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|OTP appearance||colorless noxious|
|Solubility in water(g/L)||94|
|Speed of sound
20°C, 1atm (m/s)
|Immediate Danger to Life and Health||100ppm|
- Sulfur dioxide occurs naturally in volcanic vents and sulfur springs
- Inhalation of large amounts of sulfur dioxide can result in pulmonary edema, which (according to ) is treated with supportive care for breathing and heart issues.
There are many ways to produce sulfur dioxide depending on the raw materials available. Each of the below produces approximately 1 mol of sulfur dioxide:
Molten sulfur combines with air almost quantitatively producing sulfur dioxide:
- Burn (or melt) 1 mol (32g) of sulfur in air
- S8 + 8 O2 → 8 SO2
Thermal decomposition of mineral sulfides and sulfates
- Roast 1 mol (240g) of galena in air at 1000°C
- 2 PbS + 3 O2 → 2 PbO + 2 SO2
- Roast 1/2 mol (60g) of iron pyrite in air
- 4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2
- Roast 5/6 mol (113.3g) of gypsum and 1/6 mol (20g) of iron pyrite with 1/2 mol (30g) of silicon dioxide
- Very roughly, 1ubm of sulfite to 2 ubm of commercial or 1:3 of azeotropic HCl produces SO2
- Gather 126ubm (1M) sodium sulfite
- Gather 500ubm of water
- Gather 255ubm (222ml, 2M) of commercial (30%-ish, 9M) hydrochloric acid
- or 365ubm (333ml, 2M) of azeotropic (20.2%, 6M) hydrochloric acid
- Completely dissolve the sodium sulfite in the water.
- Drip hydrochloric acid into sodium sulfite solution producing 2 mols of salt, 1 mol of water, and 1 mol of sulfur dioxide
- Na2SO3 + 2 HCl → 2 NaCl + SO2 + H2O
- Sulfur dioxide is only slightly soluble in water, whereas sulfur trioxide reacts, and carbon dioxide is very soluble. Bubbling through warm water, therefore, will remove the bulk of these compounds.
- A paper strip made with a solution of potassium permanganate will rapidly turn from purple to brown in the presence of sulfur dioxide
- Sulfur dioxide will decolor a solution of potassium permanganate rapidly
- A practical way to contain and store sulfur dioxide effluent is to combine it with sodium hydroxide, producing sodium bisulfite. Sodium bisulfite is readily convertible back to sulfur dioxide by adding almost any acid.
- SO2(g) + NaOH(aq) → NaHSO3 // put
- NaHSO3 + HCl → NaCl + H2O(l) + SO2(g) // get
- Burn with hydrogen sulfide producing elemental sulfur and water
- SO2 + 2 H2S → 2 H2O + 3 S
- Bubble through a solution of potassium permanganate
- 5 SO2 + 2 KMnO4 + 2 H2O → 2 H2SO4 + 2 MnSO4 + K2SO4
courtesy US CDC.