Related Experiment Video
Updated: May 7, 2026
07:17
Non-equilibrium Microwave Plasma for Efficient High Temperature Chemistry
Published on: August 1, 2017
14.8K
Probability theory for 3-layer remote sensing in ideal gas law environment
Optics Express
|October 10, 2013
Summary
This study extends radiative transfer models to ideal gas conditions. The correlation between transmission and temperature in 3 layers has a minimal impact on at-sensor radiance probability density functions.
Area of Science:
- Atmospheric science
- Radiative transfer modeling
- Remote sensing
Background:
- Existing probability models for radiative transfer are extended.
- Ideal gas conditions introduce correlations between transmission and temperature in atmospheric layers.
Purpose of the Study:
- To investigate the impact of transmission-temperature correlations on radiative transfer models.
- To determine if the complexity of accounting for these correlations is necessary.
Main Methods:
- Extending a 3-layer radiative transfer probability model.
- Analyzing the effect of transmission-temperature correlations on the probability density function of at-sensor radiances.
Main Results:
- The correlation between transmission and temperature has a surprisingly small effect on the probability density function for at-sensor radiances.
- Perturbations on variance population parameters are small.
- Cancellation of perturbation terms in model moment expressions minimizes the overall effect.
Conclusions:
- The added complexity of addressing transmission-temperature correlations in ideal gas conditions can be avoided.
- The current radiative transfer model is robust to these correlations.
- Simplified modeling approaches are validated for specific atmospheric conditions.
Related Concept Videos
04:01Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation
30.8K
Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and molecular formula problems to determining the density and molar mass of a gas. However, the behavior of a gas is often non-ideal, meaning that the observed relationships between its pressure, volume, and temperature are not accurately described by the gas laws.
30.8K
01:17Ideal Gas Equation
6.5K
The ideal gas equation is an equation of state that relates the state variables pressure, volume, temperature, and the number of moles of a hypothetical gas. This equation is a combination of four empirical laws, namely Boyle’s Law, Charles’s Law, Avogadro’s Law, and Gay-Lussac’s Law. When the proportionalities of the above four empirical laws are combined, it results in a single proportionality constant known as the universal gas constant.
6.5K
03:19Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law
61.2K
Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and volume, volume and temperature, and volume and moles, that hold for an ideal gas.
61.2K
01:25Adsorption Isotherms II
146
Brunauer, Emmett, and Teller (BET) introduced a theory in 1938 that modified Langmuir's assumptions to explain multilayer physical adsorption. This theory is applicable to Type II isotherms and provides a more realistic picture of adsorption processes. The BET theory assumes a uniform solid surface with localized adsorption sites, where adsorption at one site doesn't affect adsorption at neighboring sites. This theory also allows for the possibility of additional molecules being adsorbed on top...
146
01:23Deviation from Ideal Behaviour
174
Real gases do not perfectly obey the ideal gas laws, especially at high pressures and low temperatures or when they are about to condense to a liquid. These deviations occur due to intermolecular forces between gas molecules. Repulsive forces aid expansion and are significant when molecules are very close together, typically at high pressure. Attractive forces assist compression and have a longer range, being effective over several molecular diameters. They become significant when molecules are...
174
01:24The Kinetic Model of Gases
160
The kinetic model of gases explains the properties of a perfect gas using three main assumptions: molecules move in ceaseless random motion, their size is negligible compared to the distances between them, and they do not interact except during perfectly elastic collisions. The total energy of a gas is the sum of the kinetic energies of all its constituent molecules. The pressure exerted by the gas arises from the continual bombardment of the container walls by billions of colliding molecules.
160