Exam F - Summer 2005

Exam F - Summer 2005 - Chemistry 12 Name Exam IV Form A...

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Unformatted text preview: Chemistry 12 Name _______________________ Exam IV Form A Section _______________________ August, 10 2005 Student No._______________________ IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover = test form A; yellow cover = test form B). Use a #2 pencil. There are 27 questions on this exam. Check that you have done all of the problems and filled in the first 27 bubbles on the scantron. Your score will be reported in percents (max 100%). Exam policy • • • • Calculators with text-programmable memory are not allowed. Relevant data and formulas, including the periodic table, are attached at the end of this exam. Your grade will be based only on what is on the scantron form. The answer key will be posted on the web after the exam (under "News"). Hints • • • As you read the question, underline or circle key words to highlight them for yourself. Avoid errors from "mis-reading" the question. Pay attention to units and magnitudes (decimal places) of numbers obtained from calculations. There is no penalty for guessing. Chemistry 12 Exam 4 Basic Skills 1.) Which one of the following is the ground state electron configuration of Zn? a) b) [Ar] 4s1 3d10 c) [Ar] 4s2 3d10 d) [Ar] 3s2 3d10 e) 2.) [Kr] 4s2 3d10 [Kr] 3s2 3d10 What is the balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed? a) 2Na+(aq) + CO32–(aq) → Na2CO3(aq) b) 2Na+(aq) + 2Cl–(aq) → 2 NaCl(aq) c) Na+(aq) + Cl–(aq) → NaCl(aq) d) Ca2+(aq) + CO32–(aq) → CaCO3(s) e) Na2CO3(aq) + CaCl2(aq) → 2NaCl(aq)+ CaCO3(s) 3.) Which one of the follow has 54 electrons? i 137 56 ii 128 52 iii 132 54 a) iii only d) i and ii e) Xe 2+ ii only c) Te 2− i only b) 4.) Ba +2 ii and iii A stock solution is prepared by adding 27.00 mL of 2.19 M MgCl2 to enough water to make 122.00 mL. What is the Cl− concentration of 40.00 mL of the stock solution? a) b) c) d) e) 0.0388 M 0.485 M 0.969 M 1.48 M 2.96 M 5.) How many valence electrons are there in ClO4−? a) b) 30 c) 29 d) 28 e) 6.) 32 25 An ionic compound has the formula MPO4. What is the identity of M? a) b) Mg c) H d) Al e) 7.) Na Ca What are the spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia? a) H+ and NH3 b) H+, Cl–, NH3, and NH4+ c) Cl– and NH4+ d) H+, Cl–, and NH4+ e) Cl– only 8.) Put these atoms in order of increasing size (radius). Ba O a) O < F < S < Mg < Ba b) F < S < O < Mg < Ba c) F < O < S < Ba < Mg d) O < F < S < Ba < Mg e) F < O < S < Mg < Ba End of Basic Skills F S Mg 9.) The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) is 54.0 at 427 °C. What is the value of Keq at 427 °C for the equilibrium below? HI (g) ½H2(g) + ½I2 (g) a) 27 b) 7.35 c) 0.136 d) 2.92 x 103 e) 3.43 x 10–4 10.) A 3.82 g sample of magnesium nitride is reacted with 7.73 g of water and 3.60 g of MgO is recovered. Mg3N2 + 3H2O → 2NH3 + 3MgO What is the percent yield of the reaction? a) 94.5% b) 78.8% c) 46.6% d) 49.4% e) 99.9% 11.) Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: PCl3(g) + Cl2(g) PCl5(g) An equilibrium mixture at 450 K contains PPCl3 = 0.202 atm PCl2 = 0.256 atm PPCl5 = 3.45 atm What is the value of Kp at this temperature? a) 66.7 b) 1.50 x 10–2 c) 1.78 x 10–1 d) 2.99 e) 7.54 12.) A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution? a) 0.183M b) 8.57M c) 3.50M d) 0.0500M e) 0.117M 13.) When the following equation is balanced, the coefficient of H3PO4 is ____________. H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l) a) 1 b) 2 c) 3 d) 4 e) 0 14.) In which species does sulfur have the highest oxidation number? a) S8 (elemental form) b) H2S c) SO2 d) H2SO3 e) K2SO4 15.) At 400 K, the equilibrium constant for the reaction below is Kp = 7.0. Br2(g) + Cl2(g) 2 BrCl (g) A closed vessel at 400 K is initially charged with 1.00 atm of Br2(g), 1.00 atm of Cl2(g), and 2.00 atm of BrCl(g). Which one of the statements below is true? a) The equilibrium partial pressures of Br2(g), Cl2(g), and BrCl(g) will be the same as the initial values. b) The equilibrium partial pressure of Br2(g) will be greater than 1.00 atm. c) At equilibrium, the total pressure in the vessel will be less than the initial total pressure. d) The equilibrium partial pressure of BrCl(g) will be greater than 2.00 atm. e) The reaction will go to completion (i.e., all of the reactants will be used up) since initially there are equal amounts of Br2(g) and Cl2(g). 