Bibliography of Papers: 1913–1958 by L. Ƶechmeister (auth.)

By L. Ƶechmeister (auth.)

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101) 4 η + ζ + (Cp,A /Cv,x − 1) λ/Cp,x 3 − (∂ρ/∂x)p,T + kT (∂ρ/∂T )x,p (∂A/∂x)p,T Cp,x 2 D (∂p/∂ρ)x,T ρ0 (∂A/∂x)p,T . 102) September 11, 2009 10:7 42 World Scientific Book - 9in x 6in General-nn Chemistry versus Physics: Chemical Reactions near Critical Points One can readily use the hydrodynamic equation including the chemical term (L0 = 0) and perform the analogous calculations, but this procedure leads to very cumbersome expressions. Therefore, we consider the influence of a chemical reaction for the simplified case of a non-compressible liquid (div (v) = 0), neglecting fluctuations of pressure (p = 0) [60].

In the general case, such a calculation involves a very cumbersome analysis. To avoid this, we consider some special cases. When one neglects the thermal variables, viscous, diffusive and chemical modes appear in Eq. 84), × 1+ L = L20 + × ∂A ∂ξ 2 4 3η 2 p,S 4 3η + ζ 2 2 +ζ ∂ρ ∂A L1 /ρ0 Dk 2 + L0 (∂A/∂ξ)ρ,S ρ0 (∂ξ/∂ρ)A,S k + 4ρ0 L1 (∂A/∂ρ)ξ,S + ρ20 ξ,S ∂ξ ∂ρ A,S ∂ρ ∂p . 114) ξ,S Note that the diffusive mode appears in Eq. 114) because of the additional phenomenological visco-reactive coefficient L1 introduced in Eqs.

5) where kf and kb are the microscopically determined rate coefficients for the forward and backward reactions, and Ci are the concentrations (fugacities) of the i-th species in an ideal (nonideal) solution. 6) one can rewrite Eq. 7) where A is the affinity of reaction. 2Cl, the rate r is defined as r = For chlorine dissociation, Cl2 2 , and, using µi = µ0i +RT ln Ci , and kf /kb = exp ν i µ0i /RT , kf CCl2 −kb CCl September 11, 2009 10:7 20 World Scientific Book - 9in x 6in General-nn Chemistry versus Physics: Chemical Reactions near Critical Points one gets r = kf CCl2 1 − exp − A RT .

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