2824729
Description
Mind Map by sachakoeppen, updated more than 1 year ago
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Created by sachakoeppen
over 9 years ago
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Dynamic Equilibrium
- Occurs in reversible reactions, when the forward and backward rate are equal
- It needs a closed system (no reactants or products can escape)
- It needs a closed system (no reactants or products can escape)
- Pressure (gas) / concentration (solution)
- 2NO2 (g) = N2O4 (g)
Brown : Colourless
2 moles: 1 mole
- If pressure is increased, the equilibrium
moves to where there are fewer molecules.
- More N2O4 is produced therefore the container looks more colourless
- More N2O4 is produced therefore the container looks more colourless
- If pressure is increased, the equilibrium
moves to where there are fewer molecules.
- 2NO2 (g) = N2O4 (g)
Brown : Colourless
2 moles: 1 mole
- Temperature
- 2NO2 (g) = N2O4 (g)
Brown : Colourless
- Forward reaction is exothermic (ΔH= -ve) therefore
the backward reaction is endothermic ( ΔH= +ve)
- If temperature is increased, the equilibrium moves to the endothermic direction
- More NO2 (higher yield of NO2) formed therefore the container looks more brown
- More NO2 (higher yield of NO2) formed therefore the container looks more brown
- Forward reaction is exothermic (ΔH= -ve) therefore
the backward reaction is endothermic ( ΔH= +ve)
- 2NO2 (g) = N2O4 (g)
Brown : Colourless
- Catalysts have no overall effect on equilibrium as they
speed up the forward + reverse reaction equally
- 3H + N2 = 2NH3 ΔH= -ve
- Temp increased - the equilibrium will move to 3H + N2 because it is the endothermic direction
- Pressure increased - the equilibrium will move to 2HN3 because there are fewer molecules
- Temp increased - the equilibrium will move to 3H + N2 because it is the endothermic direction
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