Kinetic Modeling Study of the Industrial Sulfur Recovery Process for Operating Condition Optimization

Table 1

The kinetic parameters for the pyrolysis of H₂S.

Reactions^a	A (cm^3·mol^−1·s^−1)	n	E (cal·mol^−1)
S + H + M = SH + M	0.62 × 10^17	−0.6	0
S + H2 = SH + H	0.14 × 10^15	0.0	19 300
S2 + M = S + S + M	0.48 × 10^14	0.0	77 000
H + S2 + M = HS2 + M	0.40 × 10^14	2.84	1 665
SH + SH = S2 + H2	0.50 × 10^12	0.0	0.0
SH + S= S2 + H	0.30 × 10^14	0.0	0.0
H2S + M = S + H2 + M	0.16 × 10^25	2.613	89 100
H2S + H = SH + H2	0.35 × 10^08	1.94	904
H2S + S = SH + SH	0.83 × 10^14	0.0	7400
HS2 + H = SH + SH	0.97 × 10^08	1.62	−1030
Duplicate	0.11 × 10^14	0.353	210
HS2 + H = S2 + H2	0.12 × 10^09	1.653	−1105
HS2 + H = H2S + S	0.44 × 10^14	0.0	6326
HS2 + S = S2 + SH	0.42 × 10^07	2.2	−600
HS2 + SH = H2S + S2	0.63 × 10^04	3.050	−1105
HS2 + HS2 = H2S2 + S2	0.96 × 10^1	1.0	57030
H2S2 + M = SH + SH + M	0.14 × 10^16	0.0	15 000
H2S2 + H = HS2 + H2	0.50 × 10^08	1.933	−1408
H2S2 + H = H2S + SH	0.20 × 10^15	0.0	0.0
H2S2 + S = HS2 + SH	0.29 × 10^07	2.31	1204
H2S2 + SH = HS2 + H2S	0.64 × 10^04	2.98	−1480

^aDeclared duplicate reaction.