Note for any pressure other than 100 bar k k x r g o

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Note: For any pressure other than 1.00 bar, K K X r G o : 3 ln (8.31 10 / )(298 )ln(0.326) 2.78 / 2.8 / o r G RT K x kJ mol K K kJ mol kJ mol     E6.9a 1 ln o G RT K   3 1 33 / 3.10 (8.31 10 / )(1280 ) 1 0.045 o kJ mol G RT x kJ mol K K K e e e H o = +224 kJ/mol , K 1 = 0.045 at T 1 = 1280 K , K 2 = 1.00 at T 2 = ?? 2 1 2 1 1 1 ln / o H K K R T T   2 1 2 1 1 1 ln / o R K K T T H 3 4 1 2 1 1 8.31 10 / ln 1/ 0.045 6.662 10 1280 224 / x kJ mol K x K T K kJ mol 2 4 1 1 1501 1500 6.662 10 T K K x K
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E6.17a Reaction: (1/2) N 2 (g) + (3/2) H 2 (g) NH 3 (g) G o = f G o = -16.5 kJ/mol T = 25 o C = 298 K , p N2 = 3.0 bar , p H2 = 1.0 bar , p NH3 = 4.0 bar 3 2 2 1/2 3/2 3 1/2 3/2 ln (4.0) 16.5 / (8.31 10 / )(298 )ln (3.0) (1.0) 16.5 / 2.07 / 14.4 / NH o N H p G G RT p p kJ mol x kJ mol K K kJ mol kJ mol kJ mol         E6.23a Reduction Potentials are taken from Resource Section Table 6.2 (pg. 929) (a) Sn(s) + Sn 4+ (aq) 2 Sn 2+ (aq) Reduction: Sn 4+ (aq) + 2 e - Sn 2+ (aq) E o Red (Sn 4+ ) = +0.15 v Oxidation: Sn(s) Sn 2+ (aq) + 2 e - E o Oxid (Sn) = -E o Red (Sn 2+ ) = +0.14 V E o Cell = +0.15 V + 0.14 V = +0.29 V ln ln o o Cell Cell RT nF E K K E nF RT (2)(96,500) ln ( 0.29) 22.60 (8.31)(298) K   22.60 9 6.5 10 K e x (b) Sn(s) + 2 AgCl(s) Sn 2+ (aq) + 2 Cl - (aq) + 2 Ag(s) Reduction: 2 AgCl(s) + 2 e - 2 Ag(s) + 2 Cl - (aq) E o Red (Sn 4+ ) = +0.22 v Oxidation: Sn(s) Sn 2+ (aq) + 2 e - E o Oxid (Sn) = -E o Red (Sn 2+ ) = +0.14 V E o Cell = +0.22 V + 0.14 V = +0.36 V ln ln o o Cell Cell RT nF E K K E nF RT (2)(96,500) ln ( 0.36) 28.06 (8.31)(298) K   28.06 12 1.5 10 K e x
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Supplementary Homework S6.1 = 0.30 A(g) B(g) + 3 C(g) n o (1- ) n o 3n o n tot = n o (1- ) + n o + 3n o = n o (1+3 ) (1 ) 1 0.30 2.0 0.737 (1 3 ) 1 3(0.30) o A A o n p X p p bar bar n 0.30 2.0 0.316 (1 3 ) 1 3(0.30) o B B o n p X p p bar bar n 3 3(0.30) 2.0 0.947 (1 3 ) 1 3(0.30) o C C o n p X p p bar bar n 3 3 (0.316)(0.947) 0.364 0.36 0.737 B C A p p K p
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