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Hydrogen is a chemical element; it has symbol H and atomic number 1. It is the lightest element and, at standard conditions, is a gas of diatomic molecules with the formula H 2, sometimes called dihydrogen, [11] hydrogen gas, molecular hydrogen, or simply hydrogen. It is colorless, odorless, [12] non-toxic, and highly combustible.
Hydrogen gas is produced by several industrial methods. [1] Nearly all of the world's current supply of hydrogen is created from fossil fuels. [2] [3] Most hydrogen is gray hydrogen made through steam methane reforming. In this process, hydrogen is produced from a chemical reaction between steam and methane, the main component of natural gas.
The hydrogen cycle consists of hydrogen exchanges between biotic (living) and abiotic (non-living) sources and sinks of hydrogen-containing compounds. Hydrogen (H) is the most abundant element in the universe. [1] On Earth, common H-containing inorganic molecules include water (H 2 O), hydrogen gas (H 2), hydrogen sulfide (H 2 S), and ammonia ...
Natural hydrogen is generated from various sources. Many hydrogen emergences have been identified on mid-ocean ridges. [22] Serpentinisation occurs frequently in the oceanic crust; many targets for exploration include portions of oceanic crust which have been obducted and incorporated into continental crust.
In acidic conditions, the hydrogen evolution reaction follows the formula: [6] 2 H + + 2 e − → H 2. In neutral or alkaline conditions, the reaction follows the formula: [6] 4 H 2 O + 4 e − → 2 H 2 + 4 HO −. Both of these mechanisms can be seen in industrial practices at the cathode side of the electrolyzer where hydrogen evolution occurs.
The natural abundance of hydrogen (H 2) in the Earth's atmosphere is only of the order of parts per million, but H 2 is the most abundant diatomic molecule in the universe. The interstellar medium is dominated by hydrogen atoms.
Good morning. Is hydrogen the answer to the world’s energy problems? Our guest on Leadership Next this week answers that with a definite yes.
The addition of hydrogen to double or triple bonds in hydrocarbons is a type of redox reaction that can be thermodynamically favorable. For example, the addition of hydrogen to ethene has a Gibbs free energy change of -101 kJ·mol −1, which is highly exothermic. [11]