3 NO2 (l) + H2O (l) → 2 HNO3 (aq) + NO (g)
This is an oxidation-reduction (redox) reaction:
NIV + 2 e- → NII (reduction)
2 NIV - 2 e- → 2 NV (oxidation)
NO2 is both an oxidizing and a reducing agent (disproportionation (dismutation)).
Reactants:
- NO2 – Nitrogen dioxide
- Other names: Nitrogen(IV) oxide , Deutoxide of nitrogen , Nitrogen peroxide
- Appearance: Brown gas ; Reddish-brown gas or brown or yellow liquid with pungent odour ; Yellowish-brown liquid or reddish-brown gas (above 70°F) with a pungent, acrid odor. [Note: In solid form (below 15°F) it is found structurally as N2O4.]
- H2O – Water, oxidane
Products:
- HNO3 – Nitric acid
- Other names: Aqua fortis , Spirit of niter , Eau forte
- Appearance: Colorless, yellow or red fuming liquid ; Colourless-to-yellow liquid with pungent odour ; Colorless, yellow, or red, fuming liquid with an acrid, suffocating odor. [Note: Often used in an aqueous solution. Fuming nitric acid is concentrated nitric acid that contains dissolved nitrogen dioxide.]
- NO – Nitrogen monoxide , Oxidonitrogen(•) (additive)