16.) Write the balanced equation for the reaction that occurs when methanol, CH3OH(l), is burned in air. What is the coefficient of oxygen in the balanced equation? a) 1 b) 2 c) 3 d) 4 e) 5/2 17.) The value of ΔH° for the reaction below is +128.1 kJ: CH3OH(l) → CO(g) + 2H2(g) How many kJ of heat are consumed when 15.5 g of CH3OH (l) decomposes as shown in the equation? a) 0.48 kJ b) 62.0 kJ c) 1.3 x 102 kJ d) 32 kJ e) 8.3 kJ 18.) What volume (mL) of 7.48 x 10–2M perchloric acid (HClO4) can be neutralized with 115 mL of 0.244 M sodium hydroxide? a) 125 mL b) 8.60 mL c) 188 mL d) 750 mL e) 375 mL 19.) For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product? a) N2(g) + 3H2(g) → 2NH3(g) b) (1/2)N2(g) + O2(g) → NO2(g) c) 6C(s) + 6H(g) → C6H6(l) d) PH3(g) + 4HBr(g) → PH4Br(l) e) 6C(s) + 11H2O(g) → C6H22O11 (s) 20.) Which of the following is an oxidation-reduction reaction? a) Cu(s) + 2AgNO3(aq) → 2Ag(s) + Cu(NO3)2(aq) b) HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) c) AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq) d) Ba(C2H3O2)2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaC2H3O2(aq) e) H2CO3(aq) + Ca(NO3)2(aq) → 2HNO3(aq) + CaCO3(s) 21.) Given the data in the table below, what is ΔH°rxn for the reaction: C2H5OH(l) + O2(g) → CH3CO2H(l) + H2O(l) ΔHf° (kJ/mol) Substance C2H4(g) 52.3 C2H5OH(l) –277.7 CH3CO2H(l) –484.5 H2O(l) –285.8 a) –79.0 kJ b) –1048.0 kJ c) –476.4 kJ d) –492.6 kJ e) There is insufficient information to answer this question. 22.) Given the following bond enthalpies, estimate ΔH° for the complete combustion of one mole of (CH3CH3) in oxygen. C⎯O C⎯C C⎯H a) b) c) d) e) 23.) 336 kJ/mol 356 kJ/mol 416 kJ/mol O⎯H O2 C=O 467 kJ/mol 498 kJ/mol 803 kJ/mol –1419 kJ/mol –648 kJ/mol +648 kJ/mol –2838 kJ/mol None of these are correct to within 1% of the answer. Consider the following reaction at equilibrium: 2NH3 (g) N2 (g) + 3H2 (g) Which one of the following changes will cause an increase in the moles of H2 in the reaction container? a) The removal of some NH3 from the reaction vessel (V and T constant) b) A decrease in the total pressure by changing the volume (T constant) c) Addition of some N2 to the reaction vessel (V and T constant) d) A decrease in the total volume of the reaction vessel (T constant) e) An increase in total pressure by addition of helium gas (V and T constant) Proceed to next page 24.) Given the following reactions: H2O (l) → H2O (g) ΔH = 44.01 kJ 2H2 (g) + O2 (g) → 2H2O (g) ΔH = –483.64 kJ what is the enthalpy for the decomposition (shown below) of liquid water into gaseous hydrogen and oxygen? 2H2O (l) → 2H2 (g) + O2 (g) a) –395.62 kJ b) –527.65 kJ c) 439.63 kJ d) 571.66 kJ e) 527.65 kJ 25.) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O(g) If 34.0 g of ammonia is consumed, how many moles of oxygen will be consumed? a) 2.0 moles b) 4.0 moles c) 7.0 moles d) 14 moles e) 3.5 moles 26.) What is the expression for Kp for the reaction below? 4CuO(s) + CH4(g) a) PCH4 2 PCO2 PH 2 b) [Cu]P P [CuO ] P CO2(g) + 4Cu(s) + 2H2O(g) CO2 4 2 H 2O CH 4 c) PCO2 PH 2O PCH 4 P P d) CO2 H 2O PCuO e) 2 2 PCH 4 2 PH 2O PCO2 Proceed to last page 27.) 27.0 g of Al are mixed with 32.0 g of O2. Assuming the reaction goes to completion, how many moles of Al2O3 will form? a) 0.500 moles b) 0.667 moles c) 1.0 mole d) 2.00 moles e) 1.5 moles Form A 1. C 2. D 3. D 4. C 5. A 6. D 7. E 8. E 9. C 10. B 11. A 12. E 13. A 14. E 15. D 16. C 17. B 18. E 19. B 20. A 21. D 22. A, D=1/2 23. B 24. D 25. E 26. C 27. A ...
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This note was uploaded on 05/24/2009 for the course CHEM 110 taught by Professor Hofmann,brucerob during the Fall '08 term at Penn State.

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