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Unformatted text preview: , of Cl 2(g) given the following: 2 K (s) + Cl 2(g) 2 KCl (s) ∆S 0 =  187.22 J K1 mol1 S (K (s) ) = 64.63 J K1 mol1 S (KCl (s) ) = 82.56 J K1 mol1 ∆S rxn = 2x S (KCl (s) ) – { 2x S (K (s) ) + S (Cl 2(g) )} Solving: S (Cl 2(g) ) = 223.08 J K1 mol1 5. (10 points) Consider the following reaction N 2 (g) + O 2 (g) 2NO (g) . a) If ∆H 0 = 180.58 kJ and ∆S = 24.8 J K1 , calculate ∆G at 200 K. ∆G 0 = ∆H T∆S = 180.58 kJ – (200 K) x (24.8x103 kJ K1 ) = 175.62 kJ b) This reaction switches from being spontaneous to being non spontaneous at a particular temperature called the crossover temperature. Complete the following statement by circling the correct choices: The reaction is spontaneous at low / high temperatures, and non spontaneous at low / high temperatures. c) Calculate the crossover temperature Set ∆ G 0 = 0 T= ∆H / ∆S = 180.58 x 10 3 J / 24.8 J K1 = 7281 K...
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 Spring '07
 veige/martin
 Thermodynamics, Reaction, Entropy, thermodynamics states, K1 mol1, Vs Vs Vs

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