3.1.10 Kp Flashcards
What is a homogeneous reaction?
A reaction where all the reactants and products are in the same state/phase
Name the three states
Gas
Liquid
Solid
What is partial pressure?
The pressure that each sample of gas would create if it was in a container on its own
Partial pressure formula
Mole fraction x total pressure
Mole fraction formula
No of moles of gas A in mixture / total number of moles of all gases
What should all mole fractions in a mixture add up to?
1
Which type of brackets do we use for Kp?
()
What happens to the equilibrium if Kp is greater than 1?
Equilibrium shifts to the right
More products than reactants
What happens to the equilibrium if Kp is less than 1?
Equilibrium shifts to the left
More reactants than products
What happens to the equilibrium if Kp is equal to 1?
Equilibrium is in the middle
Equal moles of products and reactants
What is the only condition which will affect the value of Kc?
Temperature
What is the method for calculating Kp?
- Fill in ICE rows of ice box
- Add up all values of elm moles
- Determine the mole fraction
- Calculate the partial pressure of each gas
- Sub in partial pressure values into your Kp formula
If the LHS has more moles
How will an increase in pressure effect the position of the equilibrium?
Equilibrium will shift to the right to oppose the increase in pressure
The yield of predicts will increase
If the forward reaction is exothermic How will an increase in temperature affect the position of the equilibrium?
The forward reaction is exothermic
The equilibrium will shift to the left to oppose the increase in temperature
The yield of reactants will increase
If the forward reaction is exothermic
How will a decrease in temperature affect the value of Kp?
The value of Kp will increase
The forward reaction is exothermic
The equilibrium will shift to oppose the decrease in temperature
