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Unformatted text preview: g = 9 . 81 m/s 2 c = 3 10 8 m/s d water = 1 . 00 g/mL 1 atm = 1.01325 10 5 Pa N A = 6 . 022 10 23 mol 1 k = 1 . 381 10 23 J/K R = 0 . 08206 L atm/mol K R = 8 . 314 J/mol K R = 62 . 36 L torr/mol K 1 L atm = 101.325 J E = h c = / = h p = h mv 1 2 mv 2 = h T max = 1 5 c 2 c 2 = 0 . 0144 K m = R 1 n 2 1 1 n 2 2 R = 3 . 29 10 15 Hz E n = n 2 h 2 8 mL 2 n = 1 , 2 , 3 , P = dhg PV = nRT P total = P A + P B + P C + x A = P A /P total P + a n 2 V 2 ( V nb ) = nRT v rms = 3 RT M 1 / 2 rate of effusion (or speed) r T M U = q + w H = U + PV U = q V = C V T = nC V, m T H = q P = C P T = nC P, m T w = P V w = nRT U = H P V U = H nRT H rxn = H 1 + H 2 + H 3 + ... H rxn = X nB.E. (react) X nB.E. (prod) H rxn = X n H f (prod) X n H f (react) S rxn = X nS (prod) X nS (react) G rxn = X n G f (prod) X n G f (react) H r ( T 2 ) = H r ( T 1 ) + C P T C P = X nC P, m (prod) X nC P, m (react) w = nRT ln V 2 V 1 S = nR ln V 2 V 1 S = C V ln T 2 T 1 S = C P ln T 2 T 1 H vaporization 85 J/mol K d S = d q rev /T S = k ln W G = H TS G = H T S Moore, Lauren Final 1 Due: May 10 2007, 1:00 pm Inst: McCord 2 This printout should have 56 questions. Multiplechoice questions may continue on the next column or page find all choices before answering. The due time is Central time. 001 (part 1 of 1) 10 points How many sigma and pi bonds are in the molecule CH 2 CCH 2 ? 1. 4 sigma and 2 pi 2. 6 sigma and 2 pi correct 3. 2 sigma and 2 pi 4. 6 sigma and 0 pi 5. 8 sigma and 0 pi Explanation: 002 (part 1 of 1) 10 points What volume of hydrogen at STP would be required to produce 1.000 mole of HCl? H 2 (g) + Cl 2 (g) 2HCl(g) 1. 6.6 L 2. 22.4 L 3. 5.3 L 4. 11.2 L correct 5. 44.8 L Explanation: At STP, 1 mole of an ideal gas has a volume of 22.4 L; i.e. , 22 . 4 L mol . V H 2 = 1 mol HCl 1 mol H 2 2 mol HCl 22 . 4 L H 2 mol H 2 = 11 . 2 L 003 (part 1 of 1) 10 points Which is the weakest type of attractive force between particles? 1. hydrogen bond 2. dispersion forces correct 3. ionic bond 4. covalent bond Explanation: London forces, dispersion forces, or induced dipoles all describe the same intermolecular force. London forces are induced, shortlived, and very weak. Molecules and atoms can experience London forces because they have electron clouds. London forces result from the distortion of the electron cloud of an atom or molecule by the presence of nearby atoms or molecules. Permanent dipoledipole interactions are stronger than London forces and occur be tween polar covalent molecules due to charge separation....
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This note was uploaded on 02/25/2010 for the course CH 54363 taught by Professor Mccord during the Spring '08 term at University of Texas at Austin.
 Spring '08
 McCord
 Chemistry

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