Application of nitrogen presentation. Application of nitric acid
Slide 2
A liquid nitrogen
Liquid nitrogen is non-explosive and non-toxic. Liquid of transparent color. It has a boiling point of −195.75 °C.
By evaporating, nitrogen cools the fire and displaces the oxygen necessary for combustion, so the fire stops. Since nitrogen, unlike water, foam or powder, simply evaporates and disappears, nitrogen fire extinguishing, along with carbon dioxide, is the most effective method of extinguishing fires from the point of view of preserving valuables.
Slide 3
Application of liquid nitrogen
- for cooling various equipment and machinery;
- for cooling computer components during extreme overclocking
Slide 4
- Liquid nitrogen is used in cosmetology. for the treatment of vulgar, plantar and flat warts, papillomas, hypertrophic scars, vulgar acne, rosacea.
- In the food industry, nitrogen is registered as a food additive E941, as a gaseous medium for packaging and storage, a refrigerant, and liquid nitrogen is used when bottling oils and non-carbonated drinks to create excess pressure and an inert environment in soft containers.
Slide 5
Behavior of substances in liquid nitrogen
Substances in liquid nitrogen become brittle
Slide 6
Liquid nitrogen burns
You should cool the affected areas of the body with water or cold objects, administer painkillers, and apply bandages made from sterile dressings or improvised materials to the wounds.
Slide 7
Caisson disease
Caisson sickness occurs when there is a rapid decrease in pressure (for example, when ascending from depth, leaving a caisson or pressure chamber, or ascending to a height). In this case, nitrogen gas, previously dissolved in the blood or tissues, forms gas bubbles in the blood vessels. Characteristic symptoms include pain or neurological impairment. Severe cases can be fatal.
Slide 8
Chemical properties of nitrogen
- 6Li + N2 = 2Li3N
- N2 + 3H2 = 2NH3
- N2 + O2 = 2NO
Slide 9
Chemically, nitrogen is a fairly inert gas due to its strong covalent bond, while atomic nitrogen is chemically very active. Of the metals, free nitrogen reacts under normal conditions only with lithium, forming nitride:
- 6Li + N2 = 2Li3N
As temperature increases, the activity of molecular nitrogen increases. When nitrogen reacts with hydrogen under heating, elevated pressure and the presence of a catalyst, ammonia is formed:
- N2 + 3H2 = 2NH3
Nitrogen combines with oxygen only in an electric arc to form nitrogen oxide (II):
- N2 + O2 = 2NO
Slide 10
Nitric acid
The boiling point of nitric acid is +83 °C, the freezing point is –41 °C, i.e. under normal conditions it is a liquid. The pungent odor and the fact that it turns yellow during storage is explained by the fact that the concentrated acid is unstable and partially decomposes when exposed to light or heating.
4HNO3 = 2H2O + 4NO2 + O2.
Slide 11
Interaction with metals
Concentrated nitric acid
- Me+ HNO3(conc.) → salt + water + NO2
Noble metals (Au, Ru, Os, Rh, Ir, Pt) do not interact with concentrated nitric acid, and a number of metals (Al, Ti, Cr, Fe, Co, Ni) are passivated at low temperatures with concentrated nitric acid. The reaction is possible with increasing temperature
- Ag + 2HNO3(conc.) → AgNO3 + H2O + NO2.
Slide 12
Dilute nitric acid
The reduction product of nitric acid in a dilute solution depends on the activity of the metal involved in the reaction:
Active metal
- 8Al + 30HNO3(dil.) → 8Al(NO3)3 + 9H2O + 3NH4NO3
Medium activity metal
- 10Cr + 36HNO3(dil.) → 10Cr(NO3)3 + 18H2O + 3N2
Low-active metal
- 3Ag + 4HNO3(dil.) → 3AgNO3 + 2H2O + NO
Slide 13
Preparation of nitric acid
- NaNO3 + H2SO4 = NaHSO4 + HNO3
- 4NH3 + 5O2 → 4NO + 6H2O (Conditions: catalyst – Pt, t = 500˚С)
- 2NO + O2 → 2NO2
- 4NO2 + O2 + 2H2O ↔ 4HNO3
Slide 14
Application of nitric acid
- Production of nitrogen and complex fertilizers.
- Production of explosives.
- Production of dyes.
- Medicine production.
