Nitrogen gas can be converted into liquid nitrogen by

Nitrogen exists in the atmosphere as N 2 \text N_2 N 2 ​ start text, N, end text, start subscript, 2, end subscript gas. In nitrogen fixation, bacteria convert N 2 \text N_2 N 2 ​ start text, N, end text, start subscript, 2, end subscript into ammonia, a form of nitrogen usable by plants. When animals eat the plants, they acquire usable nitrogen compounds. • Nitrogen is everywhere! In fact, N 2 \text N_2 N 2 ​ start text, N, end text, start subscript, 2, end subscript gas makes up about 78% of Earth's atmosphere by volume, far surpassing the O 2 \text O_2 O 2 ​ start text, O, end text, start subscript, 2, end subscript we often think of as "air". 1 ^1 1 start superscript, 1, end superscript But having nitrogen around and being able to make use of it are two different things. Your body, and the bodies of other plants and animals, have no good way to convert N 2 \text N_2 N 2 ​ start text, N, end text, start subscript, 2, end subscript into a usable form. We animals—and our plant compatriots—just don't have the right enzymes to capture, or fix, atmospheric nitrogen. Nitrogen enters the living world by way of bacteria and other single-celled prokaryotes, which convert atmospheric nitrogen— N 2 \text N_2 N 2 ​ start text, N, end text, start subscript, 2, end subscript —into biologically usable forms in a process called nitrogen fixation. Some species of nitrogen-fixing bacteria are free-living in soil or water, while others are beneficial symbionts that live inside of plants. ...

You shouldn't make liquid nitrogen bombs. They can be very dangerous. There, I said it. Well, what is a liquid nitrogen bomb anyway? In short, you pour some liquid nitrogen into a soda bottle or something similar. Next, put the cap on the bottle. Next, there is no next. That is it. Boom! It blows up. Essentially the liquid boils and adds nitrogen gas to the enclosed bottle. Of course, the more gas you add, the greater the pressure. Eventually the pressure gets high enough that the bottle explodes. Here is an example from So, I see something like this and it gets me thinking. Clearly there is some energy here. The water overall increases its center of mass. This means that there had to be an increase in gravitational potential energy of water-Earth system. If this explosion was caused by a stick of dynamite, it would be clear. The dynamite would decrease in stored chemical potential energy and the water would probably increase in thermal energy, kinetic energy and gravitational potential energy. All would be clear. Energy would be conserved. But with liquid nitrogen, it explodes because it essentially "warms up." So, the bomb itself increases in thermal energy. Crazy if you think about it. So, how does this work? Well, let's assume the liquid nitrogen start's at its boiling point (-196°C). In order to make the transition from a liquid to a gas, it needs energy. The amount of energy depends on the amount of material that makes the transition as well as the type of material. ...

This may not be as spectacular as you migh imagine. If one litre of liquid nitrogen turned to gas, then it would simply be no longer the liquid form of nitrogen, but the gas form of it. This starts to happen immediately: its te smoke like stuff coming of the liquid nitrogen. Nitrogen in its gas form is a normal part of our atmosphere, we need it to breathe, so one litre of LIQUID nitrogen turning to GAS nitrogen will not do anything cool., You need to put something in the liquid nitrogen, and as nitrogen can only be liquid at a very low temperature, what ever you put in it, will freeze and if you hit it it will break. Dont get any on you: it wil freeze your flesh off

Gases, Liquefaction of Liquefaction of gases is the process by which substances in their gaseous state are converted to the liquid state. When pressure on a gas is increased, its molecules closer together, and its temperature is reduced, which removes enough energy to make it change from the gaseous to the liquid state. Two important properties of gases are important in developing methods for their liquefaction: critical temperature and critical pressure. The critical temperature of a gas is the temperature at or above which no amount of pressure, however great, will cause the gas to liquefy. The minimum pressure required to liquefy the gas at the critical temperature is called the critical pressure. For example, the critical temperature for °F [31 °C]). That means that no amount of pressure applied to a sample of °F [31 °C]) will cause the gas to liquefy. At or below that temperature, however, the gas can be liquefied provided sufficient pressure is applied. The corresponding critical pressure for carbon dioxide at 304K (87.8 °F [31 °C]) is 72.9 atmospheres. In other words, the application of a pressure of 72.9 atmospheres of pressure on a sample of carbon dioxide gas at 304K (87.8 °F [31 °C]) will cause the gas to liquefy. Differences in critical temperatures among gases means that some gases are easier to liquefy than others. The critical temperature of carbon dioxide is high enough so that it can be liquefied relatively easily at or near room temperature. By comparison...

