Reversible Reactions and Equilibrium
Shifting of Equilibrium
Changing Concentrations
- Adding more reacting or removing product means yield ↑
Changing Temperature
- Forward Reaction Exothermic: Temperature ↑ means yield ↓
- Forward Reaction Endothermic: Temperature ↑ means yield ↑
Changing Pressure (reactions which involve gasses)
- Fewer molecules on the right of the equation: Pressure ↑ means Yield ↑
- Fewer molecules on the left of the equation: Pressure ↑ means Yield ↓
Adding Catalyst
From Text Books
Reversible Reactions and Equilibrium
Reversible Reactions in a closed system are in equilibrium when
- The Forward and the reverse Reactions take place at the same rate.
- The Concentrations of reactants and products stay the same.
From Text Books
Reversible Reactions
From Text Books
In a reversible reaction, you can change the direction of the reaction by changing the conditions.
CuSO4.5H2O (s) ⇌ CuSO4 (s) + 5H2O (l)
The colour of Hydrated Copper sulfate turns from Blue to White. This colour changes again if water is added.
CoCl2.6H2O (s) ⇌ CoCl2 (s) + 6H2O (l)
The colour of Hydrated Cobalt (II) Chloride turns from Pink to Blue. Both of the examples are anhydrous substances (anhydrous cobalt chloride and anhydrous copper sulfate)
Haber Process
Haber Process is used to produce Ammonia. The Forward Reaction is Exothermic and the Reverse Reaction is endothermic.
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
From Text Books
Contact Process
Contact Process is used to produce Concentrated Sulphuric Acid. The Forward Reaction is Exothermic and the Reverse Reaction is endothermic.
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
From Text Books
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