chemical reactions

• NH3 - gas

CH4

NH4+

CO3(2-)

NO3(-)

SO4(2-)

CH3COOH

C60

• equilibrium is the point in a reversible reaction where rate of forward reaction = rate of reverse reaction • reaction can only reach equilibrium if the reaction mixture is in a closed system • dynamic equilibrium means reactants are still forming products and vice versa but the rate of these are equal

• if equilibrium lies to the right, conc. of P > conc. of R - if equilibrium lies to the left, conc. of R > conc. of P

• increasing pressure favours the side with fewer gaseous moles • decreasing pressure favours the side with more gaseous moles

• adding a reactant/removing a product shifts equilibrium to the RIGHT • adding a product/removing a reactant shifts equilibrium to the LEFT

• increasing temperature favours the endothermic reaction - decreasing temperature favours the exothermic reaction

• do not change the position of equilibrium - only allows equilibrium to be achieved more quickly

PO4(3-)

form a white precipitate forms a blue precipitate forms a green precipitate forms a brown precipitate

• conc of solute is at a maximum - conc of solvent is at a minimum

1) if the metal hydroxide is concentrated, an alkene forms 2) if the metal hydroxide is dilute, an alcohol forms