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Module 3 - Chapter 10 - Equilibrium - Coggle Diagram
Module 3 - Chapter 10 - Equilibrium
Equilibrium constant
Provides the position of equilibrium
Equilibrium law
Square brackets mean concentration of
a,b,c and d are balancing numbers in overall equation, any vairation in moles raises to concentration to a power
Example
What does the constant tell us
If
= 1, equilibrium position is halway between reactants and products
If
> 1, position of equilibrium is towards the products
If
< 1, position of equilibrium is towards the reactants
Magnitude indicates the relative proportions of reactants and products in the equilibrium system
Units can be found by subbing the concentration units into the expression
Unaffected by concentration change or use of a catalyst
Changing temperature results in different concentrations
Dynamic equilibrium
Rate of the forward reaction equals the rate of the reverse reaction
Concentration of reactants and products doesn't change
System must be closed, temperature, pressure and concentrations are unaffected by external factors
Le chatelier's principle
Postion of the equilibrium indicates the extent of the reaction
When a system in equilibrium is subjected to an external chage, the system readjusts itself to minimise the effect of the change
Reaction conditions can be altered to maximise the yield of a desired product
Reversible reactions
Reactions that take place in both forward and reverse directions
Denoted by a double arrow
One reaction direction is exothermic and one is endothermic
Eventually reach a state of dynamic equilibrium
Haber process
Low temp, high yield of product by slow rate
High pressure increases rate but required expensive equipment
Conditions
350 degrees
100-200 atm
Iron catalyst
