2. Definition of NO:
NITRIC OXIDE (NO), also called nitrogen
monoxide, colourless toxic gas that is
formed by the oxidationof nitrogen. Nitric
oxide performs importantchemical
signaling functions in humans and other
animals and has various applications in
medicine. It has few industrial applications.
3. SOURCE OF NITRIC
OXIDE:
Natural Sources - Lighting Bolts
1. A natural source of nitrogen oxides occurs from a lightning stroke. The very high
temperature in the vicinity of a lightning bolt causes the gases oxygen and nitrogen in the
air to react to form nitric oxide.
N2+O2⟶NO
2.The nitric oxide very quickly reacts with more oxygen to form nitrogen
dioxide.
NO+O2⟶NO2
1.
Nitrogen oxides are produced from the reaction of nitrogen and oxygen gases in the air
during combustion, especially at high temperatures. At normal temperatures, oxygen and
nitrogen gases do not react
together.
2. Combustion of coal and oil at high temperature in industries and engines of
vehicles.
3.welding
4.factories of nitric oxide
4. EFFECTS OF NO:
SIDE EFFECTS OF NITRIC OXIDE:
1.Water Retention
2.Increased heart rate and palpitation
3.Fatigue
4.Skin irritation
5.Dry mouth
6.Kidney damage
5. OTHER EFFECTS OF NO:
1.Acid rain
2.Destroy building in particular chalk stones and marbles(think Taj
Mahal)
3.Acid rain is harmful to forests as chemicals in the soil damage the
trees
4.kill aquatic life because toxic . And it makes the lakes acidic . The
animals livingin them can die.
6. USES OF NO:
1.Nitric oxide is a gas that is inhaled.
2.It works by relaxing smooth muscle to widen (dilate)
blood vessels, especially in the lungs.
3.Nitric oxide is used togetherwitha
breathing machine (ventilator)to treat respiratory
failure in premature babies.
7. CONTROL OF NO:
1.Absorption by liquid:
* Absorption by Alkaline Solutions
* Absorption by Lime:
Aqueous suspension of calcium hydroxide can be used as the
scrubber to reduce NOx levels to 200 ppm. The calcium nitrite in the
solution can further be converted tomore valuablecalcium nitrate
by treatingwithsulphuric acid.
2H2SO4 + 3 Ca (NO2)2 → 2CaSO4 + 4 NO + Ca (NO3)2 + 2H2O
NOx Absorption by H2SO4:
H2SO4 reacts withNOx to form violetacid, H2SO4NO and nitrocyl
sulphuric acid, NOHSO4
NO + NO2 + 2H2SO4 → 2NOHSO4 + H2O
8. Methods of Controlling Nitrogen
Oxides:
fuel switching
fuel pre-treatment
combustion (or chemical process) modification
flue (or tail) gas denitrification.
