Chemistry HSC Formulas

Chemistry HSC Formulas Production of Materials Acid reactions: 

acid + base



acid + metal



acid + carbonate

salt + water

HCl(aq) + NaOH(aq)

salt + hydrogen gas

NaCl(s) + H2O(l)

HCl(aq) + Mg(s)

salt + carbon dioxide gas + water

MgCl2(s) + H2 (g) HCl(aq) + CaCO3(s)

CaCl(s) + CO2(g) + H2O 

acid + hydrogen carbonate

salt + carbon dioxide gas + water

(note: there is CO2

solid, its dry ice) – Complete combustion: 

hydrocarbon + oxygen

water + carbon dioxide

– Displacement reactions: 

X + Y (anion); where Y > X on activity series or Eo table.

Y + X (anion)

 Alkene/alkane reactions: – Cracking of pentane: 

pentane

ethylene + propane



C5H12 (g)

C2H4 (g) + C3H8 (g)

– Hydration of ethylene (the reverse can also happen known as de-hydration, where concentrated acid is used): 

ethylene + water



C2H4 (g) + H2O (l)

ethanol C2H5OH (l)

– Hydrogenation of ethylene: 

ethylene + hydrogen



C2H4 (g) + H2 (g)

ethane C2H6 (g)

– Hydrohalogenation (more specifically, Hydrofluorination) of ethylene: 

ethylene + hydrogen fluoride



C2H4 (g) + HFl (g)

fluoroethane

C2H5Fl (g)

– Reaction of cyclohexene with bromine water: 

cyclohexene + bromine water



C6H10 (l) + Br2 (aq)

2-bromo-1-cyclohexane

C6H10Br2 (aq)

– Reaction of cyclohexane with bromine water (subsitution reaction, only under sunlight, that is UV light): 

C6H12 (l) + Br2(aq) 

C6H11Br(aq) + HBr(aq)

Fermentation and combustion of ethanol:

– Fermentation of glucose: 

glucose



C6H12O6 (aq)



Note: the yeast used is zymase

ethanol + carbon dioxide 2C2H5OH (aq) + 2CO2 (g)

– Combustion of ethanol: 

ethanol + oxygen



C2H5OH (l) + 3O2 (g)

carbon dioxide + water 2CO2 (g) + 3H2O (g) + 1367 kj/mol

 Electrochemistry, an example: – Displacement of copper from solution due to zinc: 

zinc + copper sulfate



Zn (s) + CuSO4 (aq)

zinc sulfate + copper ZnSO4 (aq) + Cu (s)

– Ionic equation: 

zinc + copper(II) ion + sulfate ion



Zn + Cu2+ + SO42-

zinc(II) ion + sulfate ion + copper

Zn2+ + SO42- + Cu

– Net ionic equation: 

zinc + copper(II) ion



Zn (s) + Cu2+ (aq)

Zn2+ (aq) + Cu (s)

– Half-equations: 

Zn



Cu2+ + 2e¯

zinc(II) ion + copper

Zn2+ + 2e¯ Cu

Acidic Environment Acid reactions: 

acid + base



acid + metal

salt + water

HCl(aq) + NaOH(aq)

salt + hydrogen gas

NaCl(s) + H2O(l)

HCl(aq) + Mg(s)

MgCl2(s) + H2

salt + carbon dioxide gas + water

HCl(aq) + CaCO3(s)

(g)



acid + carbonate

CaCl(s) + CO2(g) + H2O 

acid + hydrogen carbonate

salt + carbon dioxide gas + water

there is CO2 solid, its dry ice) – Formation of hydronium: 

H+ + H2O

H3O+

 Reactions of various oxides with water: – Non-metal (acidic) oxides: 

CO2 (g) + H2O (l)

H2CO3 (aq) (carbonic acid)



SO2 (g) + H2O (l)

H2SO3 (aq) (sulfurous acid)



2NO2 (g) + H2O (l)

HNO3 (aq) + HNO2 (aq) (nitric and nitrous acid)



P2O5 (g) + H2O (l)

2H3PO4 (aq) (phosphoric acid)

– Metal (basic) oxides: 

K2O (s) + H2O (l)

2KOH (aq) (potassium hydroxide)



Na2O (s) + H2O (l)

2NaOH (aq) (sodium hydroxide)



MgO (s) + H2O (l)

Mg(OH)2 (aq) (magnesium hydroxide)

 Various equilibrium reactions: – Formation of carbonic acid: CO2 (g) + H2O (l) – Copper complex-ions: Cu(H2O)42+ (aq) + 4Cl‫(־‬aq)

H2CO3 (aq) CuCl42‫(־‬aq) + 4H2O (l)

– Decomposition of dinitrogen tetroxide: N2O4 (g)

2NO2 (g)

