Transcript Chemistry of Explosives
Explosive Properties
Explosives 189 Dr. Van Romero 26 Jan 2012
Some Definitions
• Explosion – rapid expansion of matter into a volume much greater than the original volume
Some Definitions
• • Explosion – rapid expansion of matter into a volume much greater than the original volume Burn & Detonate – Both involve oxidation – Burn – relatively slow – Detonate – burning at a supersonic rate producing a pressure Wave
Some Definitions
• • • Explosion – rapid expansion of matter into a volume much greater than the original volume Burn & Detonate – Both involve oxidation – Burn – relatively slow – Detonate – burning at a supersonic rate producing a pressure Wave Deflagration – Burning to detonation (DDT)
Some Definitions
• • • • Explosion – rapid expansion of matter into a volume much greater than the original volume Burn & Detonate – Both involve oxidation – Burn – relatively slow – Detonate – burning at a supersonic rate producing a pressure Wave Deflagration – Burning to detonation (DDT) Shock wave – High pressure wave that travels faster then the speed of sound
Explosives Vs. Propellants
• The difference between an explosive and a propellant is functional as apposed to fundamental.
Explosives Vs. Propellants
• • The difference between an explosive and a propellant is functional as apposed to fundamental.
Explosives are intended to function by detonation from shock initiation (High
Explosives)
Explosives Vs. Propellants
• • Propellants are initiated by burning and then burn at a steady rate determined by the devise, i.e. gun (Low Explosives) Single molecule explosives are categorized by the required initiation strength
Primary Explosives
• Primary Explosives – Transit from surface burning to detonation within a very small distance. – Lead Azide (PbN 6 )
Secondary Explosives
• • Secondary Explosives – Can burn to detonation, but only in relatively large quantities. Secondary explosives are usually initiated from the shock from a primary explosive (cap sensitive) TNT
Tertiary Explosives
• • Tertiary Explosives – Extremely difficult to initiate. It takes a significant shock (i.e. secondary explosive) to initiate. Tertiary explosives are often classified as non explosives.
Ammonium Nitrate (NH 4 NO 3 )
Exothermic and Endothermic Reactions
• Chemical reaction – Reactants Products.
– Internal energy of reactants ≠ internal energy of products.
– Internal energy: contained in bonds between atoms.
– Reactants contain more energy than products— energy is released as heat.
– EXOTHERMIC Reaction.
Exothermic and Endothermic Reactions
• • • • Products contain more internal energy than reactants ENDOTHERMIC Reaction Energy must be added for the reaction to occur.
Burning and detonation are
Exothermic and Endothermic Reactions
• • • • Products contain more internal energy than reactants ENDOTHERMIC Reaction Energy must be added for the reaction to occur.
Burning and detonation are Exothermic
Oxidation: Combustion
• Fuel + Oxidizer Products (propellant)
Oxidation: Combustion
• Fuel + Oxidizer Products (propellant) • CH 4 + 2 O 2 Methane Oxygen CO 2 Carbon Dioxide + 2 H 2 0 Water
Oxidation: Combustion
• Fuel + Oxidizer Products (propellant) • • CH 4 + 2 O 2 Methane Oxygen CO 2 Carbon Dioxide + 2 H 2 Water 0 Oxidation (combustion) of methane • 1 methane molecule : 2 oxygen molecules (4 oxygen atoms).
Oxidation: Decomposition
• Oxidizer + Fuel (Explosive) decomposition to products
Oxidation: Decomposition
• • • Oxidizer + Fuel decomposition to products (Explosive) Example: Nitroglycol O 2 N — O — CH 2 — CH 2 — O — NO 2 Fuel (Hydrocarbon) + Oxidizer (Nitrate Esters)
Oxidation: Decomposition
• • • • Oxidizer + Fuel decomposition to products (Explosive) Example: Nitroglycol O 2 N — O — CH 2 — CH 2 — O — NO 2 Fuel (Hydrocarbon) + Oxidizer (Nitrate Esters) Undergoes Decomposition to: 2 CO 2 + 2 H 2 O + N 2 Carbon Dioxide Water Nitrogen
CHNO Explosives
• • • • Many explosives and propellants are composed of: – Carbon – Hydrogen – – Nitrogen Oxygen General Formula: C c H h N n O o c, h, n, o are # of carbon, hydrogen, nitrogen and oxygen atoms.
For Nitroglycol: C 2 H 4 N 2 O 6
CHNO Explosive Decomposition
• • C c H h N n O o c C + h H + n N + o O Imagine an explosive detonating.
– Reactant CHNO molecule is completely broken down into individual component atoms.
• • •
CHNO Explosive Decomposition
C c H h N n O o c C + h H + n N + o O Imagine an explosive detonating.
– Reactant CHNO molecule is completely broken down into individual component atoms.