- Production of films, nitro varnishes, nitro enamels.
- Production of artificial fibers.
- As a component of a nitrating mixture for trawling metals in metallurgy.
Slide 15
Ammonia
Ammonia - NH3, hydrogen nitride, under normal conditions - a colorless gas with a sharp characteristic odor (the smell of ammonia).
Ammonia is almost twice as light as air. The solubility of NH3 in water is extremely high - about 1200 volumes (at 0 °C) or 700 volumes (at 20 °C) in volume.
Ammonia (in European languages its name sounds like “ammoniac”) owes its name to the Ammon oasis in North Africa, located at the crossroads of caravan routes. In hot climates, urea (NH2)2CO, contained in animal waste products, decomposes especially quickly. One of the decomposition products is ammonia. According to other sources, ammonia got its name from the ancient Egyptian word amonian. This was the name given to people who worshiped the god Amon. During their rituals, they sniffed ammonia NH4Cl, which, when heated, evaporates ammonia.
Slide 16
Ammonia is dangerous
In medicine, a 10% aqueous solution of ammonia is known as ammonia. The pungent odor of ammonia irritates specific receptors of the nasal mucosa and promotes excitation of the respiratory and vasomotor centers, therefore, in case of fainting or alcohol poisoning, the victim is allowed to inhale vapors of ammonia
Ammonia is dangerous if inhaled. In acute poisoning, ammonia affects the eyes and respiratory tract, and at high concentrations it can be fatal. Causes severe coughing, suffocation, and with a high concentration of vapors - agitation, delirium. Upon contact with skin - burning pain, swelling, burn with blisters.
First aid: rinse eyes and face with water, put on a gas mask or a cotton-gauze bandage moistened with a 5% solution of citric acid, rinse exposed skin with plenty of water, immediately leave the source of infection.
If ammonia gets into the stomach, drink several glasses of warm water with the addition of one teaspoon of table vinegar per glass of water and induce vomiting.
Reaction of ammonia with water and acids
Both an aqueous solution of ammonia and ammonium salts contain a special ion - the ammonium cation NH4, which plays the role of a metal cation. It is obtained as a result of the fact that the nitrogen atom has a free (lone) electron pair, due to which another covalent bond is formed with the hydrogen cation, which is transferred to ammonia from acid or water molecules:
This mechanism for the formation of a covalent bond, which arises not as a result of the sharing of unpaired electrons, but due to a free electron pair present in one of the atoms, is called donor-acceptor.
- NH3 + HCl = NH4Cl
- 2NH3 + H2SO4 = (NH4)2SO4↓
- NH3 + H20<->NH4 + OH-
If you add a few drops of phenolphthalein to an ammonia solution, it will turn crimson, i.e. it will show an alkaline environment:
Slide 20
Ammonium salts
enter into an exchange reaction with acids and salts:
- (NH4)2SO4 + Ba(NO3)2 → BaSO4 ↓ + 2NH4NO3(NH4)2CO3 + 2HCl → 2NH4Cl + H2O + CO2
react with alkali solutions to form ammonia - a qualitative reaction to ammonium ion:
- NH4Cl + NaOH → NaCl + NH3 + H2O
- decompose when heated NH4Cl → NH3 + HCl
- NH4NO3 → N2O + 2H2O
- (NH4)2Cr2O7 → N2 +Cr2O3+ 4H2O
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Nitrogen
and its connections
Unnoticeable in the atmosphere
And in reactions it is inert.
Can be beneficial
Serve in fertilizers...
Resides in the body
Plays a significant role...
We need him on the planet
To everyone, both adults and children...
What element are we talking about?
A Z O T
Being in nature
Nitrogen ranks 17th in abundance in the earth's crust, accounting for 0.0019% of the mass of the earth's crust
In bound form - mainly in the composition of two nitrates: sodium NaNO 3 (found in Chile, hence the name Chilean nitrate) and potassium KNO 3 (found in India, hence the name Indian saltpeter) and a number of other compounds.
In free form -
in the atmosphere
Five famous chemists of the 18th century. They gave a certain non-metal, which in the form of a simple substance is a gas and consists of diatomic molecules, five different names.
