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Le chantelier’s principle
An equilibrium opposes change
equilibrium concentration
Add reactant - towards product
Remove reactant - towards reactant
Add product - towards reactant
Remove product towards product
Equilibrium and pressure
Increase pressure moves towards side of fewer molecules
Decrease moves to more molecules
Harbour process
Pressure 200 atm
Temp - 450
Iron catalyst
KP
partial pressure = mole fraction of component x total pressure
Mole fraction = moles of component/ total number of moles
KC KP effected by?
Temperature only
Not change in pressure , amounts of substance , catalyst
They r constants
Changes to K
1) if equation reverse - inverse K
2) equation multiplied - square K
3) equation divided by- square root K
Bond enthalpy
Bonds broken - bonds formed
Oxidising agent
Gains electron
Reducing agent
Looses electron
Oxygen’s oxidation state
-2
-1 in peroxides
Water oxidation state
+1
-1 in metal halides