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Do now!

Do now!. Can you fill in the observations of the “Rusting” experiment?. Last lesson. Conditions needed for rusting Rust protection Sacrificial protection. Rusting. Rust is a form of iron oxide. It has water bonded loosely to it. It is called hydrated iron oxide. Learn!. Learn too!.

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Do now!

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  1. Do now! Can you fill in the observations of the “Rusting” experiment?

  2. Last lesson • Conditions needed for rusting • Rust protection • Sacrificial protection

  3. Rusting Rust is a form of iron oxide. It has water bonded loosely to it. It is called hydrated iron oxide Learn!

  4. Learn too! In order for iron to rust Both air and water’s a must, Air alone won’t do Without water there too, So protect it, or get a brown crust! It’s actually the oxygen in air

  5. Protecting from rust Painting is a barrier method But what about sacrificial protection?

  6. Copy! Sacrificial protection Zinc is electrically connected to the iron. Any water or oxygen reacts with the zinc (or magnesium) instead of the iron. Coating in zinc is called galvanization and it works even when the zinc coating is scratched.

  7. Today’s lesson • The extraction of iron from iron ore using a blast furnace • Extraction method and position in the reactivity series

  8. Ores Most metals are found naturally in rocks called ores. They are in compounds, chemically bonded to other elements iron ore

  9. Native Some unreactive metals can be found as elements. They are called native metals.

  10. Roasting Some unreactive metals can be extracted from a compound simply by heating. This is called roasting.

  11. Roasting copper sulphide Copper sulphide + oxygen copper + sulphur dioxide Cu2S(s) + O2(g) 2Cu(s) + SO2(g) Mr Porter will give you some slides to stick in

  12. Roasting lead sulphide Roasting lead sulphide produces lead oxide, NOT lead. The more reactive a metal is, the more difficult it is to extract from its ore. Can you copy please?

  13. Heating with carbon

  14. Extracting metals with carbon Carbon is higher than some metals in the reactivity series. It can be used to extract medium reactive metals.

  15. Extracting metals with carbon lead oxide + carbon lead + carbon dioxide 2PbO(s) + C(s) 2Pb(s) + CO2(g)

  16. Reduction and oxidation lead oxide + carbon lead + carbon dioxide 2PbO(s) + C(s) 2Pb(s) + CO2(g) carbon is oxidised lead oxide is reduced

  17. Mr Porter will give you some slides to stick in Reduction and oxidation lead oxide + carbon lead + carbon dioxide 2PbO(s) + C(s) 2Pb(s) + CO2(g) carbon is oxidised lead oxide is reduced Oxidation is the gain of oxygen, reduction is the loss of oxygen

  18. The Blast furnace Iron ore (haematite), coke (carbon) and limestone (calcium carbonate) Hot waste gases (recycled to heat furnace) 1000°C YouTube - Steelmaking: Blast Furnace 1500°C 1900°C Blasts of hot air Blasts of hot air Molten iron

  19. Reactions in the furnace The coke (carbon) reacts with oxygen in the hot air to make carbon dioxide C(s) + O2(g) CO2(g)

  20. Reactions in the furnace The carbon dioxide reacts with more hot coke to form carbon monoxide CO2(g) + C(s) 2CO(g)

  21. Reactions in the furnace The carbon monoxide then reduces (takes oxygen away) the iron oxide to iron Fe2O3(s) + 3CO(g) 2Fe(l) + 3CO2(g)

  22. Reactions in the furnace Limestone reacts with the impurities to form slag. CaCO3(s) + SiO2(s) CaSiO3(s) + CO2(g)

  23. Can you fill in the gaps?

  24. YouTube - Blast furnace YouTube - Steelmaking: Blast Furnace

  25. Homework Read pages 188 to 191 for next lesson (Friday)

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