- “poisonous air”
- “dephlogisticated”
air"
- “spoiled air”
- "suffocating air"
- “lifeless air”
In 1772, a Scottish chemist
botanist and doctor Daniel Rutherford
In 1772, an English chemist
Joseph Priestley
In 1773, the Swedish chemist
pharmacist Karl Scheele
In 1774, an English chemist
Henry Cavendish
In 1776, a French chemist
Antoine Lavoisier
And it's all about nitrogen
Nitrogen forms strong diatomic N molecules 2 with short distance between cores
The molecule is diatomic and very strong
Structural formula N N
It contains a molecular lattice and a covalent
non-polar bond
Nitrogen is a colorless, odorless and tasteless gas.
Slightly soluble in water (2.5 volumes of nitrogen dissolve in 100 volumes of water).
It is lighter than air - 1 liter of nitrogen has a mass of 1.25 g.
At -196 C 0 nitrogen liquefies, and at -210 C 0 turns into a snow-like mass.
N 2
Nitrogen in compounds can manifest itself as
negative and positive CO.
Chemical properties of nitrogen
- Nitrogen reacts with oxygen
(at electric arc temperature)
N 2 + O 2 =2NO
2. Nitrogen reacts with hydrogen (at a temperature of 300 0 C and pressure 20-30 MPa)
N 2 +3H 2 =2NH 3
3. At elevated temperatures, nitrogen reacts with certain metals
3Mg+N 2 =Mg 3 N 2
Production of nitrogen in industry :
Fractional distillation of liquid air
OJSC
"Nevinnomyssk Azot"
Plant for the production of nitrogen from liquid air
Obtaining nitrogen in the laboratory (decomposition of ammonium salts)
1. Decomposition of ammonium nitrite
N.H. 4 NO 2 =N 2 + 2H 2 O
2. Decomposition of ammonium dichromate
(NH 4 ) 2 Cr 2 O 7 =Cr 2 O 3 +N 2 +4H 2 O
Application
N 2
As a refrigerant
In cosmetology
For creating
inert
environment during experiments
For synthesis
ammonia
Application of nitrogen compounds
- production of mineral fertilizers
- production of explosives
- production of medicinal products
Nitric oxide (I) N 2 O
N 2 O – nitric oxide (I), nitrous oxide or “laughing gas”, has a stimulating effect on the human nervous system, and is used in medicine as an anesthetic. Physical properties: gas, colorless and odorless. Exhibits oxidizing properties and easily decomposes. Non-salt-forming oxide.
2N 2 O=2N 2 + O 2
Nitric oxide (V)
- N 2 O 5 – nitric oxide (V), nitric anhydride, white solid (mp. = 41 0 WITH). It exhibits acidic properties and is a very strong oxidizing agent.
The product of the reaction between an acidic
oxide and water is an acid
Nitric acid
One bond with oxygen is formed according to the donor-acceptor mechanism, but due to the proximity of the atoms in the molecule they become equivalent.
Application of nitric acid
Production of nitrogen and complex
fertilizers
Production of explosives
Dye production
Medicine production
Film production,
nitro varnishes, nitro enamels
Production
artificial fibers
As a nitrating component
mixtures, for trawling
metals in metallurgy
Nitric acid salts
What are the salts of nitric acid called?
Nitrates K, Na, NH 4 + are called nitrates
Make up names using the formulas:
Nitrates – white crystalline
substances. Strong electrolytes, in
solutions completely dissociate
to ions. They enter into exchange reactions.
How can you determine the nitrate ion in solution?
When heated, nitrates decompose the more completely the more to the right the metal forming the salt is in the electrochemical voltage series.
Li K Ba Ca Na Mg Al Mn Zn Cr Fe Co Sn Pb Cu Ag Hg Au
Me + NO 2 + O 2
nitrite + O 2
metal oxide + NO 2 + O 2
Write down equations for the decomposition reactions of sodium nitrate, lead nitrate, and silver nitrate.
2NaNO3 = 2NaNO2 + O2
2Pb(NO 3) 2 = 2PbO + 4NO 2 + O 2
Slide 1
The letters are given: R, Z, I, O, A, P, T, M. These letters contain the name of an element about which it is known: - 78% of air consists of a simple substance formed by this chemical element; - the hydrogen compound of this element helps to bring a person out of fainting; - ancient manuscripts are stored in the atmosphere of this gas; - the acid formed by this element dissolves silver, but does not dissolve iron and aluminum; - this acid forms salts that are beneficial to plants, but harmful to people; - if the Russian names of chemical elements are arranged in alphabetical order, then the first one will be...Slide 2
Nitrogen is the eternal source of tantalum torment of humanity, it is the eternal torment of hunger in the midst of an ocean of abundance. M. Kamen (American biochemist).
