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Thermodynamics filled in class notes_Part_120

Thermodynamics filled in class notes_Part_120 - 247 7.1...

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7.1. ISOTHERMAL, ISOCHORIC KINETICS 247 O 2 O 10 Minus 11 10 Minus 9 10 Minus 7 10 Minus 5 0.001 t LParen1 s RParen1 0.00100 0.00050 0.00030 0.00150 0.00070 LBracket1 O RBracket1 , LBracket1 O2 RBracket1LParen1 mole Slash1 cc RParen1 Figure 7.6: Plot of ρ O ( t ) and ρ O 2 ( t ) for oxygen dissociation with reversible reaction. Thus, by Eq. (7.121), we have Δ G o 13 = 2( 7 . 53908 × 10 12 ) ( 1 . 34628 × 10 13 ) = 1 . 61536 × 10 12 erg mole . (7.133) Thus, by Eq. (7.120) we get for our system K c, 13 = 1 . 01326 × 10 6 dyne cm 2 ( 8 . 31441 × 10 7 erg mole K ) (5000 K ) × exp parenleftBigg parenleftBigg 1 . 61536 × 10 12 erg mole ( 8 . 31441 × 10 7 erg mole K ) (5000 K ) parenrightBiggparenrightBigg , (7.134) = 1 . 187 × 10 4 mole cm 3 . (7.135) Substitution of all numerical parameters into Eq. (7.126) and expansion yields the fol- lowing d ρ O dt = 3899 . 47 (2 . 23342 × 10 10 ) ρ 2 O (7 . 3003 × 10 12 ) ρ 3 O = f ( ρ O ) , ρ O (0) = 0 . 001 . (7.136) A plot of the time-dependent behavior of ρ O and ρ O 2 from solution of Eq. (7.136) is given in Figure 7.6. The behavior is similar to the predictions given by the pair of irreversible reactions in Fig. 7.1. Here direct calculation of the equilibrium from time integration reveals

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Thermodynamics filled in class notes_Part_120 - 247 7.1...

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