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Hydrogen Gas Flammability Reasons
On the cause of hydrogen flammability
Hydrogen is a flammable gas. The cause of its flammability is covered by the following numbers.
First, the molecular structure of hydrogen is simple, only two hydrogen atoms are connected by covalent bonds to form a state of\ (H_ {2}\). This simple structure causes its chemical bond energy to be relatively low. When external energy is involved, such as an open flame, hot topic, etc., the covalent bond is easily broken, and the hydrogen atom is energized and active, thereby promoting the combustion reaction.
Second, the combustion reaction of hydrogen is a strong exothermic reaction. Hydrogen and oxygen meet and burn, generating water and releasing a large amount of heat energy. The chemical reaction equation is\ (2H_ {2} + O_ {2}\ stackrel {ignited }{=\!=\!=} 2H_ {2} O\). This large amount of heat energy not only maintains the reaction, but also promotes the energy of surrounding hydrogen molecules, accelerates the reaction rate, and causes the combustion to spread rapidly.
Third, hydrogen has strong diffusivity. Hydrogen has a much lower density than air and is easily diffused in the air. Once leaked, it can quickly mix with air to form a combustible mixture, expanding the combustion range and increasing the risk of fire.
Fourth, the ignition energy requirement of hydrogen is low. A very small amount of energy input can cause a hydrogen-air mixture to catch fire and burn. This property makes it easy to ignite in many seemingly ordinary environments, causing danger.
In summary, due to factors such as the molecular structure of hydrogen, the thermal effect of combustion, diffusivity, and ignition energy requirements, its flammable properties are jointly created. When using and storing hydrogen, it is necessary to take precautions to avoid the risk of fire and explosion.
Hydrogen is a flammable gas. The cause of its flammability is covered by the following numbers.
First, the molecular structure of hydrogen is simple, only two hydrogen atoms are connected by covalent bonds to form a state of\ (H_ {2}\). This simple structure causes its chemical bond energy to be relatively low. When external energy is involved, such as an open flame, hot topic, etc., the covalent bond is easily broken, and the hydrogen atom is energized and active, thereby promoting the combustion reaction.
Second, the combustion reaction of hydrogen is a strong exothermic reaction. Hydrogen and oxygen meet and burn, generating water and releasing a large amount of heat energy. The chemical reaction equation is\ (2H_ {2} + O_ {2}\ stackrel {ignited }{=\!=\!=} 2H_ {2} O\). This large amount of heat energy not only maintains the reaction, but also promotes the energy of surrounding hydrogen molecules, accelerates the reaction rate, and causes the combustion to spread rapidly.
Third, hydrogen has strong diffusivity. Hydrogen has a much lower density than air and is easily diffused in the air. Once leaked, it can quickly mix with air to form a combustible mixture, expanding the combustion range and increasing the risk of fire.
Fourth, the ignition energy requirement of hydrogen is low. A very small amount of energy input can cause a hydrogen-air mixture to catch fire and burn. This property makes it easy to ignite in many seemingly ordinary environments, causing danger.
In summary, due to factors such as the molecular structure of hydrogen, the thermal effect of combustion, diffusivity, and ignition energy requirements, its flammable properties are jointly created. When using and storing hydrogen, it is necessary to take precautions to avoid the risk of fire and explosion.
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