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AE S2 K6 Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen.

AE S2 K6 Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen. AE S2 K6- Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen AE S2 K7 reactions which release these oxides.

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AE S2 K6 Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen.

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  1. AE S2 K6 Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen.

  2. AE S2 K6- Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen AE S2 K7 reactions which release these oxides Since the industrial revolution more coal has been burnt and more metals have been produced. Sulfur dioxide is generated in both of these processes.

  3. AE S2 K6- Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen AE S2 K7 reactions which release these oxides Industrial sulfur dioxide: 1) sulfur in fossil fuels, particularly coal. When combusted the sulfur combines with oxygen to form SO2. S(s) + O2(g)  SO2(g) 2) Smelting of metal ores to produce metals. CuS(l) + O2(g)  Cu(l) + SO2(g)

  4. AE S2 K6- Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen AE S2 K7 reactions which release these oxides • Natural sulfur dioxide: • Volcanic eruptions and bushfires release sulfur dioxide. • 2) Bacteria decompose organic matter to produce H2S(g) • Then.. • 2H2S(g) + 3O2(g)  2SO2(g) + 2H2O(g)

  5. AE S2 K6- Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen AE S2 K7 reactions which release these oxides • Industrial nitrogen oxides: • Formed in car engines where high temp overcomes the normally v. high activation energy needed to break the triple bonded N2 • Then • N2(g) + O2(g)  2NO(g) High T needed • 2) 2NO + O2(g)  2NO2(g) Spontaneous

  6. AE S2 K6- Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen AE S2 K7 reactions which release these oxides • Natural nitrogen oxides: • NO produced by bacteria and lightening (N2) • NO2 produced by sunlight breaking bonds in NO and O2 • N2O produced by bacteria.

  7. Health and other effects: • Sulfur dioxide: irritating gases which worsen respiratory disorders (asthma). • Acid rain (see later)

  8. Health and other effects: • Sulfur dioxide: irritating gases which worsen respiratory disorders (asthma). • Acid rain (see later) • Nitrogen oxides: Photochemical smog • Acid rain

  9. AE S2 K10 – Explain the formation and effects of acid rain

  10. AE S2 K10 – Explain the formation and effects of acid rain

  11. What is acid rain? Normal rainwater has a pH of about 5.6, which means it is naturally slightly acidic. This natural acidity is due to carbon dioxide which dissolves in rainwater and forms carbonic acid, a weak acid. CO2 (g) + H2O  H2CO3 (aq) Rainwater with a lower pH than normal is called acid rain.

  12. What is acid rain? The burning of fossil fuels in power stations and cars forms pollutants such as SO2and NO2. Dissolve in water to produce SO2 + H2O  H2SO3 (sulfurous acid) 4NO2 + 2H2O + O2 4HNO3 (nitric acid) Also 2SO2(g) + O2 (g)  2 SO3(g) SO3(g) + H2O(l)  H2SO4(aq)

  13. Acid rain has many damaging effects on the environment: • Buildings: • The strong acids in acid rain speed up the chemical weathering of rocks and buildings especially those made of marble and limestone (calcium carbonate) • CaCO3 (s) + 2H+(aq)  Ca2+(aq) + H2O(l) + CO2(g) • Also corrodes iron Fe(s) + 2H+ (aq)  H2(g) + Fe2+ (aq)

  14. Acid rain has many damaging effects on the environment: • Plants • The acidification of soil can affect plant growth as many are pH sensitive. • Acids remove the waxy coating on leaves, killing some trees, especially pines. • Acids in rain leach Mg2+and Ca2+ions from the soil thereby reducing the supply of nutrients to plants and trees.

  15. Acid rain has many damaging effects on the environment: Aquatic life • Acid rain also leaches Al3+ ions from soil which accumulate in waterways and affect fish life. • The acidification of waterways can affect aquatic life as they too are pH sensitive. This can lead to loss of biodiversity, indirectly affecting all organisms in the ecosystem and in some cases the loss of all aquatic life.

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