Chemical reactions are build upon educts, a reaction arrow and
products. Each reaction is closed by a semicolon. Educts, or
products, respectively, constitute a sum of reaction partners.
A reaction partner is described by a leading coefficient ('1' can
be omitted) and the species name. Note that a blank between coefficient and name
is necessary. Otherwise the compiler would confuse
the coefficient with a part of the species name.
2 A | <=> | S + 5 D; |
1^(1+) | --> | 1^(2+) + 1; |
The kinetics of a reaction is per default determined by its reaction arrow. The arrow '<=>' describes a reaction with a reversible power rate law (see below). The arrow '-->' describes an irreversible power rate law.
In general, all heterogeneous reaction steps as well as surface reactions occur locally on specific boundary faces, e.g. on an electrode surface. Depending on the geometric model, various boundaries are involved which can be supplied with so called boundary indices, e.g. a boundary with index 1 is described by the boundary operator
Within the input language, adsorptions and surface reactions as well as heterogeneous
electron transfers need to be linked with the corresponding boundary face.
Boundary operators are specified behind the according reaction in the so called option
section which is again closed by a semicolon.
Thus, an adsorption process can be formulated as:
A{ads} + B{ads} | --> | C{ads}; | b<1>; |
For homogeneous and surface reactions, Ecco assumes per default that the reaction kinetics follow
a power rate law (r = kf * prodi(cipi) - kb * prodj(cjqj) ) in which the reaction order of a species (p or q)
equals its stoichiometric coefficient.
For irreversible reactions, it is kb = 0.
Optionally, each reaction order can be changed to any real number (as long as equilibrium
conditions are fullfilled) through so called power operators, p<>, e.g.
A{ads} | <=> | B{ads}; | b<1>, p< A{ads} > = 2, p< B{ads} > = 2; |
2 CO + 3 H2 | <=> | CH3OH + CO + H2; | p<CO> = (-0.3,-1.3), p<H2> = (1.3,-0.7); |
This will change the reaction orders of A{ads} and B{ads} to 2. The orders of CO and H2 are set to -0.3 and 1.3 for the forward reaction (=>) and -1.3 and -0.7 in the backward reaction (<=).
The most general concept supported is that of generic rate laws. These reaction rates can be specified for homogeneous and surface reactions as arbitrary algebraic expressions, composed of species concentrations, kinetic and equilibrium constants, as well as user defined constants. Species concentrations are described by concentration operators, c<>, forward and backward rate constants by 'kfj ' and 'kbj ', respectively. Equilibrium constants are denoted as 'Kj ' (j is the number, counted from zero, of the corresponding reaction). The mechanism
E + S | <=> | ES; | |
ES | <=> | P + E; | r = kf1*E0*c<S>/(K0 + c<S>); |