH 4 SO 2 a. nonpolar, nonpolar, nonpolar b. nonpolar, nonpolar, polar c. polar, nonpolar, polar d. polar, polar, polar 31. Which is the correct listing in order of the strongest type of force that must be overcome to allow each of the processes below? I. the evaporation of propanol (CH 3 CH 2 CH 2 OH) II. the boiling of liquid CH 2 Cl 2 III. the melting of solid Br 2 IV. the boiling of liquid BF 3 a. hydrogen bonding, London (dispersion) forces, dipole-dipole, dipole-dipole b. hydrogen bonding, dipole-dipole, London (dispersion) forces, London (dispersion) forces c. dipole-dipole, dipole-dipole, London (dispersion) forces, London (dispersion) forces d. London (dispersion) forces, covalent bonding, dipole-dipole, dipole-dipole 32. What happens to a helium balloon at a party on a hot day if the balloon was filled on a cold morning? a. The balloon expands because the warmer day temperature causes the helium atoms to be less attracted to each other and allows them to occupy more space inside the balloon. b. The balloon expands because the warmer day temperature speeds up the helium atoms and increases the force and frequency of gas collisions on the inner wall of the balloon. c. The balloon shrinks because the warmer day temperature causes the helium atoms to be more attracted to each other and allows them to occupy less space inside the balloon. d. The balloon keeps the same volume because the amount of gas inside the balloon does not change. 33. Calculate the number of moles of a gas that occupy ml at STP. Page 7 of 7

8 a b. 3.1 c d A sample of chlorine gas (Cl 2 ) occupies 1.65 L at 1.0 atm and 308 K. What pressure (in mm Hg) will the sample exert at 3.00 L and 51 C? a b. 69 c. 297 d What volume (in L) of oxygen at 298K and 1.50 atm is required for the complete combustion of 25.0 g of hexane? a b c d C 6 H O 2 12 CO H 2 O 36. In an equimolar mixture of nitrogen and neon gases at 50 C, a. the partial pressure of neon will be higher than nitrogen because the neon molecules are moving more rapidly. b. the partial pressure of neon will be lower than nitrogen because the neon molecules are moving more slowly. c. both gases exert the same partial pressure. d. the total pressure is independent of the partial pressures of the two gases. 37. A mixture of H 2 (g) and Cl 2 (g) exerts a total pressure of 2.50 atm. If the mole fraction of H 2 is 0.490, what is the partial pressure (in atm) of H 2? a b c d Page 8 of 7

9 38. A 5.00 L flask contains 3.50 g of sulfur trioxide, 2.45 g of carbon monoxide, and 3.99 g of argon all at 35 C. What is the pressure (in atm) in the flask? a b c d Under what conditions do real gases most closely approximate the behavior of ideal gases? a. high pressure and high temperature b. high pressure and low temperature c. standard temperature and pressure d. low pressure and high temperature 40. Which of the following gases is the most significant contributor to the greenhouse effect? a. water vapor b. carbon dioxide c. nitrogen d. ozone Page 9 of 7

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.

7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790. CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,

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