CHEM1310_MidtermW10_PartA_wAnswers

CHEM1310_MidtermW10_PartA_wAnswers -...

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THE UNIVERSITY OF MANITOBA March 4 2010 MIDTERM EXAMINATION PAPER NO XXX PAGE NO: 1 of 2 Data Pages DEPARTMENT & COURSE NO: CHEM 1310 TIME: 2 HOURS EXAMINATION: University I Chemistry: Intro. to Phys. Chem. EXAMINER: CHEM 1310 Committee I A V I I I A 1 H 1.008 IIA atomic number Symbol atomic mass IIIA IVA VA VIA VIIA 2 He 4.003 3 Li 6.941 4 Be 9.0122 5 B 10.81 6 C 12.011 7 N 14.007 8 O 15.999 9 F 18.998 10 Ne 20.179 11 Na 22.990 12 Mg 24.305 IIIB IVB VB VIB VIIB VIIIB IB IIB 13 Al 26.982 14 Si 28.086 15 P 30.974 16 S 32.06 17 Cl 35.453 18 Ar 39.948 19 K 39.098 20 Ca 40.08 21 Sc 44.956 22 Ti 47.88 23 V 50.942 24 Cr 51.996 25 Mn 54.938 26 Fe 55.847 27 Co 58.933 28 Ni 58.69 29 Cu 63.546 30 Zn 65.38 31 Ga 69.72 32 Ge 72.59 33 As 74.922 34 Se 78.96 35 Br 79.904 36 Kr 83.80 37 Rb 85.468 38 Sr 87.62 39 Y 88.906 40 Zr 91.22 41 Nb 92.906 42 Mo 95.94 43 Tc (98) 44 Ru 101.07 45 Rh 102.91 46 Pd 106.42 47 Ag 107.87 48 Cd 112.41 49 In 114.82 50 Sn 118.69 51 Sb 121.75 52 Te 127.60 53 I 126.90 54 Xe 131.29 55 Cs 132.91 56 Ba 137.33 57 La 138.91 72 Hf 178.49 73 Ta 180.95 74 W 183.85 75 Re 186.21 76 Os 190.2 77 Ir 192.22 78 Pt 195.08 79 Au 196.97 80 Hg 200.59 81 Tl 204.38 82 Pb 207.2 83 Bi 208.98 84 Po (209) 85 At (210) 86 Rn (222) 87 Fr (223) 88 Ra 226.03 89 Ac 227.03 58 Ce 140.12 59 Pr 140.91 60 Nd 144.24 61 Pm (145) 62 Sm 150.36 63 Eu 151.96 64 Gd 157.25 65 Tb 158.93 66 Dy 162.50 67 Ho 164.93 68 Er 167.26 69 Tm 168.93 70 Yb 173.04 71 Lu 174.97 90 Th 232.04 91 Pa 231.04 92 U 238.03 93 Np 237.05 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260) PHYSICAL CONSTANTS CONVERSION FACTORS Avogadro’s number N = 6.022 × 10 23 mol –1 101.3 kPa = 1.00 atm Charge on proton e = 1.602 × 10 –19 C 1.00 atm = 760 torr or 760 mmHg Gas constant R = 0.0821 L atm K –1 mol –1 ln(x) = 2.303 log(x) R = 8.314 J K –1 mol –1 1 V = 1 J C –1 Planck’s constant h = 6.626 × 10 –34 J s 1 kPa L = 1 J Speed of light c = 2.998 × 10 8 m s –1 1 J = 1 kg m 2 s –2 Mass of electron m e = 9.11 × 10 –28 g 1 cal = 4.184 J Mass of proton m p = 1.673 × 10 –24 g 1 L = 1000 cm 3 Mass of neutron m n = 1.675 × 10 –24 g 1 bar = 100.0 kPa 0.00 ºC = 273.15 K OTHER USEFUL DATA: Density of water = 1.00 g cm -3 , K w (25 ºC) = 1.0 x 10 -14 , Specific heat of water = 4.184 J K –1 g –1 Δ H fusion of water = 6.01 kJ/mol Δ H vap of water = 40.7 kJ/mol You may tear off this page. Please note there are useful equations given on the back of this page For rough work use the two blank pages found at the back of Part A of the exam.
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Paper: 576 CHEM 1310 University I Chemistry: Intro. to Phys. Chem. Page: 2 of 2 Data Pages kt R R t + = 0 ] [ 1 ] [ 1 SOME USEFUL EQUATIONS a ac b a b x are solutions c bx ax For 2 4 2 0 2 2 ± = = + + P V = n R T P X V = n X RT Δ E = q + w Δ G = Δ H T Δ S Δ G o = – R T ln( K o ) Δ G = Δ G o + RT ln( Q ) Δ S = q rev T q = C s m Δ T w = – P ext Δ V H = E + P V At constant pressure, Δ E = Δ H + w K p = K c ( RT ) Δ n gas ln( K 2 ) = ln( K 1 )– Δ H R 1 T 2 1 T 1 ln P 2 P 1 = Δ H vap R 1 T 2 1 T 1 Integrated zero order rate law: [R] t = [R] o kt zero order half-life: [ ] k R t 2 0 2 / 1 = Integrated first order rate law: [] kt R R t = 0 ln first order half-life: k t 2 ln 2 / 1 = Integrated 2nd order rate law: second order half-life: 0 2 / 1 1 R k t = k = A e –Ea/ RT ln k 2 k 1 = –Ea R 1 T 2 1 T 1 ln( k ) = ln( A) E a RT Beer's law: Absorbance = ε ·b·c pH = –log[H 3 O + ] pOH = –log[OH - ] K w = K a K b pK w = pH + pOH Henderson-Hasselbalch equation: pH = p K a + log [conjugate base] [acid]
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THE UNIVERSITY OF MANITOBA March 4 20 10 MIDTERM EXAMINATION
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This note was uploaded on 12/19/2011 for the course AP CHEM 1300 taught by Professor James during the Fall '11 term at Manitoba.

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CHEM1310_MidtermW10_PartA_wAnswers -...

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