Slide 3
Slide 4
According to the UN, one third of the world's population is hungry, and every minute several people die from this cause. What is the importance of nitrogen for the existence of life on Earth? Why is nitrogen associated with problems of food shortage and hunger? How can nitrogen solve this problem?
Slide 5
Sub-problems. History of the discovery of nitrogen. Prove the high reactivity of the element nitrogen. What physical properties are characteristic of the simple substance nitrogen? What reactions does molecular nitrogen enter into and what properties does it exhibit in them? What properties of nitrogen are its applications based on?
Slide 6
Give definitions of concepts. Atmosphere. Covalent chemical bond. Molecular crystal lattice. Oxidation-reduction reaction. Oxidizing agent, reducing agent.
Slide 7
Project assignments. When, by whom and how was the element nitrogen discovered? How common is the element in nature? What explains the discrepancy between its name and symbol? What is the importance of nitrogen for the existence of life on earth? Why is the literal translation “lifeless”? What do you know about the element nitrogen? Give its general characteristics. Write the electronic formula and electronic diagram of the structure of the nitrogen atom. Determine the characteristic oxidation states. Why is the chemical element nitrogen highly reactive?
Slide 8
Project assignments. What physical properties are characteristic of the simple substance nitrogen? Draw a diagram of the structure of a nitrogen molecule. What is the mechanism of formation and the nature of the chemical bond in the nitrogen molecule? Why is the nitrogen molecule inert? What reactions does molecular nitrogen enter into and what properties does it exhibit in them? Give examples of reactions that characterize the chemical properties of nitrogen. Why, despite the high nitrogen content in the air, does life on our planet not stop?
Slide 9
Project assignments. How is nitrogen obtained in industry? What properties of nitrogen are its applications based on? What is the essence of the cycle of the element nitrogen in nature? Why is nitrogen called the element of war in some cases, and the element of life and peace in others?
Slide 10
Nominations. "The most scientific." "The most ineresting". "The most original." "Most Illustrated"
Application of nitrogen
Pure nitrogen is used in various production processes, including ammonia synthesis and the production of nitrogen fertilizers, methane conversion, and associated gas processing.
Nitrogen is used to protect ferrous and non-ferrous metals during annealing. It finds applications in the processes of neutral hardening, stress relief annealing, carburizing, cyanidation, brazing, powder metal sintering, and die cooling. Metallurgy
The use of nitrogen when treating paper, cardboard and even wood objects with ultraviolet or cathode rays to polymerize the varnish coating allows for reduced photoinitiator costs, reduced VOC emissions, improved processing quality, etc. Pulp and paper industry
In the food industry, nitrogen is registered as a food additive E941, as a gaseous medium for packaging and storage, a refrigerant, and liquid nitrogen is used when bottling oils and non-carbonated drinks to create excess pressure and an inert environment in soft containers Food industry
Nitrogen is used in oil and gas production to maintain in-situ pressure and increase product production. This inert gas is widely used to create an inert cushion to ensure explosion and fire safety in process tanks, as well as during loading and unloading operations. Nitrogen is used to maintain a certain pressure in oil and gas tanks, to clean process tanks on gas carriers and LNG and LNG storage facilities, and to purge pipelines. Oil and gas industry
Nitrogen is used to protect tanks, to store raw materials and product, to transport chemical products and to package pharmaceuticals. Pharmaceuticals
Preventing oxidation in semiconductor and electrical circuit manufacturing, purging and cleaning are the main applications of nitrogen in the electronics industry. Electronics
Nitrogen is used in this industry to cool the electrodes of arc furnaces. In addition, it is used to protect against oxidation during production and reduce air temperature. Glass industry
Liquid nitrogen is widely used as a refrigerant; it is used in medicine, especially in cosmetology. Medicine
Nitrogen is the most popular gas for ensuring explosion and fire safety in various industries: from food to nuclear. Being an inert gas, nitrogen allows, when supplied to a technological volume, to displace oxygen and avoid an oxidation reaction. Firefighting