“fuel cell”的概念、定义、翻译、参考文献-科学参考

fuel cell

Physics

A cell in which the chemical energy of a fuel is converted directly into electrical energy. The simplest fuel cell is one in which hydrogen is oxidized to form water over porous sintered nickel electrodes. A supply of gaseous hydrogen is fed to a compartment containing the porous cathode and a supply of oxygen is fed to a compartment containing the porous anode; the electrodes are separated by a third compartment containing a hot alkaline electrolyte, such as potassium hydroxide. The electrodes are porous to enable the gases to react with the electrolyte, with the nickel in the electrodes acting as a catalyst. At the cathode the hydrogen reacts with the hydroxide ions in the electrolyte to form water, with the release of two electrons per hydrogen molecule:

$H_{2} + 2 {OH}^{-} \to 2 H_{2} O + 2 e^{-}$

At the anode, the oxygen reacts with the water, taking up electrons, to form hydroxide ions:

$½ O_{2} + H_{2} {O + 2 e}^{-} \to 2 {OH}^{-}$

The electrons flow from the cathode to the anode through an external circuit as an electric current. The device is a more efficient converter of electric energy than a heat engine, but it is bulky and requires a continuous supply of gaseous fuels. Their use to power electric vehicles is being actively explored.

The second generation of fuel cells uses molten salts, especially carbonates of metals such as lithium and potassium, as electrolytes. The third generation of fuel cells uses conducting solid ionic oxides as electrolytes.

Space Exploration

A cell converting chemical energy directly to electrical energy. It works on the same principle as a battery but is continually fed with fuel, usually hydrogen. Fuel cells are used on spacecraft because batteries are too heavy. Crews can also drink the water that is produced as a by-product. Fuel cells on a space shuttle can produce 12 kW of power, six times as much as those flown during the Apollo project.
Hydrogen is passed over an electrode (usually nickel or platinum) containing a catalyst, which splits the hydrogen into electrons and protons. The electrons pass through an external circuit while the protons pass through a polymer electrolyte membrane to another electrode, over which oxygen is passed. Water is formed at this electrode (as a by-product) in a chemical reaction involving electrons, protons, and oxygen atoms. A current is generated between the electrodes.

Chemistry

A cell in which the chemical energy of a fuel is converted directly into electrical energy. The simplest fuel cell is one in which hydrogen is oxidized to form water over porous sintered nickel electrodes. A supply of gaseous hydrogen is fed to a compartment containing the porous anode and a supply of oxygen is fed to a compartment containing the porous cathode; the electrodes are separated by a third compartment containing a hot alkaline electrolyte, such as potassium hydroxide. The electrodes are porous to enable the gases to react with the electrolyte, with the nickel in the electrodes acting as a catalyst. At the anode the hydrogen reacts with the hydroxide ions in the electrolyte to form water, with the release of two electrons per hydrogen molecule:
$H_{2} + 2 {OH}^{-} \to 2 H_{2} O + 2 e^{-}$
At the cathode, the oxygen reacts with the water, taking up electrons, to form hydroxide ions:
$½ O_{2} + H_{2} O + 2 e^{-} \to 2 {OH}^{-}$
The electrons flow from the anode to the cathode through an external circuit as an electric current. The device is a more efficient converter of electric energy than a heat engine, but it is bulky and requires a continuous supply of gaseous fuels. Their use to power electric vehicles is being actively explored.

Chemical Engineering

An electrochemical device in which the energy of a chemical reaction is converted directly into a low-voltage, direct current electrical energy. The simplest fuel cell involves the oxidation of hydrogen to form water. Hydrogen gas is used as the fuel and fed to the porous anode, and oxygen is fed to the porous cathode. The two electrodes are separated by a hot alkaline electrolyte such as potassium hydroxide. The electrodes are porous to allow the two gases to react with the electrolyte. At the anode the hydrogen reacts with the hydroxide ions in the electrolyte to form water and the release of two electrons per hydrogen molecule. At the cathode, the oxygen reacts with the water to take up the electrons and form hydroxide ions. The flow of electrons from the anode to the cathode is via an external circuit as an electrical current:
$Anode : H_{2} + O H^{-} \to 2 H_{2} O + 2 e^{-}$
$Cathode : 1 / 2 O_{2} + H_{2} O + 2 e^{-} \to 2 O H^{-}$

The overall fuel cell reaction of $H_{2} + \frac{1}{2} O_{2} \to H_{2} O$ is, in effect, the spontaneous coldcombustion of hydrogen. However, unlike the combustion process, hydrogen and oxygen must be kept separate. Little heat is liberated in the fuel cell and instead the free energy is released directly as electrical energy. Fuel cells are therefore more efficient than combustion processes. However, fuel cells are more bulky than heat engines and require a continuous supply of gaseous fuels.

Electronics and Electrical Engineering

A chemical cell that combines fuel in the form of hydrogen with oxygen to produce electricity, with water and heat as by-products. Such cells are fed a continuous stream of fuel rather than having an internal chemical store. They can be compact and light, so are particularly suited for use in remote locations.

