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The contact process is the current method of producing sulfuric acid in the high concentrations needed for industrial processes. Platinum used to be the 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.
This process was patented in 1831 by British vinegar merchant Peregrine Phillips. 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.
The process can be divided into five stages:
- combining of sulfur and oxygen
- purifying sulfur dioxide in the purification unit
- adding excess of oxygen to sulfur dioxide in presence of catalyst vanadium pentoxide, with temperatures of 450 °C and pressure of 1-2 atm
- sulfur trioxide formed is added to sulfuric acid which gives rise to oleum (disulfuric acid)
- the oleum then is added to water to form sulfuric acid which is very concentrated.
To conserve energy, the mixture is heated by exhaust gases from the catalytic converter by heat exchangers.
Sulfur dioxide and oxygen then react as follows:
- 2 SO2(g) + O2(g) ⇌ 2 SO3(g) : ΔH = -197 kJ·mol−1
According to the Le Chatelier's principle, a lower temperature should be used to shift the chemical equilibrium towards the right, hence increasing the percentage yield. However too low of a temperature will lower the formation rate to an uneconomical level. Hence to increase the reaction rate, high temperatures (450 °C), medium pressures (1-2 atm), and vanadium(V) oxide (V2O5) are used to ensure a 96% 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:
- Oxidation of SO2 into SO3 by V5+:
- 2SO2 + 4V5+ + 2O2− → 2SO3 + 4V4+
- Oxidation of V4+ back into V5+ by oxygen (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(l) + SO3(g) → H2S2O7(l)
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(l) + H2O(l) → 2 H2SO4(l)
This includes the dusting tower, cooling pipes, washing tower, drying tower, arsenic purifier and testing box. Sulfur dioxide has many impurities such as vapours, dust particles and arsenous oxide. Therefore, it must be purified to avoid catalyst poisoning (ie: destroying catalytic activity and loss of efficiency). In this process, the gas is washed with water, and dried by sulfuric acid. In the dusting tower, the sulfur dioxide is exposed to a steam which removes the dust particles. After the gas is cooled, the sulfur dioxide enters the washing tower where it is sprayed by water to remove any soluble impurities. In the drying tower, sulfuric acid is sprayed on the gas to remove the moisture from it. Finally, arsenic oxide is removed when the gas is exposed to ferric hydroxide.
The next step to the Contact Process is DCDA or Double Contact Double Absorption. 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 resulting not only achieving high conversion efficiency for SO2 but also enabling production of 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.
- On March 21, 1831, Peregrine Phillips, Jr., a vinegar manufacturer in Bristol, England, received British patent 6096 for "Certain improvements in manufacturing sulfuric acid, … " See:
- The Repertory of Patent Inventions … , no. 72 (April 1831), page 248.
- (Anon.) (1832) "English patents: Specification of the patent granted to Peregrine Phillips, Jr. of Bristol, in the county of Somersetshire, Vinegar Maker, for an improvement in manufacturing Sulphuric Acid. Dated March 21, 1831." Journal of the Franklin Institute, new series, vol. 9, pages 180-182.
- Ernest Cook (March 20, 1926) "Peregrine Phillips, the inventor of the contact process for sulphuric acid," Nature, 117 (2942) : 419-421.
- George Lunge, Theoretical and Practical Treatise on the Manufacture of Sulphuric Acid and Alkali, with the Collateral Branches, 3rd ed., vol. 1, part 2 (London, England: Gurney and Jackson, 1903), page 975.