This video shows how to predict products in combustion reactions, including several varieties of reactions with oxygen. See end links for other videos in this series
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- Stoichiometry
- Quantum Numbers
- Rutherford's Gold Foil Experiment, Explained
- Covalent Bonding Tutorial: Covalent vs. Ionic bonds
- Metallic Bonding and Metallic Properties Explained: Electron Sea Model
- Effective Nuclear Charge, Shielding, and Periodic Properties
- Electron Configuration Tutorial + How to Derive Configurations from Periodic Table
- Orbitals, the Basics: Atomic Orbital Tutorial - probability, shapes, energy
- Metric Prefix Conversions Tutorial
- Gas Law Practice Problems: Boyle's Law, Charles Law, Gay Lussac's, Combined Gas Law
- Ionic Bonds and Compounds
- Chemical reaction types
- product prediction for specific reaction types
- Surface Tension
- what is heat
- what is fire
- The Bohr Model of the Atom
- Organic Molecules and the Versatility of Carbon
- Hybrid Orbitals-- Valence Bond Theory
- Ideal Gas Law and Gas Density
-More on Combustion | Wikipedia- Nov 2019
Combustion, or burning, is a high-temperature exothermic redox chemical reaction between a fuel (the reductant) and an oxidant, usually atmospheric oxygen, that produces oxidized, often gaseous products, in a mixture termed as smoke. Combustion in a fire produces a flame, and the heat produced can make combustion self-sustaining. Combustion is often a complicated sequence of elementary radical reactions. Solid fuels, such as wood and coal, first undergo endothermic pyrolysis to produce gaseous fuels whose combustion then supplies the heat required to produce more of them. Combustion is often hot enough that incandescent light in the form of either glowing or a flame is produced. A simple example can be seen in the combustion of hydrogen and oxygen into water vapor, a reaction commonly used to fuel rocket engines. This reaction releases 242 kJ/mol of heat and reduces the enthalpy accordingly (at constant temperature and pressure):
Combustion of an organic fuel in air is always exothermic because the double bond in O2 is much weaker than other double bonds or pairs of single bonds, and therefore the formation of the stronger bonds in the combustion products CO2 and H2O results in the release of energy.[2] The bond energies in the fuel play only a minor role, since they are similar to those in the combustion products; e.g., the sum of the bond energies of CH4 is nearly the same as that of CO2. The heat of combustion is approximately -418 kJ per mole of O2 used up in the combustion reaction, and can be estimated from the elemental composition of the fuel.
Uncatalyzed combustion in air requires fairly high temperatures. Complete combustion is stoichiometric with respect to the fuel, where there is no remaining fuel, and ideally, no remaining oxidant. Thermodynamically, the chemical equilibrium of combustion in air is overwhelmingly on the side of the products. However, complete combustion is almost impossible to achieve, since the chemical equilibrium is not necessarily reached, or may contain unburnt products such as carbon monoxide, hydrogen and even carbon (soot or ash). Thus, the produced smoke is usually toxic and contains unburned or partially oxidized products. Any combustion at high temperatures in atmospheric air, which is 78 percent nitrogen, will also create small amounts of several nitrogen oxides, commonly referred to as NOx, since the combustion of nitrogen is thermodynamically favored at high, but not low temperatures. Since combustion is rarely clean, flue gas cleaning or catalytic converters may be required by law..
Oxidants for combustion have high oxidation potential and include atmospheric or pure oxygen, chlorine, fluorine, chlorine trifluoride, nitrous oxide and nitric acid. For instance, hydrogen burns in chlorine to form hydrogen chloride with the liberation of heat and light characteristic of combustion. Although usually not catalyzed, combustion can be catalyzed by platinum or vanadium, as in the contact process.
November 12 WIKIPEDIA 2019 "COMBUSTION"