Equilibrium Constant Kp Flashcards
Mole fraction equation
Number of moles of gas \ total number of moles of all gasses
Partial pressure equation
Mole fraction x total pressure of gas 1
What does 𝓅 mean
The partial pressure of a gas
How do you write an expression for Kp from an equation and what to make sure to only include
Kp=𝓅 of product^n° in front/ 𝓅 of reactants^n° in front
Include only gases, ignore liquids, solids and aqueous.
What does Kp stand for?
Equilibrium constant
Equation to work out moles at equilibrium for reactants and products
Reactant =Initial moles - moles reacted
Product = initial moles + moles formed
What is an heterogeneous reaction
A reaction with substances in different states
The larger the Kp…
If Kp is small we say…
… the greater the amount of products
…the equilibrium favours the reactants
Kp and Kc only change with…
Temperature
If temperature is increased in an equilibrium which is exothermic is in the forward reaction..
The reaction will shift to oppose the change and move in the backwards endothermic direction. The value of Kp gets smaller as there are fewer products.
If pressure is increased what will happen in a reaction which has fewer moles of gas in the product side.
The reaction will shift to oppose the change and move to the side with fewer moles of gas. The position of equilibrium shifts right. The value of Kp stays the same.
What effect does increasing pressure have on Kp
No effect
What effect does increasing pressure have?
Increases the pressure terms on bottom of Kp expression more than the top.
System no longer in equilibrium so shifts right, increasing mole fraction of products as decreases mole fraction of reactants. The top of the Kc therefore increases and bottom decreases until original value of Kp restored.