– Decomposition of calcium carbonate: CaCO3 (s)

CaO (s) + CO2 (g)

(note:

 Non-Arrhenius acid/base reaction (ie no water present and no free H+ ions): – Gaseous hydrogen chloride and ammonia react: 

HCl

(g) +

NH3 (g)

NH4Cl (s)

 Ionisation of strong and weak acids: H3O+ (aq) + Cl‫( ־‬aq)

– Hydrochloric: HCl (g) + H2O (l)

H3O+ (aq) + NO3-

– Nitric: HNO3 (l) + H2O (l)

2H3O+ (aq) + SO42‫־‬

– Sulfuric: H2SO4 (l) + 2H2O (l)

H3O+ (aq) + CH3COO‫( ־‬aq)

– Ethanoic: CH3COOH (s) + H2O (l)

 Sources of sulfur and nitrogen oxides in the atmosphere: – Sulfur Oxides: 

Organic decomposition: 2H2S (g) + 3O2 (g)



Burning high-sulfur coals: S (s) + O2 (g)



Smelting metal sulfides: 2PbS (s) + 3O2 (g)

2SO2 (g) + 2H2O (l) SO2 (g) 2PbO (s) + 2SO2

– Nitrogen Oxides: 

Lightning: N2 (g) + O2 (g)



Further Catalysed by oxygen particles: 2NO (g) + O2 (g)

2NO (g) NO2 (g)

 Amphiprotic substances: – Hydrogen carbonate (ie bicarbonate): 

HCO3‫( ־‬aq) + H3O+ (aq)



HCO3‫( ־‬aq) + OH ‫( ־‬aq)

H2CO3 (aq) + H2O (l) CO32‫( ־‬aq) + H2O (l)

 Natural Buffers: – The carbonic acid/hydrogen carbonate ion buffer in the mammalian blood system: 

H3O+ (aq) + HCO3‫( ־‬aq)

H2CO3 (aq) + H2O (l)

 Esterification: – General word-formula: 

acid + alcohol



alkanoic acid + alkanol

ester + water ester + water

– Example: 

butanoic acid + pentanol



C3H7COOH (aq) + C5H11OH (l)

pentyl butanoate C3H7COOCH2C4H9 (aq) + H2O (l)

Chemical Monitoring & Management Different products under different conditions: 

Complete combustion:  propane + oxygen  C3H8 (g) + 5O2 (g)



carbon dioxide + water 3CO2 (g) + 4H2O (g)

Incomplete combustion:  propane + oxygen  C3H8 (g) + 3O2 (g)

carbon + carbon monoxide + water C (s) + 2CO (g) + 4H2O (g)

– Reaction of ammonia to form important products: 

Common Fertiliser:  NH3 (g) + HNO3 (aq)

NH4NO3 (aq)

 NH3 (g) + H2SO4 (aq) 

(NH4)2SO4 (aq)

Nitric acid (through the Ostwald Process).  NH3 (g) + 2O2 (g)

HNO3 (g) + H2O (l)

– Haber Process: 

nitrogen + hydrogen



N2 (g) + 3H2 (g)

ammonia + heat 2NH3 (g)

∆H = -92 kJ/mol

– Sulfate Content in Fertilizer: 

barium chloride + sulfate



BaCl2 (aq) + SO42- (aq)

barium sulfate + chloride BaSO4 (s) + 2Cl- (aq)

– How Ozone Protects Us From UV Radiation: 

Oxygen reacts with UV, forming 2 radicals:  O2 + UV radiation



Radical reacts with oxygen, forming ozone:  O· + O2



O3

Ozone reacts with UV, forming oxygen and a radical:  O3 + UV radiation



2O·

O· + O2

Radical reacts with ozone, creating oxygen:  O· + O3

2O2

-

All the CFC-Related Equations: 

Formation of chlorine radical:  CCl2F2 (g) + UV radiation



Reaction of ozone:  ·Cl (g) + O3 (g)



·Cl (g) + O2 (g)

Removal of chlorine radical:  ·Cl (g) + CH4 (g)



·ClO (g) + O2 (g)

Regeneration of chlorine:  ·ClO (g) + O (g)



HCl (g) + ·CH3 (g)

Removal of chlorine monoxide radical:  ·ClO (g) + NO2 (g)



ClONO2 (g)

Formation of molecular chlorine:  HCl (g) + ClONO2 (g)



·Cl (g) + ·CClF2 (g)

Cl2 (g) + HNO3 (g)

Decomposition of molecular chlorine:  Cl2 (g) + UV radiation

2·Cl (g)

– The Heavy-Metal Sulfide Test: 

The sulfide-test is based on the following equilibrium:  S2- (aq) + 2H3O+ (aq)

H2S (aq) + 2H2O (l)