2008_05_30_14_57_33

2008_05_30_14_57_33 - Final FILL IN YOUR STUDENT ID NUMBER...

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Unformatted text preview: Final. FILL IN YOUR STUDENT ID NUMBER. NAME, AND TEST FORM=C 3. 10. ll. 12. 13. N qu/I/lél/ FOR NUMERICAL QUESTIONS CHOOSE THE CLOSEST VALUE (R= 8. 314JIK-mol= 0.08206 L-atmlmol-K) You may not be seated next to a friend. You may not use a graphing calculator. One sheet of notes only. You may not possess or touch a cell phone' In your possession during the test. Consider the following processes. (Treat all gases as ideal.) I. The pressure of one mole of oxygen gas is doubled isothennally. 2 ZNHp 3(a) --> N (g) + 3 H 2(a); / 3. Fixing a deck oTcards' In order to cheat 4. Defrag gmenting a hard drive on a computer ' S. HOHgm(s) --> CH 301-10) — Whicho these processes leads to a decrease in entropy? (a) none; (b) just one; (c) just 2; @ust 3; (e) 4 or more All of the following compounds become lessstable with respect to their elements as the temperature is raised except (a) N009; (b) Csz(g); (C) N2H4(1); \(d) C“0(5); (e) N02(g) At 101°C, the boiling of water is spontaneous. Predict the sign (+,- , or 0) of AG,°, AH,°, and AS,°, respectively at 101°C. @ 0, +; (b) ’I'I'; (C) ‘ ’+’+; (d) 01+ 9+ +. (9)94, ' ' 5C7 ’: H ’ '01 ‘5 Consider the following reaction:: NO (g) -) N(g) + Om Which of the following statements regarding this reaction are true? @31‘ he reaction is spontaneous at high temperatures. (b) The reaction is spontaneous at low temperatures; (c) The reaction is not spontaneous at any temperature. (d) The reaction is spontaneous at all temperatures; (e) need more information to answer this question 4 , y. L. t: ’ ”I ‘1 (a) solid XY has a higher density than liquid XY; lId XY has a lower density than liquid XY; \ (c) solid XY has the same density as liquid XY; freezing XY IS an endothemiic process; t + The phase diagram for compound XY has a [email protected] with a negative slope. Which of the following Is true? (e) XY can never be sublimated. ' 57 For an exothermic reaction, under which conditions hill the enthalpy of reaction be of smaller magnitude than c ange in internal energy (IAH|<|AU|)? (a) When moles 01 product gas are reater than moles of reactant gas; When moles of reactant gas are greater than moles of prodeas; efit constant volume; (d) At high pressure; eAt low pressure; L’ l,\ ’ [\U r 1)" ALF“ A ”- -10AV ’ Which order of enthalpies of vaporization lS wrong? (a) Al > CH30H > CH3CHO; (b) Hg I> CH3CH2OII> Xc; (c) NaCl> CH3CH20H> Xe; (d) CH3CH2NH3 > gCH3CH2F > CH4; l(e))NaC1> CH30CH3 > CHJCHle-lz ; u . Which of the following has the smallest lattice energy? @hlalf; (b) Y203; (c) NaCl; ((1) (NHOZS (e) Na2804 2 - 1 ‘l -\ 4 ‘ Calculate the enthalpy for the decomposition of NO; in kJ/mol ’1 2N02(g) —> 2N0(g) + 02(g) from the standard reaction enthalpies of N0(g) —> 1/2N2(g) + 1/202 AH° = -9o.3 kJ-mol" 2Nz(g) + 4020;) —> 4N02(g) AH° = +1323 krmor‘ a) 114; (b)-247; (c) -114; (d)+294; (e)-247 Use average bond enthalpies to calculate mm,” in kJ/mol for: H2C=Cl-lz(g) + 2N2(g) —>2H2C=N=N(g) The bond enthalpies in kJ/mol arc(C=C) = 620; (N.=_N) = 914; ('N=N) = 418; (C=N) = 615; (C-I-l) = unknown; (C-C) = 348; (N-N) =l63. (a) less than -300; (b) -300 to -100; (c) -100 to +100; ((1) +100 to +300; @more than +300 For the equilibrium Si02(s) + 411F(g)(-> SiF4(g) + 211200;) with AH° = - 148.9 kJ/mol, which of the follouing would cause the equilibrium to shift to the right? (a) Adding more SiOz; (b) increasing the temperature; (c/Adding a cataly;st Gd) Decreasing the pressure by' Increasing the volume; @emoving water (v, The decomposition of phosgene, COC12(g) <===> CO(g) + C|2(g),' Is an endothermic process. How many of the following factors will cause the value of the equilibrium to shift to the left? addingCOClz; adding afitalyst; increasing the temperature; decreasing the total pressure. (a) none; (b) one; o; (d) three; (e) four; The reaction rates of many spontaneous reactions (i. e. K>l and AG°<0) are actually very slow. Which of the following' 15 the best explanation for this observation? (a) AS°<<0; (b) AS°>>0; (c) Q <<K (d) Q >>K; .10116 of the above Which 0.0666M solution will be the most basic? (a) NaCH3COO; @004; (c) Na(CHC12)COO; (d) CO; (e) Na(CHBr2)COO; w a N x, 1 , 15. 