What does Dynamic Equilibrium mean? Dynamic equilibrium means that both forward
and backward reactions are occurring simultaneously
List two features of Dynamic Equilibriums 1. Forward and Backward reactions are
occurring at equal rates
2. The concentration of reactants and products remain constant
What is Le Chatelier's Principle? Le Chatelier's principle states that if an external
condition is changed, the equilibrium will shift to oppose that change
Effect of Increased Temperature on Equilibrium If Temperature is increased, the
equilibrium will shift to oppose this and move in the endothermic direction to try and reduce
the temperature by absorbing heat
Effect of Decreasing Temperature on Equilibrium If Temperature is decreased, the system
will try and oppose this by increasing the surrounding heat by giving out heat exothermically
What is the benefits and downside of using a LOW-temperature Positive is that there will
be a high yield, Negative is that the reaction time will be slow. Therefore there is usually a
compromise
Effect of increasing pressure on equilibrium? If pressure is increased, the equilibrium
will shift to the side with the fewer moles of gas to oppose the change to reduce the pressure
Effect of lowering pressure on equilibrium? If the pressure is decreased, the equilibrium
shifts to the side with the more moles to increase the pressure
What happens when pressure is changed, but the number of moles is the same on both sides?
If both sides have the same number of moles, changing the pressure will have no
effect on the position of equilibrium
What is the effect of a catalyst on equilibrium? A catalyst does not affect the position of
equilibrium, but it will speed up the rate at which equilibrium is achieved
Why do Catalysts not affect the position of equilibrium? Catalysts do not affect the
position of equilibrium, because it speeds up the rate of the forward and backward reactions
by the same amount
List 2 industrial processes in which a catalyst is used in equilibrium 1. Haber Process
2. Contact process
3. Methanol from CO
4. Hydration of ethene to produce ethanol
List the details of the Haber Process: 1. N2 + 3H2 --> 2NH3
2. Exothermic (-ve)
3.450 temp, 450 atmospheric pressure, Iron catalyst
4. low temp, good yield, low rate
5. if pressure is too high, expensive
and backward reactions are occurring simultaneously
List two features of Dynamic Equilibriums 1. Forward and Backward reactions are
occurring at equal rates
2. The concentration of reactants and products remain constant
What is Le Chatelier's Principle? Le Chatelier's principle states that if an external
condition is changed, the equilibrium will shift to oppose that change
Effect of Increased Temperature on Equilibrium If Temperature is increased, the
equilibrium will shift to oppose this and move in the endothermic direction to try and reduce
the temperature by absorbing heat
Effect of Decreasing Temperature on Equilibrium If Temperature is decreased, the system
will try and oppose this by increasing the surrounding heat by giving out heat exothermically
What is the benefits and downside of using a LOW-temperature Positive is that there will
be a high yield, Negative is that the reaction time will be slow. Therefore there is usually a
compromise
Effect of increasing pressure on equilibrium? If pressure is increased, the equilibrium
will shift to the side with the fewer moles of gas to oppose the change to reduce the pressure
Effect of lowering pressure on equilibrium? If the pressure is decreased, the equilibrium
shifts to the side with the more moles to increase the pressure
What happens when pressure is changed, but the number of moles is the same on both sides?
If both sides have the same number of moles, changing the pressure will have no
effect on the position of equilibrium
What is the effect of a catalyst on equilibrium? A catalyst does not affect the position of
equilibrium, but it will speed up the rate at which equilibrium is achieved
Why do Catalysts not affect the position of equilibrium? Catalysts do not affect the
position of equilibrium, because it speeds up the rate of the forward and backward reactions
by the same amount
List 2 industrial processes in which a catalyst is used in equilibrium 1. Haber Process
2. Contact process
3. Methanol from CO
4. Hydration of ethene to produce ethanol
List the details of the Haber Process: 1. N2 + 3H2 --> 2NH3
2. Exothermic (-ve)
3.450 temp, 450 atmospheric pressure, Iron catalyst
4. low temp, good yield, low rate
5. if pressure is too high, expensive
