equilibrium constant Kp for homogenous systems Flashcards
What is the total pressure of a gas mixture?
The total pressure is the sum of all the partial pressures of the individual gases.
What is partial pressure?
The pressure a gas would exert if it occupied a container on its own.
How do you calculate partial pressure?
First, calculate the mole fraction of a gas in a mixture.
What is the equation for the equilibrium constant Kp?
Kp = products / reactants
What is the relationship between Kp and the equilibrium expression for a reaction?
Kp = (pC^c * pD^d) / (pA^a * pB^b)
What are the units for Kp?
Units for Kp are by cancelling the pressures.
How does temperature affect Kp?
Kp is affected by temperature; changing temperature shifts equilibrium to counteract the change.
What happens to Kp when the equilibrium lies to the right?
Kp is larger.
What happens to Kp if there are more reactants?
Kp decreases (larger denominator).
What happens to Kp if there are more products?
Kp increases (larger numerator).
What is the effect of temperature on Kp for exothermic reactions?
Increase in temperature = decrease Kp; decrease in temperature = increase Kp.
What is the effect of temperature on Kp for endothermic reactions?
Increase in temperature = increase Kp; decrease in temperature = decrease Kp.
Is Kp affected by changes in pressure?
Kp is not affected by pressure changes.
What happens to equilibrium when pressure of reactants is changed?
Equilibrium shifts in the other direction to increase the pressure of the other side.
Is Kp affected by catalysts?
Kp is not affected by catalysts.
What does a catalyst do in a gas phase reaction?
It speeds up the rate of reaction but does not affect the number of particles.
What factors can increase the rate at which equilibrium is reached?
Increasing pressure, temperature, and using a catalyst.
Fill in the blank: The equilibrium constant Kp must be calculated for a system at _______.
CONSTANT TEMPERATURE
