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Catalysts for fuel cell application would need to operate at low temperatures. Since the WGSR is slow at lower temperatures where equilibrium favors hydrogen production, WGS reactors require large amounts of catalysts, which increases their cost and size beyond practical application. [2]
The WGSR also requires a catalyst, typically over iron oxide or other oxides. The byproduct is CO 2. [35] Depending on the quality of the feedstock (natural gas, naphtha, etc.), one ton of hydrogen produced will also produce 9 to 12 tons of CO 2, a greenhouse gas that may be captured. [36]
The name-giving reaction is the steam reforming (SR) reaction and is expressed by the equation: [] + + = /Via the water-gas shift reaction (WGSR), additional hydrogen is released by reaction of water with the carbon monoxide generated according to equation [1]:
WGSR may refer to: WGSR-LD, a low-power television station (channel 19) licensed to serve Reidsville, North Carolina, United States; Water-gas shift reaction
The first step in the WGS reaction is the high temperature shift which is carried out at temperatures between 320 °C and 450 °C. As mentioned before, the catalyst is a composition of iron-oxide, Fe 2 O 3 (90-95%), and chromium oxides Cr 2 O 3 (5-10%) which have an ideal activity and selectivity at these temperatures.
As a hydrogenation catalyst, Urushibara cobalt is used for nitrile reduction where it serves as a superior catalyst for the production of primary amines. [3] Urushibara iron is limited as a catalyst due to its relatively low activity toward most functional groups, however; it does finds some use in the partial hydrogenation of alkynes to alkenes.
Squaramide catalysts are easily prepared from starting materials like methyl squarate, possess high activities under low catalyst loadings. Squaramide catalysis can be a replacement for thiourea organocatalysis in some scenarios. [2] [3] Squaramides have higher affinity for halide ions than thiourea. [4] Aqueous mediums can be used. [1]
Paul Sabatier (1854-1941) winner of the Nobel Prize in Chemistry in 1912 and discoverer of the reaction in 1897. The Sabatier reaction or Sabatier process produces methane and water from a reaction of hydrogen with carbon dioxide at elevated temperatures (optimally 300–400 °C) and pressures (perhaps 3 MPa [1]) in the presence of a nickel catalyst.