0. Hydrogen doesn't "reackt" to form Nitrogen Monoxide.
4 moles of hydrogen consume 2 moles of oxygen for complete oxidation to water.
Water is oxidized in the process of photosynthesis.
The hydrogen peroxide is both oxidized and reduced, to produce water and elemental oxygen.
Water does not ordinarily burn because of the massive amount of energy required to break the chemical bond between Hydrogen and Oxygen. If enough heat is added to break apart this bond, then the Hydrogen will burn.
5g of oxygen are required to completely react with 10g of hydrogen resulting in water with no net losses. Or exactly 2:1 = H20 (2 hydrogen < > 1 oxygen)
Can't tell, 'cause water doesn't burn. Water is totally oxidized hydrogen. It is essentially hydrogen "ash". Just as you cannot reignite the ashes from a fire you cannot re-burn water after hydrogen is burned with oxygen to water.
hydrogen, polar
Water is oxidized in the process of photosynthesis.
The hydrogen peroxide is both oxidized and reduced, to produce water and elemental oxygen.
Water does not ordinarily burn because of the massive amount of energy required to break the chemical bond between Hydrogen and Oxygen. If enough heat is added to break apart this bond, then the Hydrogen will burn.
hydrogen + oxygen is hydro oxidie now oxidized hydrogen and oxygen leave a miss content not it will blow up in ur face if u do this so instead you need to - hyrdo and oxidize it before it becomes hyrdo oxide with a miss lead of oxidized chemical
Hydrogen and oxygen are two completely different elements. When combined in a chemical reaction, two hydrogen atoms (H2) combine one oxygen atom to form a molecule of water (H2O)
Glucose is oxidized into CO2. Oxygen is reduced into Water
The process by which nutrients and oxygen are oxidized in cells is cellular respiration. It involves the oxidation of nutrients usually by oxygen.
When hydrogen burns, it is combining with oxygen. Once it has combined to form water, the molecule does not want to readily accept more oxygen atoms. Fire is rapid oxidation, so if it is already oxidized, it is done.
The hydrogen must be reduced. This takes its oxidation number from +1 to 0. However, the oxygen may be either reduced as well (from -1 to -2) or oxidised (from -1 to 0).
5g of oxygen are required to completely react with 10g of hydrogen resulting in water with no net losses. Or exactly 2:1 = H20 (2 hydrogen < > 1 oxygen)
C carbon, hydrogen and oxygen