“Langmuir adsorption isotherm”的概念、定义、翻译、参考文献-科学参考

Langmuir adsorption isotherm

Physics

An equation used to describe the amount of gas adsorbed on a plane surface, as a function of the pressure of the gas in equilibrium with the surface. The Langmuir adsorption isotherm can be written:

$θ = b p / (1 + b p),$

where θ‎ is the fraction of the surface covered by the adsorbate, p is the pressure of the gas, and b is a constant called the adsorption coefficient, which is the equilibrium constant for the process of adsorption. The Langmuir adsorption isotherm was derived by the US chemist Irving Langmuir (1881–1957), using the kinetic theory of gases and making the assumptions that:
1. (1) the adsorption consists entirely of a monolayer at the surface;
2. (2) there is no interaction between molecules on different sites and each site can hold only one adsorbed molecule;
3. (3) the heat of adsorption does not depend on the number of sites and is equal for all sites.
The Langmuir adsorption isotherm is of limited application since for real surfaces the energy is not the same for all sites and interactions between adsorbed molecules cannot be ignored.

Chemistry

An equation used to describe the amount of gas adsorbed on a plane surface, as a function of the pressure of the gas in equilibrium with the surface. The Langmuir adsorption isotherm can be written:
$θ = b p / (1 + b p),$
where θ‎ is the fraction of the surface covered by the adsorbate, p is the pressure of the gas, and b is a constant called the adsorption coefficient, which is the equilibrium constant for the process of adsorption. The Langmuir adsorption isotherm was derived by the US chemist Irving Langmuir (1881–1957) in 1916, using the kinetic theory of gases and making the assumptions that:
1. (1) the adsorption consists entirely of a monolayer at the surface;
2. (2) there is no interaction between molecules on different sites and each site can hold only one adsorbed molecule;
3. (3) the heat of adsorption does not depend on the number of sites and is equal for all sites.
The Langmuir adsorption isotherm is of limited application since for real surfaces the energy is not the same for all sites and interactions between adsorbed molecules cannot be ignored.

Chemical Engineering

An equation expressing the equilibrium fraction, f, of an adsorbent homogeneous surface which is covered with a single layer of adsorbed and non-interacting molecules as:
$f = \frac{a p}{1 + a p}$

where a is an empirical adsorption constant known as the Langmuir adsorption constant and p is the equilibrium partial pressure of the adsorbate in the gas phase. Adsorption isotherms are used in the design of gas–solid processes such as solid catalyzed gas phase reactions as in the synthesis of ammonia. It is named after American chemist Irving Langmuir (1881–1957).

单词	Langmuir adsorption isotherm
释义	Langmuir adsorption isotherm Physics An equation used to describe the amount of gas adsorbed on a plane surface, as a function of the pressure of the gas in equilibrium with the surface. The Langmuir adsorption isotherm can be written: $θ = b p / (1 + b p),$ where θ‎ is the fraction of the surface covered by the adsorbate, p is the pressure of the gas, and b is a constant called the adsorption coefficient, which is the equilibrium constant for the process of adsorption. The Langmuir adsorption isotherm was derived by the US chemist Irving Langmuir (1881–1957), using the kinetic theory of gases and making the assumptions that: (1) the adsorption consists entirely of a monolayer at the surface; (2) there is no interaction between molecules on different sites and each site can hold only one adsorbed molecule; (3) the heat of adsorption does not depend on the number of sites and is equal for all sites. The Langmuir adsorption isotherm is of limited application since for real surfaces the energy is not the same for all sites and interactions between adsorbed molecules cannot be ignored. Chemistry An equation used to describe the amount of gas adsorbed on a plane surface, as a function of the pressure of the gas in equilibrium with the surface. The Langmuir adsorption isotherm can be written: $θ = b p / (1 + b p),$ where θ‎ is the fraction of the surface covered by the adsorbate, p is the pressure of the gas, and b is a constant called the adsorption coefficient, which is the equilibrium constant for the process of adsorption. The Langmuir adsorption isotherm was derived by the US chemist Irving Langmuir (1881–1957) in 1916, using the kinetic theory of gases and making the assumptions that: (1) the adsorption consists entirely of a monolayer at the surface; (2) there is no interaction between molecules on different sites and each site can hold only one adsorbed molecule; (3) the heat of adsorption does not depend on the number of sites and is equal for all sites. The Langmuir adsorption isotherm is of limited application since for real surfaces the energy is not the same for all sites and interactions between adsorbed molecules cannot be ignored. Chemical Engineering An equation expressing the equilibrium fraction, f, of an adsorbent homogeneous surface which is covered with a single layer of adsorbed and non-interacting molecules as: $f = \frac{a p}{1 + a p}$ where a is an empirical adsorption constant known as the Langmuir adsorption constant and p is the equilibrium partial pressure of the adsorbate in the gas phase. Adsorption isotherms are used in the design of gas–solid processes such as solid catalyzed gas phase reactions as in the synthesis of ammonia. It is named after American chemist Irving Langmuir (1881–1957).
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