Properties of Sulfuric acidPhysicalChemicalStandard ReactionsStructuralManufacturing ProcessIndustrial and Laboratory UsageEnvironmental and Health Issues

Chemical Formula:H2SO4Appearance:Transparent [colourless]Texture:OilyMolar Mass:98.078g/molBoiling Point:315-338CMelting Point:10.35CDensity:1.84g/cc [25C]Heat Capacity:1.414J/Kg

Acidity:-3 pHAcid Type:DiproticCorrosiveness:Very HighReactivity: HighSolubility: MiscibleOxidizing Power:HighVolatility:Low

The Contact ProcessCombustion ChamberPurifierElectrostatic Precipitator

Conversion ChamberT = 450CP = 1-2atmV2O5Absorption TowersWet Sulfuric AcidHydration of Disulfuric AcidH2SO4Recycling of Unreacted Material[Impurities]

The Contact Process Step by step of contact process

1.Combustion of sulfur to sulfur dioxide2. Oxidation of sulfur dioxide to sulfur trioxide3. Reaction of sulfur trioxide and sulfuric acid 4.Hydration of disulfuric acid yielding sulfuric acid as product

Equations of contact process

S(s) + O2(g) SO2(g) 2SO2(g) + O2(g) 2SO3(g) [Done via a vanadium oxide catalyst V2O5]3.(a) SO3(g) + H2O(l) H2SO4 (aq) [WSAP] (b) SO3(g) + H2SO4 (aq) H2S2O7 (aq) [DCDA]4. H2S2O7 (aq) + H2O(l) 2H2SO4 (aq)

An electrochemical cell capable of a reverse reaction.Sulfuric acid is used as the electrolyte solutionCathode reaction:PbO2 (s) +4H+ (aq) + 2e- Pb2+ +2H2O (l)Anode reaction:Pb (s) Pb2+ (aq) +2e-

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English land-owner John Lawes discovered in 1842 a technique to produce a superphosphate.

Supplies soil with the required nutrients for healthy growth

Pickling is the treatment of metallic surfaces to remove impurities, stains and rust via a solution.The surface is dipped in a solution known as a pickle liquor which is usually an acid.Two most commonly used acids are sulfuric and hydrochloric.Due to the pickle liquors corrosive properties, hydrogen embrittlement can occur.Hydrogen from the acid reacts with the metal surface causing cracks and thus an overall loss in strength.

[1]The drying capability of sulfuric acid enables it to char organic molecules; as water is extracted.This effect can be observed when concentrated sulfuric acid is added to sucrose.Since sucrose is a carbohydrate, when the water is extracted we are left with elemental carbon

C11H22O12 (s) + 11H2SO4 (aq) 12C(s) + 11[H2SO4 . H2O]

[1] Slater B, The chemistry dimension

Due to sulfuric acids low volatility it can be used in the manufacture of other acids such as HCl, HF, HNO3.The general equation is shown below.

2XyYx + xyH2SO4 2xHyY + yX2 [SO4]x

Where:XyYx = SaltX = Metal componentY = Non metal componentx,y = valence of x and y respectively

This is not the case for the preparation of some acids, as the reactions will only proceed at high temperatures [550-600]o

The second equation is for salts that have a high reaction rate.

XyYx +xyH2SO4 xHyY + yX [H2SO4]x

Due to its dehydrating ability, contact with the skin will result in third degree burns.

Occurs because the reaction is exothermic, as the amount of water drawn from the skin increases, the intensity also increases

Sulfuric acid produced in the earths atmosphere is transferred to Earth most commonly as precipitation called acid rain.

Generally has a pH between 4.3 -5.0.

Caused mainly by industrial emissions such as combustion of fossil fuels causing particular emissions of SO2 and NOx

Decaying vegetation and erupting volcanoes contribute up to 20% of the emissions of SO2 and NOx