1B-quiz-2-S09-key336

1B-quiz-2-S09-key336 - Name: 2 Quiz 2 Chem 1B, Spring 09...

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Unformatted text preview: Name: 2 Quiz 2 Chem 1B, Spring 09 Fossum Kp = KC(RT)A“ R = 0.08206 L-atm/K-moi lug: R= 8.314 J/m010K k1 R T1 T2 Always show your work and reasoning, include units, and check significant figures. ma 2. (3 points) Draw a sketch of the Boltzmann distribution (a graph of the number of molecules vs. kinetic energy) for a high temperature sample and a low temperature sample. Explain clearly how this applies to reaction rates. m M 0L0 CULQ S (fluff CC +va P , mac-f— MVC E Eq C)£LV\ . _ lg . ‘ ‘ 0m H: an increase, T“! a 5mg. pram”: 5 01f ‘ beetles has W W “ 3P6 Qt 50 “Kn W‘“ be. asifir ad" [At T n: j [)LWLVWCMK’W is raid/{tag #2) W fiach of Mair-atlas have Elna/6L" "fa dad. r. KG = 6.8 x106 at 25°C F01” the reaction: NO (g) + 1/2 02 (g) N02 (g) a. (1 point) Write the Kc expression for this reaction. ~ : (No; KC CM 03 CO 211/2 b. (1 point) When this reaction reaches equilibrium at 25°C, is the equilibrium mixture composed of mostly products or mostly reactants? Explain how you can tell. MO is wig. Marsh: pmaiuc‘is M‘equflaiow‘uw c. (2 points) Calculate the value of Kc for the following reaction at 25°C. 2 N02(g) 2 N0(g) + 02(g) Kc = ? ‘ . gm wrfia mum. WWW 52‘ T2) gm" M W K, m dud Square. rt. K O >z - 54.52le04“ d. (2 points) Calculate the value of Kp for the following reaction at 25°C. 2 N02 0;) 2 N0<g> + 02 (g) Kp = 7 K? : KC C QT Avx Awaas : (3-2 \4“. 2 (21T103x10"“)<(0.0m\(2ag3> x10” :9 ‘— —> ‘— —> W [l— 3. 4+2 a. (4 points) Given the following proposed mechanism, determine the rate law. Remember that intermediates can’t be in the overall rate law. Show your work/reasoning. 1. 12 S 21 (fast, equilibrium) 2. I+I+ H2 —> 2H1 (slow) _ 2' Wafl trait am}: 0‘? slow stcf ~= lat—C] [HQ bust I is aux inwwiate. “Mtg/make Subsbiww, {w step !, I’d/it emwa Few“ "kllc/lZFd : $4 [:11 15:21 ’li-t await 3 4&2 Q&\ H23 “L: 80 b. (1 point) State the molecularity of each step in the above mechanism. s46?! — minnoquin €46? 2‘ " WWQa/«iflf (6 points) The rate constant of a reaction is 8.85 ><10'5 M'lsec'1 at 23°C. If the activation energy of this reaction is 46.3 kJ/mol, calculate the value of the rate constant at 44°C. 1&2 —— a t 7.. -%(~+:~%D lnlz. 8 .88 x (O'SM‘B'ZF‘ $3.3M KIM-K ( 0.0033534 e" ~0w3i'§% K") AA = Aft/5cm TM! _...-.................-_..__.._ (0. ooo2§390~t L") J?» : Limosg L"; (0'53 _ — . ‘l - 3.431% A h. 30 “of «w- \ -‘fl = (ms Mo'sw‘gec'X'éflwc): 3 Md“ Mam-i 17: iii {1. : e. Jlflz ...
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This note was uploaded on 09/04/2011 for the course CHEM 1B taught by Professor Fossum during the Spring '10 term at Laney College.

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1B-quiz-2-S09-key336 - Name: 2 Quiz 2 Chem 1B, Spring 09...

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