Editing Lead chamber process (section)

== Chemistry ==
Sulfur dioxide is generated by burning elemental sulfur or by roasting [[Pyrite|pyritic ore]] in a current of air:

:S<sub>8</sub> + 8 O<sub>2</sub> → 8 SO<sub>2</sub> 
:4 FeS<sub>2</sub> + 11 O<sub>2</sub> → 2 Fe<sub>2</sub>O<sub>3</sub> + 8 SO<sub>2</sub>

Nitrogen oxides are produced by decomposition of niter in the presence of sulfuric acid, or by hydrolysis of nitrosylsulfuric acid:

:2 NaNO<sub>3</sub> + H<sub>2</sub>SO<sub>4</sub> → Na<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O + NO + NO<sub>2</sub> + O<sub>2</sub>
:2 NOHSO<sub>4</sub> + H<sub>2</sub>O →  2 H<sub>2</sub>SO<sub>4</sub> + NO + NO<sub>2</sub>

In the reaction chambers, sulfur dioxide and nitrogen dioxide dissolve in the reaction liquor. Nitrogen dioxide is hydrated to produce [[nitrous acid]], which then oxidizes the sulfur dioxide to sulfuric acid and nitric oxide. The reactions are not well characterized, but it is known that nitrosylsulfuric acid is an intermediate in at least one pathway. The major overall reactions are:

:2 NO<sub>2</sub> + H<sub>2</sub>O → HNO<sub>2</sub> + HNO<sub>3</sub>
:SO<sub>2</sub> (aq) + HNO<sub>3</sub> → NOHSO<sub>4</sub>
:NOHSO<sub>4</sub> + HNO<sub>2</sub> →  H<sub>2</sub>SO<sub>4</sub> + NO<sub>2</sub> + NO
:SO<sub>2</sub> (aq) + 2 HNO<sub>2</sub> → H<sub>2</sub>SO<sub>4</sub> + 2 NO

Nitric oxide escapes from the reaction liquor and is subsequently reoxidized by molecular oxygen to nitrogen dioxide.  This is the overall rate determining step in the process:<ref>Jones, pp 2209.</ref>

:2 NO + O<sub>2</sub> → 2 NO<sub>2</sub>

Nitrogen oxides are absorbed and regenerated in the process, and thus serve as a [[catalyst]] for the overall reaction:

:2 SO<sub>2</sub> + 2 H<sub>2</sub>O + O<sub>2</sub> → 2 H<sub>2</sub>SO<sub>4</sub>