Contact process

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For the stochastic process used to model population, see Contact process (mathematics).

The contact process is the current method of producing

catalyst for this reaction; however, as it is susceptible to reacting with arsenic impurities in the sulfur feedstock, vanadium(V) oxide (V2O5) is now preferred.[1]

History

This process was patented in 1831 by British vinegar merchant Peregrine Phillips.[2][3][4] In addition to being a far more economical process for producing concentrated sulfuric acid than the previous lead chamber process, the contact process also produces sulfur trioxide and oleum.

In 1901 Eugen de Haën patented the basic process involving combining sulfur dioxide and oxygen in the presence of vanadium oxides, producing sulfur trioxide which was easily absorbed into water, producing sulfuric acid.[5] This process was improved remarkably by shrinking the particle size of the catalyst (e.g. ≤ 5000 microns), a process discovered by two chemists of BASF in 1914.[6][7][8]

Process

The process can be divided into four stages:

  1. Combining of sulfur and oxygen (O2) to form sulfur dioxide, then purify the sulfur dioxide in a purification unit
  2. Adding an excess of oxygen to sulfur dioxide in the presence of the catalyst vanadium pentoxide at 450 °C and 1-2 atm
  3. The sulfur trioxide formed is added to sulfuric acid which gives rise to oleum (disulfuric acid)
  4. The oleum is then added to water to form sulfuric acid which is very concentrated. Since this process is an exothermic reaction, the reaction temperature should be as low as possible.

Purification of the air and sulfur dioxide (SO2) is necessary to avoid catalyst poisoning (i.e. removing catalytic activities). The gas is then washed with

water
and dried with sulfuric acid.

To conserve energy, the mixture is heated by exhaust gases from the catalytic converter by heat exchangers.

Sulfur dioxide and dioxygen then react as follows:

2 SO2(g) + O2(g) ⇌ 2 SO3(g) : ΔH = -197 kJ·mol−1

According to the

atm), and vanadium(V) oxide (V2O5) are used to ensure an adequate (>95%) conversion. The catalyst only serves to increase the rate of reaction as it does not change the position of the thermodynamic equilibrium
. The mechanism for the action of the catalyst comprises two steps:

  1. Oxidation of SO2 into SO3 by V5+:
    2SO2 + 4V5+ + 2O2− → 2SO3 + 4V4+
  2. Oxidation of V4+ back into V5+ by dioxygen (catalyst regeneration):
    4V4+ + O2 → 4V5+ + 2O2−

Hot sulfur trioxide passes through the heat exchanger and is dissolved in concentrated H2SO4 in the absorption tower to form oleum

H2SO4 + SO3 → H2S2O7

Note that directly dissolving SO3 in water is impractical due to the highly exothermic nature of the reaction. Acidic vapor or mists are formed instead of a liquid.

Oleum is reacted with water to form concentrated H2SO4.

H2S2O7 + H2O → 2 H2SO4

Purification unit

This includes the dusting tower, cooling pipes, scrubbers, drying tower, arsenic purifier and testing box. Sulfur dioxide has many impurities such as vapours, dust particles and

ferric hydroxide
.

Double contact double absorption

The next step to the contact process is double contact double absorption (DCDA). In this process the product gases (SO2) and (SO3) are passed through absorption towers twice to achieve further absorption and conversion of SO2 to SO3 and production of higher grade sulfuric acid.

SO2-rich gases enter the catalytic converter, usually a tower with multiple catalyst beds, and are converted to SO3, achieving the first stage of conversion. The exit gases from this stage contain both SO2 and SO3 which are passed through intermediate absorption towers where sulfuric acid is trickled down packed columns and SO3 reacts with water increasing the sulfuric acid concentration. Though SO2 too passes through the tower it is unreactive and comes out of the absorption tower.

This stream of gas containing SO2, after necessary cooling is passed through the catalytic converter bed column again achieving up to 99.8% conversion of SO2 to SO3 and the gases are again passed through the final absorption column thus achieving not only high conversion efficiency for SO2, but also enabling production of a higher concentration of sulfuric acid.

The industrial production of sulfuric acid involves proper control of temperatures and flow rates of the gases as both the conversion efficiency and absorption are dependent on these.

See also

Notes

  1. ^ "History". Ravensdown. Archived from the original on May 23, 2010. Retrieved March 1, 2010.
  2. ISBN 9780905118833
    .
  3. ^ UK 6093, Peregrine Phillips Junior, "Manufacturing of Sulphuric Acid", issued 1831 
  4. ISBN 9783642932786
    .
  5. ^ US 687834A, Carl Johann Eugen de Haën, "Method of Making Sulfuric Anhydrid", issued 1901-12-03 
  6. ^ US 1371004, Franz Slama & Hans Wolf, "Oxidation of sulfur dioxid and catalyst therefor", issued 1921-05-8, assigned to General Chemical Company 
  7. ISBN 9783642932786
    .
  8. ISBN 9788187224990
    .

References

External links

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