Topic 4 - Extracting Metals and Equilibria

reactivity series

potassium, sodium, calcium, magnesium, aluminium, zinc, iron, hydrogen, copper, silver gold

displacement reactions

a more reactive metal will displace a less reactve metal from its salt. this is an exothermic reaction

how are most metals extracted

reduction of ores

how are unreactive metals extracted

they can be found in their natural state

why are metals not always extracted using electrolysis

it is very expensie, and if a metal is less reactive than carbon, reduction with carbon can occur

phytoextraction

plants absorb and concentrate the metal

doesnt cause pollution however takes a long time

bioleaching

bacteria oxidise ions and release atoms

why recycle metals

saves energy and produces less pollution

what must a life cycle assessment include

obtaining raw materials

manfucaturing the product

using the product

disposing of the product

dynamic equilibrium

the point at which the rate of forward and backwards reaction is equal, the concentration of the reacting substances does not change, and the forward and backward reactions dont stop

haber process

ammonia is formed when nitrogen (from air) and hydrogen (from natural gas) are reacted together, and reach dynamic equilibrium

Haber Process conditions

temp of 450 degrees, pressure of 200 atm, and iron catalysts

increase of temp in dynamic equilibrium

move positions of equilibrium towards the endothermic reaction

increase of pressure in dynamic equilibrium

shifts the position of equilibrium in the direction of the fewest mols of gas

increase of concentration of a reacting substance

moves position of equilibrium away from reacting substances

adding a catalyst in dynamic equilirium

causes both forward and backwards reactions to increase rate, so overall does not move position of equilibrium, and doesnt increase yield