Related Experiment Video

Updated: Feb 11, 2026

Permeabilization of Adhered Cells Using an Inert Gas Jet
08:21

Permeabilization of Adhered Cells Using an Inert Gas Jet

Published on: September 4, 2013

10.1K

Application of gas cyclone-liquid jet absorption separator for purification of tail gas containing ammonia

Liang Ma1, Zhi-Huang Zhao1, Lv Peng1

  • 1School of Mechanical and Power Engineering, East China University of Science and Technology , Shanghai , People's Republic of China.

Environmental Technology
|May 8, 2018
PubMed

Keywords:
HPOJet absorptionNHcyclone separationtail gas treatment

More Related Videos

Ammonia Synthesis at Low Pressure08:14

Ammonia Synthesis at Low Pressure

Published on: August 23, 2017

27.4K
Cryogenic Liquid Jets for High Repetition Rate Discovery Science08:34

Cryogenic Liquid Jets for High Repetition Rate Discovery Science

Published on: May 9, 2020

3.4K

Related Concept Videos

Gas Exchange and Transport01:20

Gas Exchange and Transport

Gas exchange, the intake of molecular oxygen (O2) from the environment and the outflow of carbon dioxide (CO2) into the environment, is necessary for cellular function. Gas exchange during respiration occurs largely via the movement of gas molecules along pressure gradients. Gas travels from areas of higher partial pressure to areas of lower partial pressure. In mammals, gas exchange occurs in the alveoli of the lungs, which are adjacent to capillaries and share a membrane with them.
77.1K
Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules02:34

Kinetic Molecular Theory and Gas Laws Explain Properties of Gas Molecules

The test of the kinetic molecular theory (KMT) and its postulates is its ability to explain and describe the behavior of a gas. The various gas laws (Boyle’s, Charles’s, Gay-Lussac’s, Avogadro’s, and Dalton’s laws) can be derived from the assumptions of the KMT, which have led chemists to believe that the assumptions of the theory accurately represent the properties of gas molecules.
37.5K
Applications of the Ideal Gas Law: Molar Mass, Density, and Volume03:43

Applications of the Ideal Gas Law: Molar Mass, Density, and Volume

The volume occupied by one mole of a substance is its molar volume. The ideal gas law, PV = nRT,  suggests that the volume of a given quantity of gas and the number of moles in a given volume of gas vary with changes in pressure and temperature. At standard temperature and pressure, or STP (273.15 K and 1 atm), one mole of an ideal gas (regardless of its identity) has a volume of about 22.4 L — this is referred to as the standard molar volume.
63.6K
Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion03:48

Behavior of Gas Molecules: Molecular Diffusion, Mean Free Path, and Effusion

Although gaseous molecules travel at tremendous speeds (hundreds of meters per second), they collide with other gaseous molecules and travel in many different directions before reaching the desired target. At room temperature, a gaseous molecule will experience billions of collisions per second. The mean free path is the average distance a molecule travels between collisions. The mean free path increases with decreasing pressure; in general, the mean free path for a gaseous molecule will be...
31.4K
Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law03:19

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

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.
77.6K
Ideal Gas Equation01:17

Ideal Gas Equation

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.
8.6K