Reversible Reactions Flashcards
Example of an RR and equation
Heating copper (II) sulphate crystals CuSO4 (s) + 5H2O (g) --> CuSO45H2O(s)
And heating ammonium chloride
NH3(g) + HCl(g) –> NH4Cl (s)
Conditions of reversible reactions
Closed conditions
Dynamic equilibrium
Le Chatlier Principle
If dynamic equilibrium is disturbed by changing something, the reaction will counteract this change
Changing the pressure
If you increase the pressure, the reaction will go in the direction to produce less molecules in order to reduce the pressure eg
A + 2B –> C + D
The reaction will produce more C and D
Adding a catalyst
Equilibrium will be reached faster
Changing the temperature
If you increase the temperature the reaction will go in the exothermic direction to release the heat
The Haber Process
N2 + 3H2 2NH3
Nitrogen + hydrogen ammonia
Equation to calculate energy change
Break - make
Change= energy need to break - energy needed to break
Catalyst
Lowers the activation energy
Ammonia ideal conditions
Low temperature for more production
High temperature for speed
Very high pressure
Adding a catalyst
Conditions used to make ammonia
400 degrees- not high or low
200 atmospheres- low
Iron catalyst
Why are the ideal conditions not used to make ammonia
Low temperature would make more ammonia but at a slow speed to medium temperature is used
Low pressure is used because its very expensive to build a plant which can maintain high pressures
Uses of ammonia
Making fertiliser
Cleaning agent
Making explosives
Raw materials for ammonia and their production
Hydrogen made from methane and steam
Nitrogen is in the air
