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Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
Revision on chapter 3 and chapter 9= chemistry
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Revision on chapter 3 and chapter 9= chemistry

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Revision on basic knowledge of chemistry on calculation on moles and chemical substances in industry

Revision on basic knowledge of chemistry on calculation on moles and chemical substances in industry

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  • 1. sulphur Sulphur dioxide Sulphur trioxide Oleum Sulphuric acid Stage 1 Stage 2 Stage 3 Hot air Dry oxygen X Water
  • 2.
    • State the name of the process to manufacture sulphuric acid in industry
    • Sulphur is heated in air in stage 1. Write chemical equation
    CONTACT PROCESS
  • 3.
    • Stage 2 is the production of SO3.
    • Write the equation
    • State the conditions
    • Temp . pressure .catalyst
    450-550 oC 1 atm VANADIUM PENTOXIDE
  • 4.
    • Stage 3 is the production of sulphuric acid
    • State substance X
    • Write equation for the formation of oleum
    • Oleum is mixed with water to form sulphuric acid. Write the equation
    Concentrated sulphuric acid
  • 5. State 2 uses of sulphuric acid As Fertilisers As detergents Electrolyte in car batteries Manufacture of plastic and synthetic fibres Manufacture of pesticides
  • 6.
    • Nitrogen +hydrogen  Ammonia
    • State the name of the process
    • Write chemical equation
    • State conditions.
    CONTACT PROCESS
  • 7. State 2 uses of ammonia in industry Manufacture fertilisers Manufacture explosives Manufacture nitric acid As a cooling agent Prevent coagulation of latex
  • 8. Fe + Cu Cu + Zn Cu + Sn Al + Mg Alloy Mixture of metals Alloy Mixture of metals Steel Bronze Brass Magnelium
  • 9. Plastic bag Name of polymer Structure monomer Structure polymer uses Polythene
  • 10. Raincoat, pipes Name of polymer Structure monomer Structure polymer uses Polyvinyl chloride
  • 11. Plastic chairs & tables Name of polymer Structure monomer Structure polymer uses Polypropene
  • 12. Soda lime glass Lead glass Fused silicate glass Borosilicate glass Type of glass Uses Type of glass Uses Cheap glass containers, mirrors Optical lenses, spectrometer Decorative glass and lamps Cooking utensils
  • 13. Relative atomic mass of magnesium is 24
    • Explain in terms of hydrogen standard
    • Explain in terms of carbon-12 standard
  • 14.
    • If an atom W is 32 times heavier than 1/12 of the mass of 1 atom carbon -12, what is its relative atomic mass?
    32
  • 15.
    • An atom of metal M is 1.6 times heavier than an atom of calcium. What is the relative atomic mass of M? ( Ca=40)
    •  
    1.6 x 40 =64
  • 16.
    • How many times a lead atom is heavier than a carbon atom?
    • ( Pb= 207, C=12)…
    207 / 12 = 17.25
  • 17.
    • A compound has the formula of NaXO 3 . The relative molecular mass is 151. Find the relative atomic mass of X (given RAM Na,23: O,16)
    151 – 23 – 3(16) = 80
  • 18.
    • What is meant by empirical formula and molecular formula?
    • Empirical formula is the simplest formula that shows s implest ratio of atoms in a molecule
    • Molecular formula is the real formula that shows actual number of atoms in a molecule
  • 19. substance Molecular form Empirical form substance Molecular form Empirical form benzene Glucose
  • 20. substance Molecular form Empirical form substance Molecular form Empirical form Propene ammonia
  • 21.
    • Metal X combines with 4.32 g of oxygen to form 13.68 g of metal oxide X. What is the empirical formula of the metal oxide X? [ RAM X, 52; O,16]
    Mass of X = 13.68 -4.32 g =9.36 g Mole of X = 9.36/52 = 0.18 Mole of O = 4.32/16 =0.27 X : O 0.18 : 0.27 18 : 27 X : O 2 : 3
  • 22.
    • The empirical formula of a compound is CH 2 . If its molecular formula is 56, what is its molecular formula?
  • 23.
    • A compound contain 40% carbon, 53.3 % oxygen , hydrogen 6.7% . If the relative atomic mass of the compound is 180, find
    • Empirical formula
    Mole of carbon = 40/12 = 3.33 Mole of O = 53.3/16 =3.33 C : O : H 3.33 : 3.33 : 6.7 1: 1 :2 C : O :H 1 : 1 :2 Mole of H = 6.7/1 =6.7
  • 24.
    • If the relative atomic mass of the compound is 180, find Molecular formula
  • 25. Mole = mass Mole = volume of gas Mole = number of particles Molar mass Molar volume Avogadro’s constant
  • 26.
    • Given that RAM Cu=64, C=12, O=16)
    • Mole of copper carbonate used
    •  
    CuCO 3 6.2 gram CO 2 CuO + Mole= mass/ mmass Mole= 6.2/ 124 Mole= 0.05
  • 27.
    • Mass of copper oxide formed
    CuCO 3 6.2 gram CO 2 CuO + Mass= mole x mmass Mass= 0.05 x CuO = 0.05 x 80 = 4 g From the equation, CuCO3 : CuO 1 : 1 0.05 : 0.05
  • 28.
    • Volume of carbon dioxide released at room conditions
    CuCO 3 6.2 gram CO 2 CuO + Volume of gas = mole x mvolume volume= 0.05 x 24 = 1.2 dm3 From the equation, CuCO3 : CO2 1 : 1 0.05 : 0.05
  • 29.
    • Number of molecules of carbon dioxide released
    CuCO 3 6.2 gram CO 2 CuO + Mole of carbon dioxide = 0.05 No of molecules = mole x NA No of molecules =
  • 30.
    • Number of atoms of carbon dioxide released
    CuCO 3 6.2 gram CO 2 CuO + No of atoms = 3 x no of molecules No of atoms =

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