Metallurgy - chemical reactions 1.1

 

🔴 Metallurgy - chemical reactions  .1.1

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• Sodium metal exposed to air

4Na(s) + O₂ ----- > 2Na₂O(s)

When sodium metal exposed to air it react with oxygen to form sodium oxide

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• Magnesium ribbon burn in air

2Mg + O₂ ------ > 2MgO

Magnesium ribbon burn in air to form white powder of magnesium oxide.

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🔴 Reaction of metal oxide with water.

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• Sodium oxide dropped in water.

Na₂O + H₂O ----- > 2NaOH

Would you oxide soluble in water to form aqueous alkali sodium hydroxide.

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• Magnesium oxide dropped in water. 

MgO + H₂O ----- >Mg(OH)₂

Magnesium oxide when dropped in water to form an weak alkali,  milk of magnesia means magnesium hydroxide.

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🔴 Reaction of metals with water.

• Sodium metal dropped in water. 

2Na(s) + 2 H₂O(l)  -----> 2 NaOH(aq) + H₂(g) + Heat 

Sodium metal react rapidly and vigorously with water to form aqueous solution of sodium hydroxide in this process hydrogen gas and heat is liberated.

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• Potassium metal react with water

2K(s) + 2 H₂O(l) 2 KOH (aq) + H₂(g) + Heat

Potasium metal react rapidly and vigorously with water, in this process aqueous solution of potassium hydroxide form, hydrogen gas and heat is liberated.

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• Calcium metal was dropped into water. 

2 Ca(s) + 2 H₂O(l) -----> 2 Ca(OH)₂(aq) + H₂(g)

Calcium reacts with water slowly and lessly in this process calcium hydroxide is formed and hydrogen gas is liberated.

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• Water vapours are passed over aluminium metal.

2Al(s) + 3 H₂O(g) ---à  Al₂O₃(s) + 3H₂(g)

Water vapours are passed over aluminium metal to form Aluminium oxide and hydrogen gas is released.

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• Water vapour passed over iron metal. 

3Fe(s) + 4 H₂O(g) ---à  Fe₃O₄(s) + 4H₂(g)

Water vapour passed over air metal to form iron (II,III) oxide and hydrogen gas is liberated.

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• Water vapor passed over zinc.

Zn(s) +H₂O(g) ----- > ZnO(s) +H₂(g)

Water vapor passed over zinc to form zinc oxide and hydrogen gas is released.

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🔴 Reaction of metals with acids

Metal react with acid to form metal chloride and hydrogen gas is liberated.

• Magnesium metal react with hydrochloric acid. 

Mg(s) + 2HCl(aq) ------ > MgCl2(aq) + H2(g)

Magnesium metal react with hydrochloric acid to form magnesium chloride and hydrogen gas is liberated. 

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• Aluminium metal react with hydrochloric acid. 

2Al(s) + 6HCl(aq) ------ > 2AlCl₃(aq) + 3H₂(g)

Aluminium metal react with hydrochloric acid to form aluminium chloride and hydrogen gas is liberated.

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• Iron react with hydrochloric acid.
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• Fe(s) + 2HCl(aq) ----- > FeCl₂(aq) + H₂(g)

Iron react with hydrochloric acid to form iron chloride and hydrogen gas is liberated.

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• Zinc react with sulphuric acid.

Zn(s) + 2H₂SO₄aq) ----- > Zn SO₄(aq) + H₂(g)

Zinc react with sulphuric acid to form zinc sulphate and hydrogen gas is liberated.

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🔴 Reaction of metals with nitric acid. 

• Copper react with concentrated nitric acid. 

Cu(s) + 4 HNO₃(aq) ----- >  Cu(NO₃)₂₍aq) + 2NO₂(g) + 2H₂O(l)

Copper reacts with concentrated nitric acid to form copper nitrate and nitrogen dioxide gases liberated.

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• Copper react with dilute nitric acid.

3Cu(s) + 8 HNO₃(aq) ---à  3Cu(NO₃)₂₍aq) + 2NO(g) + 4H₂O(l)

Copper react with dilute nitric acid to form copper nitrate and in this process Nitric oxide liberates.

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