For Nitroglycol: – – – – 2N N 2 2H + O C + O H 2 0 CO CO + O CO 2
• • • • •
Overoxidation vs Underoxidation
In the case of nitroglycol O 2 N—O—CH 2 —CH 2 —O—NO 2 2 CO 2 + 2 H 2 O + N 2 Exactly enough oxygen to burn all carbon to CO 2 Some have more than enough oxygen to burn all the carbon into CO 2 – OVEROXIDIZED OR FUEL LEAN Most explosives do not have enough oxygen to burn all the carbon to CO 2 – UNDEROXIDIZED OR FUEL RICH
Simple Product Hierarchy for CHNO Explosives
• First, all nitrogen forms N 2
Simple Product Hierarchy for CHNO Explosives
• • First, all nitrogen forms N 2 Then, all the hydrogen is burned to H 2 O
Simple Product Hierarchy for CHNO Explosives
• • • First, all nitrogen forms N 2 Then, all the hydrogen is burned to H 2 O Any oxygen left after H 2 0 formation burns carbon to CO.
Simple Product Hierarchy for CHNO Explosives
• • • • First, all nitrogen forms N 2 Then, all the hydrogen is burned to H 2 O Any oxygen left after H 2 0 formation burns carbon to CO.
Any oxygen left after CO formation burns CO to CO 2
Simple Product Hierarchy for CHNO Explosives
• • • • • First, all nitrogen forms N 2 Then, all the hydrogen is burned to H 2 O Any oxygen left after H 2 0 formation burns carbon to CO.
Any oxygen left after CO formation burns CO to CO 2 Any oxygen left after CO 2 formation forms O 2
Simple Product Hierarchy for CHNO Explosives
• • • • • • First, all nitrogen forms N 2 Then, all the hydrogen is burned to H 2 O Any oxygen left after H 2 0 formation burns carbon to CO.
Any oxygen left after CO formation burns CO to CO 2 Any oxygen left after CO 2 formation forms O 2 Traces of NO x (mixed oxides of nitrogen) are always formed.
Decomposition of Nitroglycerine
• • C 3 H 5 N 3 O 9 – 3N 1.5 N 2 3C + 5H + 3N + 9O – – 5H + 2.5O 2.5 H 2 O (6.5 O remaining) 3C + 3O 3 CO (3.5 O remaining) – 3 CO 3O 3 CO 2 (0.5 O remaining) 8.5 of 9 oxygen atoms consumed – 0.5 O 0.25 O 2
Decomposition of Nitroglycerine
• • • • C 3 H 5 N 3 O 9 – 3N 1.5 N 2 3C + 5H + 3N + 9O – – 5H + 2.5O 2.5 H 2 O (6.5 O remaining) 3C + 3O 3 CO (3.5 O remaining) – 3 CO + 3O 3 CO 2 (0.5 O remaining) 8.5 of 9 oxygen atoms consumed – 0.5 O 0.25 O 2 Overall Reaction: – C 3 H 5 N 3 O 9 1.5 N 2 + 2.5 H 2 O + 3 CO 2 + 0.25 O 2 Oxygen Remaining = Nitroglycerine is – OVEROXIDIZED
Decomposition of RDX
H 2 • C 3 H 6 N 6 O 6 – 6N 3N 2 – 6H + 3O 3C + 6H +6N +6O 3H 2 O (3 O remaining) – 3C + 3O 3CO (All O is consumed) – No CO 2 formed.
H 2 H 2
Decomposition of RDX
H 2 • • • C 3 H 6 N 6 O 6 – – 6N 3N 2 6H + 3O – 3C + 3O 3C + 6H +6N +6O 3H 2 O (3 O remaining) 3CO (All O is consumed) – No CO 2 formed.
Overall Reaction: – C 3 H 6 N 6 O 6 3 N 2 + 3 H 2 O + 3 CO Not enough oxygen to completely burn all of the fuel – UNDEROXIDIZED H 2 H 2
Oxygen Balance
• • OB (%) – 1600/MW exp [oxygen-(2 carbon+ hydrogen/2)] Oxygen balance for Nitroglycol C 2 H 4 N 2 O 6 – c = 2, h = 4, n = 2, o = 6 – Mw exp =12.01 (2) + 1.008 (4) + 14.008 (2) + 16.000 ( 6) = 152.068 g/mol – 152.068
6 – 2 (2) – 4 2
Perfectly Balanced
Oxygen Balance
• Oxygen balance for Nitroglycerine C 3 H 5 N 3 O 9 – C = 3, h = 5, n = 3, o = 9 – Mw exp =12.01 (3) + 1.008 (5) + 14.008 (3) + 16.000 ( 9) = 227.094 g/mol – 9 – 2 ( 3) – 5 2
Slightly overoxidized
Oxygen Balance
• Oxygen balance for RDX: C 3 H 6 N 6 O 6 – C = 3, h = 6, n = 6, o = 6 – Mw exp =12.01 (3) + 1.008 (6) + 14.008 (6) + 16.000 ( 6) = 222.126 g/mol – 6 – 2 ( 3) – 6 2
Underoxidized
Homework
• Calculate the oxygen balance for: – TNT – Picric Acid