16. 17. 18. 19. 23. 24 25 26. Which of the following 1 M solution would be basic (pH>7) HF, NaOH, NaF, NH4CI, K28? @aOH only; (b) all; (e) NaOl-l, NaF, NH4C1, K25 only; (d) NaOH, N114Cl, K28 only; (e) some other com ination . f 1 Which of the following would you ect to be the least soluble in H20 and having a boiling point above 200 °C: (a) I???“ (b) KNO, (c) CaBrz; @gfl; (c) CH3OH , / /’ Calculate the molecular weight in g/mol of a salt X+Y- if a 3.33 g sample dissolved in 666 mL of water has an osmotic pressure of 0.876 atm at 25.0 °C. (R = 0.0821 L-atm/mol—K ). Assume the solution is ideal. (3)0-50 (b)51-100;@01-200; (d)201-300; (e) 30|ormore When a unknown salt is dissolved in water, the solution becomes colder. This information indicates . (a) the entropy of the solution is negative; (b)‘AH of solution is negative' (c) the salt has a small lattice energy (c) the solubilitymvill decrease as the temperature increases; he solubility of will increase as the temperature increases; (e) the salt probably contains a transition etal lnitial pressures of P(NO) = 0.129 atm and P(Br ) = 0.0543 atm were allowed to react at an unknown temperature. At equilibrium, P(total) = 0.145 atm. Calculate t e itt units of atm'l for the reaction ‘ 2N0(g) + Br2(g)<—> 2NOBr(g). (a) 1 x 10‘; (b) 6. ; (c) 34; @40; (e) 51; For PCl3(g) + Clg(g) <--> PCls(g), if the initial concentration of PC15(g) is 6.0 M and the others are zero, at equilibrium the concentration of Clz(g) is 1.60 M. Calculate the value of Kc at this temperature in M". (a)0.6; (b)3.4; @J; (d)0.29; (e) 2.2 Calculate the molar solubility of Ba3(l’0 )2 in a 0.666M Na31’0. solution. (KSp = 1.3 x 10'”). (a) more than 10*; (b) 10“6 to 10'”; 10'9 to 10'”: (d) 10%» 10'”; (1:) less than 10''5 Which of the following will increase the solubility of l’b(CN)2(s) (agtldition of 0.1 M llCN; " (ha/addition of a strong acid; (c) addition of a strong base; (d) addition of Pblz(s); (e) none Calculate the minimum number of moles of Mg(NO3)2 (a strong electrolyte) that must be added to 1L of 0.010 M NaF solution in order to initiate a precipitati of magnesium fluoride. F or high, K,,,“= 6.9 x 109. (a) 10" or more; (b) 10"; (c) 10*; (d) 10"; 510'9 or less What is the molar concentration of free Zn” in a 0.30 M solution of [Zn(C_1:J)4]2'? (K; = 1.0 x 10‘9) ((3’)).1 x 10"; (b) 8.7 x10'5; (c) 2.4 x 10“; (d) 2.4x 10"; (e) 1.2 x 10 A solution is buffered at a pH = 6.66. Estimate the concentrations of Zn2+ in this solution? Zn2+(aq) + 2 HCN(aq) <--> Zn(CN)2(s) + 2 H+(aq). K = 2.0 x 10' ; (a) l M or more; (b) 0.1 M; (c) 0.01 M @7001 M (e) 0.00010r less . 1, In which of the following solution will the acid have the greatest percent ionization? (Kim Jon ll loves this one) (a) 0.1M CHC|2COOH dissolved in 0.1 M HClOi; (b) 0.1M CHZCICOOH dissolved in 0.2 M HC103; /(c)' 0.1M CH3COOH dissolved in 0.1M CH3COONa; (fl) 0.1M CH3COOH dissolved in 0.2 M CH3COONa; (e) 0.1M CH3COOH dissolved in 0.1 M NaClO; Estimate the ratio of [HSOg']/[SO3’2] at equilibrium in a 1.0 M H2803(aq) solution (pKn. = 1.81; pKaz = 6.91). (a) 103 or less; (b) 104; (c) 10’; (d) 10°; @107 or more Estimate the pH at the equivalence point for the titration of 0.333 M HClO4 versus 0.666 M NH}. Kb =1.8 x10". (a)2 to 4; @4 to 6; (c) 6 to 8; (d) 8 to 10; (e) 10 to 12 Calculate the pH after 75 ml. of 0.40 M KOH has been added to 100 mL of 0.20 M HZA (PKal = 3.82 and PKaZ = 6.10). (a) 4 or less; (b) 4 to 5; (c) 5 to 6; (d) 6 to 7; ”(3))7 or more Which of the following mixtures gives a buffer with a pOH greater than 7.0? For CH3COOH, K. =18 x 10‘5 and for NH3, K, = 1.8 x 10” a 6.66 mL of0.l M NH3(aq) + 3.33 ml of0.l M l-lCl(aq); 11556.66 mL of0.1 M CH3COOH + 3.33 ml. of .l M NaOH(aq); (276.66 ml. of 0.1 M CH3COOI-l + 6.66 mL of 0.1 M Na0H(aq); (d) 6.66 mL of 0.1 M NH3(aq) + 3.33 mL of 0.1 M HCl(aq); (e) none of these FILL IN YOUR STUDENT ID NUMBER, NAME, AND TEST FORM=C ...
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