单词	fuel cell
释义	fuel cell Physics A cell in which the chemical energy of a fuel is converted directly into electrical energy. The simplest fuel cell is one in which hydrogen is oxidized to form water over porous sintered nickel electrodes. A supply of gaseous hydrogen is fed to a compartment containing the porous cathode and a supply of oxygen is fed to a compartment containing the porous anode; the electrodes are separated by a third compartment containing a hot alkaline electrolyte, such as potassium hydroxide. The electrodes are porous to enable the gases to react with the electrolyte, with the nickel in the electrodes acting as a catalyst. At the cathode the hydrogen reacts with the hydroxide ions in the electrolyte to form water, with the release of two electrons per hydrogen molecule: $H_{2} + 2 {OH}^{-} \to 2 H_{2} O + 2 e^{-}$ At the anode, the oxygen reacts with the water, taking up electrons, to form hydroxide ions: $½ O_{2} + H_{2} {O + 2 e}^{-} \to 2 {OH}^{-}$ The electrons flow from the cathode to the anode through an external circuit as an electric current. The device is a more efficient converter of electric energy than a heat engine, but it is bulky and requires a continuous supply of gaseous fuels. Their use to power electric vehicles is being actively explored. The second generation of fuel cells uses molten salts, especially carbonates of metals such as lithium and potassium, as electrolytes. The third generation of fuel cells uses conducting solid ionic oxides as electrolytes. Space Exploration A cell converting chemical energy directly to electrical energy. It works on the same principle as a battery but is continually fed with fuel, usually hydrogen. Fuel cells are used on spacecraft because batteries are too heavy. Crews can also drink the water that is produced as a by-product. Fuel cells on a space shuttle can produce 12 kW of power, six times as much as those flown during the Apollo project. Hydrogen is passed over an electrode (usually nickel or platinum) containing a catalyst, which splits the hydrogen into electrons and protons. The electrons pass through an external circuit while the protons pass through a polymer electrolyte membrane to another electrode, over which oxygen is passed. Water is formed at this electrode (as a by-product) in a chemical reaction involving electrons, protons, and oxygen atoms. A current is generated between the electrodes. Chemistry A cell in which the chemical energy of a fuel is converted directly into electrical energy. The simplest fuel cell is one in which hydrogen is oxidized to form water over porous sintered nickel electrodes. A supply of gaseous hydrogen is fed to a compartment containing the porous anode and a supply of oxygen is fed to a compartment containing the porous cathode; the electrodes are separated by a third compartment containing a hot alkaline electrolyte, such as potassium hydroxide. The electrodes are porous to enable the gases to react with the electrolyte, with the nickel in the electrodes acting as a catalyst. At the anode the hydrogen reacts with the hydroxide ions in the electrolyte to form water, with the release of two electrons per hydrogen molecule: $H_{2} + 2 {OH}^{-} \to 2 H_{2} O + 2 e^{-}$ At the cathode, the oxygen reacts with the water, taking up electrons, to form hydroxide ions: $½ O_{2} + H_{2} O + 2 e^{-} \to 2 {OH}^{-}$ The electrons flow from the anode to the cathode through an external circuit as an electric current. The device is a more efficient converter of electric energy than a heat engine, but it is bulky and requires a continuous supply of gaseous fuels. Their use to power electric vehicles is being actively explored. Chemical Engineering An electrochemical device in which the energy of a chemical reaction is converted directly into a low-voltage, direct current electrical energy. The simplest fuel cell involves the oxidation of hydrogen to form water. Hydrogen gas is used as the fuel and fed to the porous anode, and oxygen is fed to the porous cathode. The two electrodes are separated by a hot alkaline electrolyte such as potassium hydroxide. The electrodes are porous to allow the two gases to react with the electrolyte. At the anode the hydrogen reacts with the hydroxide ions in the electrolyte to form water and the release of two electrons per hydrogen molecule. At the cathode, the oxygen reacts with the water to take up the electrons and form hydroxide ions. The flow of electrons from the anode to the cathode is via an external circuit as an electrical current: $Anode : H_{2} + O H^{-} \to 2 H_{2} O + 2 e^{-}$ $Cathode : 1 / 2 O_{2} + H_{2} O + 2 e^{-} \to 2 O H^{-}$ The overall fuel cell reaction of $H_{2} + \frac{1}{2} O_{2} \to H_{2} O$ is, in effect, the spontaneous coldcombustion of hydrogen. However, unlike the combustion process, hydrogen and oxygen must be kept separate. Little heat is liberated in the fuel cell and instead the free energy is released directly as electrical energy. Fuel cells are therefore more efficient than combustion processes. However, fuel cells are more bulky than heat engines and require a continuous supply of gaseous fuels. Electronics and Electrical Engineering A chemical cell that combines fuel in the form of hydrogen with oxygen to produce electricity, with water and heat as by-products. Such cells are fed a continuous stream of fuel rather than having an internal chemical store. They can be compact and light, so are particularly suited for use in remote locations.
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