• Like
  • Save
E2 Acid Rain
Upcoming SlideShare
Loading in...5
×
 

E2 Acid Rain

on

  • 2,767 views

 

Statistics

Views

Total Views
2,767
Views on SlideShare
2,767
Embed Views
0

Actions

Likes
1
Downloads
114
Comments
0

0 Embeds 0

No embeds

Accessibility

Categories

Upload Details

Uploaded via as Microsoft PowerPoint

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Processing…
Post Comment
Edit your comment

    E2 Acid Rain E2 Acid Rain Presentation Transcript

    • E.2 Acid Rain
      • Acid deposition refers to acidic particles and gases that deposit or fall to earth
      • Acidic particles and vapours are deposited via two processes - wet and dry deposition.
        • Wet deposition is acid rain, the process by which acids with a pH normally below 5.6 are removed from the atmosphere in rain, snow or hail.
        • Dry deposition takes place when particles such as sulphates, nitrates, and gases (such as SO 2 and NOx), are deposited on, or absorbed onto, surfaces. The gases can then be converted into acids when they contact water.
      • Rain is naturally acidic because of dissolved CO2 but acid rain has a pH of less than 5.6. It is caused by oxides of sulfur and oxides of nitrogen.
    •  
    •  
    •  
    • The Origins of Acid Rain
      • Oxides of sulfur:
      • Sulfur dioxide occurs naturally from volcanoes and is produced industrially from the combustion of sulfur-containing fossil fuels and the smelting of sulfide ores.
      • S (s) + O 2 (g) -> SO 2 (g)
      • In the presence of sunlight sulfur dioxide is oxidized to sulfur trioxide
      • SO 2 (g) + ½ O 2 (g) -> SO 3 (g)
      • The oxides can react with water in the air to form sulfurous acid and sulfuric acid:
      • SO 2 (g) + H 2 O (l) H 2 SO 3 (aq)
      • SO 3 (g) + H 2 O (l) H 2 SO 4 (aq)
    • The Origins of Acid Rain
      • Oxides of nitrogen:
      • Nitrogen oxides occur naturally from electrical storms and bacterial action. Nitrogen monoxide is produced in the internal combustion engine and in jet engines.
      • N 2 (g) + O 2 (g) -> 2NO (g)
      • Oxidation to nitrogen dioxide occurs in the air.
      • 2NO (g) + O 2 (g) -> 2NO 2 (g)
      • The nitrogen dioxide then reacts with water to form nitric acid and nitrous acid:
      • 2NO 2 (g) + H 2 O (l) -> HNO 3 (aq) + HNO 2 (aq)
      • It can also be oxidized directly to nitric acid by oxygen in the presence of water:
      • 4NO 2 (g) + O 2 (g) + 2H 2 O (l) 4HNO 3 (aq)
    • Environmental Effects of Acid Rain
    • Methods to reduce the effects of acid rain
      • Removing sulfur dioxide from coal emissions using fluidized beds
      • Removing nitrogen dioxide from petrol combustion by using catalytic converters
      • Using more renewable forms of energy
      • Adding calcium oxide base (lime) to soil or water to neutralize the acid