Liquid Nitrogen Liquid nitrogen is inert, colorless, odorless, non corrosive, nonflammable, and extremely cold. Nitrogen makes up the major portion of the atmosphere (78% by volume). Nitrogen is inert and will not support combustion; however, it is not life supporting. When nitrogen is converted to liquid form it becomes a cryogenic liquid. Cryogenic liquids are liquefied gases that have a normal boiling point below -150 °C (-238 °F). Liquid nitrogen has a boiling point of -195.8 °C (-320.5 °F). All cryogenic liquids produce large amounts of gas when they vaporize. Health Effects Extensive tissue damage or burns can result from exposure to liquid nitrogen or cold nitrogen vapors. Being odorless, colorless, tasteless, and nonirritating, nitrogen has no warning properties. Humans possess no senses that can detect the presence of nitrogen. Although nitrogen is nontoxic and inert, it can act as a simple asphyxiant by displacing oxygen in air to levels below that required to support life. Inhalation of nitrogen in excessive amounts can cause dizziness, nausea, vomiting, loss of consciousness, and death. Death may result from errors in judgment, confusion, or loss of consciousness that prevents self-rescue. At low oxygen concentration, unconsciousness and death may occur in seconds and without warning. Personnel, including rescue workers, should not enter areas where the oxygen concentration is below 19.5%, unless provided with a self-contained breathing apparatus or air-line re...

Glossary Group A vertical column in the periodic table. Members of a group typically have similar properties and electron configurations in their outer shell. Period A horizontal row in the periodic table. The atomic number of each element increases by one, reading from left to right. Block Elements are organised into blocks by the orbital type in which the outer electrons are found. These blocks are named for the characteristic spectra they produce: sharp (s), principal (p), diffuse (d), and fundamental (f). Atomic number The number of protons in an atom. Electron configuration The arrangements of electrons above the last (closed shell) noble gas. Melting point The temperature at which the solid–liquid phase change occurs. Boiling point The temperature at which the liquid–gas phase change occurs. Sublimation The transition of a substance directly from the solid to the gas phase without passing through a liquid phase. Density (g cm −3) Density is the mass of a substance that would fill 1 cm 3 at room temperature. Relative atomic mass The mass of an atom relative to that of carbon-12. This is approximately the sum of the number of protons and neutrons in the nucleus. Where more than one isotope exists, the value given is the abundance weighted average. Isotopes Atoms of the same element with different numbers of neutrons. CAS number The Chemical Abstracts Service registry number is a unique identifier of a particular chemical, designed to prevent confusion arising from diff...

Xuanyu Han / Getty Images There are two main ways nitrogen can become " • Fixation by lightning: The energy from lightning causes nitrogen (N 2) and water (H 2O) to combine to form ammonia (NH 3) and nitrates (NO 3). Precipitation carries the ammonia and nitrates to the ground, where they can be assimilated by plants. • Biological fixation: About 90% of nitrogen fixation is done by bacteria. Cyanobacteria convert nitrogen into ammonia and ammonium: N 2+ 3 H 2 → 2 NH 3. Ammonia can then be used by plants directly. Ammonia and ammonium may be further reacted in the nitrification process. Tony C French / Getty Images Nitrification occurs by the following reactions: 2 NH3 + 3 O2 → 2 NO2 + 2 H++ 2 H2O 2 NO2- + O2 → 2 NO3- Aerobic bacteria use oxygen to convert ammonia and ammonium. Nitrosomonas bacteria convert nitrogen into nitrite (NO2-), and then Nitrobacter converts nitrite to nitrate (NO3-). Some bacteria exist in a symbiotic relationship with plants (legumes and some root-nodule species), and plants utilize the nitrate as a nutrient. Meanwhile, animals obtain nitrogen by eating plants or plant-eating animals. Simon McGill / Getty Images When plants and animals die, bacteria convert nitrogen nutrients back into ammonium salts and ammonia. This conversion process is called ammonification. Anaerobic bacteria can convert ammonia into nitrogen gas through the process of denitrification: NO3- + CH2O + H+ → ½ N2O + CO2 + 1½ H2O Denitrification returns nitrogen to the atmosphere,...

Nitrogen is one of the primary nutrients critical for the survival of all living organisms. Although nitrogen is very abundant in the atmosphere, it is largely inaccessible in this form to most organisms. This article explores how nitrogen becomes available to organisms and what changes in nitrogen levels as a result of human activity means to local and global ecosystems. Nitrogen is one of the primary nutrients critical for the survival of all living organisms. It is a necessary component of many biomolecules, including proteins, DNA, and chlorophyll. Although nitrogen is very abundant in the atmosphere as dinitrogen gas (N 2), it is largely inaccessible in this form to most organisms, making nitrogen a scarce resource and often limiting primary productivity in many ecosystems. Only when nitrogen is converted from dinitrogen gas into ammonia (NH 3) does it become available to primary producers, such as plants. In addition to N 2 and NH 3, nitrogen exists in many different forms, including both inorganic (e.g., ammonia, nitrate) and organic (e.g., amino and nucleic acids) forms. Thus, nitrogen undergoes many different transformations in the ecosystem, changing from one form to another as organisms use it for growth and, in some cases, energy. The major transformations of nitrogen are nitrogen fixation, nitrification, denitrification, anammox, and ammonification (Figure 1). The transformation of nitrogen into its many oxidation states is key to productivity in the biosphere...