Metallurgy - chemical reactions. 1.2

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🔴 Reaction of metals with nonmetals. 

• Sodium reacts with chlorine  

2 Na + Cl ₂  ----- > 2 NaCl

Sodium reacts with chlorine to form salt of sodium chloride.

🔴 Reaction of non metals with oxygen.

• Complete combustion of carbon 
  
  
  C + O₂  ----- > CO₂

Complete combustion of carbon, carbon dioxide gas is formed. 

• Partial combustion of carbon. 

2C + O₂  ----- >  2CO

Partial combustion of carbon to form carbon monoxide gas.

• Sulphur burn in air.  

S + O₂  ----- > SO₂

Sulphur burns in air to form Sulphur dioxide gas

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🔴 Reaction of non metal with water. 

(Generally non metals do not react with water except the halogens) 

• Chlorine gas passed through water 

Cl₂ (g)+ H₂ O(l)  ----- > HOCl(aq)+HCl(aq)

Chlorine gas passes through water to form hypochlorous acid.

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🔴Reaction of dilute acids with nonmetals. 

(Generally non metals do not react with acid except the halogens) 

• Chlorine gas reacts with hydrogen bromide /hydro bromic  acid

Cl₂(g) + 2HBr (aq) ----- > 2HCl(aq)+Br₂ (aq)

Chlorine gas reacts with hydrogen bromide /hydro bromic  acid to form hydrochloric acid and aqueous bromine liberate.

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🔴Reaction of non-motals with hydrogen.

• Molten sulphur reacts with hydrogen.

S + H₂ ----- > H₂S

Molten sulphur reacts with hydrogen at 450 °C temperature to form hydrogen sulphide gas.

• Nitrogen gas reacts with hydrogen gas 

N₂ + 3H₂ ----- > 2NH₃

Nitrogen gas reacts with hydrogen gas at high temperature and pressure and in presence of iron catalyst to form ammonia gas.

• Aluminium oxide means bauxite react with aqueous solution of sodium hydroxide. 

Al ₂ O ₃ .2H ₂ O (s) + 2NaOH (aq)  ----- > 2 NaAlO ₂ (aq) + 3 H₂ O (l)

Aluminium oxide means bauxite reacts with the aqueous solution of sodium hydroxide to form the aqueous solution of sodium aluminate.

• Aqueous sodium aluminate is diluted by water 

NaAlO₂ + 2H₂O ----- > NaOH + Al(OH)₃

Aqueous sodium aluminate is diluted by water to form precipitation of aluminium hydroxide. 

• Aluminium hydroxide is heated.

2Al(OH)₃  ----- > Al₂O₃ + 3H₂O

 Aluminium hydroxide is calcinated ( heated ) at 1000 °C to form alumina.

• Zinc sulphide is heated in excess air 

2ZnS + 3O ₂ ----- >2ZnO + 2SO ₂

Zinc sulphide is heated in excess air to form zinc oxide and Sulphur dioxide gas is liberated. 

• Zinc carbonate is heated in a limited supply of air.

ZnCO ₃ ----- > ZnO + CO ₂

Zinc carbonate is heated in a limited supply of air means calculated to form zinc oxide and carbon dioxide gas is limited

• Zinc oxide is reduced by carbon 
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ZnO + C ----- > Zn + CO

Zinc oxide reacts with suitable reductant such as carbon to form  zinc and carbon monoxide gas is liberated

• Manganese dioxide is ignited with aluminium.

3 MnO₂ + 4 Al ----- > 3Mn + 2 Al₂O₃ + Heat 

        

Manganese dioxide is ignited with aluminium powder we get metal manganese and Aluminium oxide.

• Iron oxide reacts with aluminium.

Fe₂O₃ + 2Al ----- > 2Fe + Al₂O₃ + Heat

Iron oxide reacts with aluminium to form metal iron and Aluminium oxide.

  

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