6.2 Flashcards
What happens to the position of the equilibrium when the proportion of products increases? (1)
moves to the right
What happens to the position of the equilibrium when the proportion of reactants increases? (1)
moves to the left
State Le Chatelier’s Principle. (2)
(1) If a system at equilibrium is disturbed,
(2) the equilibrium moves in the direction that tends to reduce the disturbance
What happens to the equilibrium and the yield when the conc. of a reactant increases in a reversible reaction? (3)
(1) the equilibrium shifts in the direction that reduces the conc. of the reactant
(2) so it’ll shift to the right
(3) so there’ll be a greater proportion of products in the mixture
When pressure changes in a gaseous reaction, the position of the equilibrium changes. Why? (1)
Because there’s a different number of molecules on either side of the equation.
Explain what happens to the position of the equilibrium when the pressure of the gaseous reaction increases. (3)
(1) the equilibrium moves to decrease the pressure
(2) so it’ll move to the side where there’s fewer molecules
(3) because fewer molecules exert less pressure
If there is the same number of moles of gases on both sides of the equation, does pressure have any effect on the position of the equilibrium? (1)
No
When temp increases in an exothermic reaction, which side does the equilibrium shift to? (3)
(1) the endothermic / left side
(2) as this side absorbs heat
(3) so it decreases the temp or counteracts the increase in temp
SUMMARY on the positions of equilibrium:
1. Pressure:
- inc = move to lower moles
- dec = move to higher moles
2. Conc. of reactants :
- inc = move to the right
- dec = move to the left
3. Temp. (forward = exo):
- inc = move to the endo / left side
- dec = move to the exo / right side
Revise this.
What effect does a catalyst have on the position of equilibrium? (1)
No effect
What is the change that a catalyst have on equilibrium? (1)
Catalysts allow equilibrium to be reached more quickly
