Formerly inorganic processes were used, employing the electrolysis of an aqueous solution of sulfuric acid or acidic ammonium bisulfate (NH4HSO4), followed by hydrolysis of the peroxodisulfate ((SO4)2)2− which is formed.

However, today hydrogen peroxide is manufactured almost exclusively by the autoxidation of a 2-alkyl anthrahydroquinone (or 2-alkyl-9,10-dihydroxyanthracene) to the corresponding 2-alkyl anthraquinone. Major producers commonly use either the 2-ethyl or the 2-amyl derivative. The cyclic reaction depicted below, shows the 2-ethyl derivative, where 2-ethyl-9,10-dihydroxyanthracene (C16H14O2), is oxidized to the corresponding 2-ethylanthraquinone (C16H12O2) and hydrogen peroxide. Most commercial processes achieve this by bubbling compressed air through a solution of the anthracene, whereby the oxygen present in the air reacts with the labile hydrogen atoms (of the hydroxy group) giving hydrogen peroxide and regenerating the anthraquinone. Hydrogen peroxide is then extracted out and the anthraquinone derivative reduced back to the dihydroxy (anthracene) compound using hydrogen gas in the presence of a metal catalyst. The cycle then repeats itself.1011
Hydrogen peroxide production with the Riedl-Pfleiderer process process

This process is known as the Riedl-Pfleiderer process11, having been first discovered by them in 1936. The overall equation for the process is deceptively simple:10

H2 + O2 → H2O2

It is important to point out that the economics of the process depend heavily on effective recycling of the quinone (which is very expensive) and extraction solvents, and of the hydrogenation catalyst.

In 1994, world production of H2O2 was around 1.9 million tonnes and grew to 2.2 million in 2006,12 most of which was at a concentration of 70% or lessneeded. In that year bulk 30% H2O2 sold for around US $0.54 per kg, equivalent to US $1.50 per kg (US $0.68 per lb) on a "100% basisneeded".
Source(s):
http://en.wikipedia.org/wiki/Hydrogen_peroxide

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