Open AccessThe reduction of metallic oxides with hydrogen at high pressures
Publication year - 1916
Publication title -
proceedings of the royal society of london. series a, containing papers of a mathematical and physical character
Language(s) - English
Resource type - Journals
eISSN - 2053-9150
pISSN - 0950-1207
DOI - 10.1098/rspa.1916.0013
Subject(s) - hydrogen , endothermic process , chemistry , thermodynamics , oxide , metal , inorganic chemistry , organic chemistry , physics , adsorption
The equilibrium relation in the reaction between a metallic oxide and hydrogen is determined at any given temperature by the concentration of the hydrogen and that of the water vapour produced by the reduction. Thus, if in the equation MeO + H2 ⇌ Me+H2 O, C denotes the concentration of the hydrogen and C' that of the water vapour, we have the relation:— C/C' = K, where K is a constant at any given temperature. If C/C' can be arranged to be greater than K, the reaction expressed in the above equation proceeds from left to right. This state of affairs may be realised:— (a ) By increasing the pressure of the hydrogen present. (b ) By diminishing the pressure of the water vapour formed during the reaction. (c ) If the reaction is endothermic, by raising the temperature, when the value of K is diminished according to van't Hoff's equation,dln K/d T = -Q(T) /RT2 , whenln K = Q(T) /RT+const.