Industrial catalysts

The first time a catalyst was used in the industry was in 1746 by J. Hughes in the manufacture of lead chamber sulfuric acid. Since then catalysts have been in use in a large portion of the chemical industry. In the start only pure components were used as catalysts, but after the year 1900 multicomponent catalysts were studied and are now commonly used in the industry.CO + H2O ⇌ H2 + CO2    (1)Kp=(pH2 x pCO2) / (pCO x pH2O)    (2)Kp=e((4577.8K/T-4.22))    (3)CO + (O) → CO2 + (*)    (4)H2O + (*) → H2 + (O)    (5)H2O → OH(ads) + H(ads)    (6)CO(ads) + OH(ads) → COOH (ads)    (7)COOH(ads) → CO2 + H(ads)    (8)2H(ads) → H2    (9)CO + (species derived from H2O) → Intermediate → CO2    (10)CO + OH → H + CO2    (11)H2O → O (surface)    (12)O (surface) + CO → CO2    (13)C + H2O → CO +H2    (14)CH4 + H2O → CO +3H2    (15)CO + 2H2 → CH3OH (l)    (16)CO2 + 3H2 → CH3OH (l) + H2O (l)    (17)CO2 → CO2*    (18)H2 → 2H*    (19)CO2* + H* → HCOO*    (20)HCOO* + 3H* → CH3OH + O*    (21)CO+ O* → CO2    (22)H2 + O* → H2O    (23)CH3OH(l) + H2O(l) → CO2 + 3H2            ΔH = +131 KJ/mol    (24)CH3OH + H2O → CO2 + 3H2    (25)CH3OH → CO + 2H2    (26)CO+ H2O → CO2 + H2    (27)2CH3OH → CH3OCHO + 2H2    (28)CH3OCHO + H2O → HCOOH + CH3OH    (29)HCOOC → CO2+H2    (30)CH3OH(l) → CO + 2H2            ΔH = +128 KJ/mol    (31)CH3OH(l) + ​1⁄2 O2 → CO2 + 2H2            ΔH = −155 KJ/mol    (32) ( s + p ) CH 3 OH ( l ) + s H 2 O ( l ) + 1 2 p O 2 ⟶   ( s + p ) CO 2 + ( 3 s + 2 p ) H 2 {displaystyle (s+p){ce {CH3OH(l)}}+s{ce {H2O(l)}}+{ce {1/2{mathit {p}}O2->}} (s+p){ce {CO2}}+(3s+2p){ce {H2}}}     (33)N2+ 3H2 ⇌ 2NH3    (34) The first time a catalyst was used in the industry was in 1746 by J. Hughes in the manufacture of lead chamber sulfuric acid. Since then catalysts have been in use in a large portion of the chemical industry. In the start only pure components were used as catalysts, but after the year 1900 multicomponent catalysts were studied and are now commonly used in the industry.