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117177
The extraction of metals
Description
Mind Map on The extraction of metals, created by jasmin.sahota on 31/05/2013.
Mind Map by
jasmin.sahota
, updated more than 1 year ago
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Created by
jasmin.sahota
about 11 years ago
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Resource summary
The extraction of metals
found in ores containing oxygen and sulfur
iron oxide, Fe2O3
Fe3+ to Fe
reduction from a 3+ to 0
copper sulphide CuS, to copper
+2 to O
need a cheap, readily available reducing agent
impurities (gangue) clay and rock have to be removed
non-polluting and easy to dispose of by-products
converting sulphides to oxides
heating in air, called roasting
zinc sulphide converted to zinc oxide
ZnS(s) + 1.5O2(g) ---> ZnO(s) + SO2(g)
however SO2 is an acidic gas and produces (sulphuric acid) when mixed with water, a contributor to acid rain
however SO2 can be coverted to sulkphuric acid in controlled conditions and sold for a variety of purposes
SO2(g)+H2O(g)+0.5O2(g)-->H2SO4(l)
choosing a reducing agent
Coke
impure form of carbon
cheaply obtained by heating coal in the absence of air
however so metals require very high temperatures (ends up uneconomic)
at high temps metal react with carbon to form carbides
Hydrogen
made from methane and water
used to extract tungsten
metals high up on the reactivity series
can use electrolysis
such as sodium and aluminium
use a more reactive metals
recycling and the environment
iron
can be melted down and reformed
easily separated from other materials because it is magnetic
does not produce CO2 when melted down
whereas extraction does
however energy needs to melt involves the production of CO2
aluminium
also recycled by melting
only uses 5% of energy needs for extraction
recycling avoids large amount of CO2 formed
however big rising costs in sorting and transporting of recycled material
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