What is the formula for equilibrium constant?
Kc = [products]^ratio / [reactants]^ratio
What does it mean if Kc value is 1?
The concentration of products and reactants is the same
What does it mean if Kc value is >1?
The equilibrium position lies towards the products
What does it mean if Kc value is <1?
The equilibrium position lids towards the restarts
What does a dynamic equilibrium exist?
A dynamic equilibrium exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and the concentrations of reactants and products does not change
What is Le Chatelier’s Principle?
Brings back to equilibrium (effect of temperature pressure or concentration on the position of equilibrium)
What is homogenous equilibrium?
Contains equilibrium species that all have the same state or phase
What is heterogenous equilibrium?
Contains equilibrium species that have different states or phases (Kc only includes in Thai case species that are (g) or (aq))
What is mole fraction?
- Under the same conditions of temperature and pressure, the same volume of different gases contains the same number of moles of gas molecules
- The mole fraction of a gas is the same as it’s proportion by volume to the to volume of gases in a gas mixture
What is the mole fraction x(A)?
Number of moles of A / total number of moles in gas mixture
What is the partial pressure of a gas?
- In a gas mixture the partial pressure, p of a gas is the contribution that the gas makes towards the total pressure P
- The sum of the partial pressures of each gas equals the total pressure
What is the partial pressure for gas A?
p(A) = mole fraction of A x total pressure P
What does a catalyst do to the equilibrium?
A catalyst increases the rate of both forward and reverse reactions in an equilibrium by the same amount resulting in an unchanged position of equilibrium
What happens if the temperature changes?
K changes and the ratio of products and reactants change to reflect the new value of K
What happens when you increase the temperature of an exothermic forwards reaction and why?
- Decrease K
- Increased temperature, decreased K as reactant concentration must increase to reflect the lower K so the equilibrium shifts to the left
What happens when you decrease the temperature of an exothermic forwards reaction and why?
- Increase K
- Decreased temperature, increase in K as the concentration of the products must increase to reflect the higher K so the equilibrium shifts to the right
What happens when you increase the temperature of an endothermic forwards reaction and why?
- Increased K
- Increased temperature, increased K and so concentration of products must increase to reflect the higher k and so equilibrium shifts to the right
What happens when you decrease the temperature of an endothermic forwards reaction and why?
- Decreased K
- Decreased temperature, decreased K and so concentration of reactants must increase to reflect lower K so the equibliruum shifts to the left
What happens to K if you change the concentration?
If the concentration changes, K does not change so the ratio of pro cuts and reactants changes to rerun to the value of K
What happens when you increase the concentration of one of products?
- No effect of Kc
- Concentration of products decreased to return to the original value
- So equilibrium shifts to the left
What happens when you increase the concentration of one of reactants?
- No effect of Kc
- Increasing [reactant] disrupts equilibrium
- Concentration of products increased to return to original Kc value
- So equilibrium shifts to the right
What happens to Kc and pressure?
If the pressure changes, k does NOT CHANGE so the ratio of products and reactants change to return to the value of K
- Kc does not change
- System is now no longer in equilibrium (increased pressure increases concentration terms on bottom of Kc expression more than the top)
- Top of Kc expression increases and bottom decreased until Kc is reached
What happens as you increase the pressure?
- No effect on Kp
- Increasing pressure disrupts equilibrium
- Increase in pressure of (less moles side) to return to original Kp value do equilibrium shifts to the right
What happens when you decrease the pressure?
- No change to Kp
- Decreasing pressure disrupts equilibrium
- Increase the partial pressure of A and B (more moles side) to return to original Kp value
- Equilibrium shifts to the left
