1. Methane and Hydrogen

2. Methane Methane is a significant and plentiful fuel which is the principal component of natural gas. Burning one molecule of methane in the presence of oxygen releases one molecule of CO2 (carbon dioxide) and two molecules of H2O:fuelnatural gasoxygencarbon dioxideH2O –CH4 + 2O2 → CO2 + 2H2O Methane's relative abundance and clean burning process makes it a very attractive fuel. However, because it is a gas (at normal temperature and pressure) and not a liquid or solid, methane is difficult to transport from the areas that produce it to the areas that consume it. Converting methane to derivatives that are more easily transported, such as methanol, is an active area of research. Certain microorganisms can effect this selective oxidation using enzymes called methane monooxygenases. methanolmethane monooxygenases

4. Sources of methane Natural gas fields::: **The major source of methane is extraction from geological deposits known as natural gas fields. It is associated with other hydrocarbon fuels and sometimes accompanied by helium and nitrogen. The gas at shallow levels (low pressure) is formed by anaerobic decay of organic matter and reworked methane from deep under the Earth's surface. In general, sediments buried deeper and at higher temperatures than those which give oil generate natural gas.natural gas fieldshydrocarbonheliumnitrogenanaerobicdecayorganic matteroil

7. Hydrogen Hydrogen (IPA: / ˈ ha ɪ drə( ʊ )d ʒ ən/), is a chemical element that has the symbol H and an atomic number of 1. At standard temperature and pressure it is a colorless, odorless, nonmetallic, tasteless, highly flammable diatomic gas (H2). With an atomic mass of 1.00794 g/mol, hydrogen is the lightest element.IPAchemical elementatomic numberstandard temperature and pressurenonmetallicflammablediatomicgasatomic mass1.00794mol

8. +-+-+-+-+-+-+-+-+-+- Hydrogen is the most abundant of the chemical elements, constituting roughly 75% of the universe's elemental mass.[1] Stars in the main sequence are mainly composed of hydrogen in its plasma state. Elemental hydrogen is relatively rare on Earth, and is industrially produced from hydrocarbons such as methane, after which most elemental hydrogen is used "captively" (meaning locally at the production site), with the largest markets about equally divided between fossil fuel upgrading (e.g., hydrocracking) and in ammonia production (mostly for the fertilizer market). Hydrogen may be produced from water using the process of electrolysis, but this process is presently significantly more expensive commercially than hydrogen production from natural gas.abundant[1]Starsmain sequenceplasmaEarthhydrocarbonshydrocrackingammonia electrolysis

9. +-+-+-+-+-+-+-+-+-+-+- The most common naturally occurring isotope of hydrogen is known as protium, has a single proton and no neutrons. In ionic compounds it can take on either a positive charge (becoming a cation composed of a bare proton) or a negative charge (becoming an anion known as a hydride). Hydrogen can form compounds with most elements and is present in water and most organic compounds. It plays a particularly important role in acid- base chemistry, in which many reactions involve the exchange of protons between soluble molecules. As the only neutral atom for which the Schrödinger equation can be solved analytically, study of the energetics and bonding of the hydrogen atom has played a key role in the development of quantum mechanics.isotopeprotonneutronsioniccationanionhydridewaterorganic compoundsacid- base chemistrySchrödinger equationquantum mechanics

11. Hydrogen can combust rapidly in air. It burned rapidly in the Hindenburg disaster on May 6, 1937HindenburgMay 6 1937

12. HYDROGEN

13. It is prepared by Raziye ALTINSOY AKSARAY HİGH SCHOOL