Topic 11 Flashcards
What is the expression for Kp?
Can only be used on gases
How do you work out total pressure
How do you work out molar fractions?
How do you calculate Partial Pressure and what is it?
p(A) is the pressure that each type of gas exerts on its own In the total volume of the gaseous mixture
What are the steps for working out Kp?
- Molar Faction for each molecule
- Partial Pressure from the molar fractions calculated using total pressure
- Expression using molecular formula
- Units using the balancing numbers form the reaction
- Calculate Kp (atm)
What are the steps to calculate Kp with NO MOLES given?
- Find missing p(A) [Algebra required]
- Use missing p(A) to find other unknown p(A)
- Units using balancing numbers from the reaction
- Calculate Kp
How can you tell if an equation is exothermic or endothermic?
Exothermic has a negative enthalpy change as more energy is lost than absorbed (the overall energy has decreased)
Endothermic has a positive enthalpy change as more energy is absorbed than lost (the overall energy has increased)
What happens to the equilibrium constant when you increase the temperature in an exothermic reaction?
- Increasing temp means the equilibrium will shift to the right
- Fewer products form as more reactants form
- Meaning the numerator (where products are in Kc + Kp) would be smaller
- Decreasing the equilibrium constant
What happens to the equilibrium constant when you increase the temperature in an endothermic reaction?
- Increasing temp means that equilibrium shifts to the left
- More products form as fewer reactants form
- Meaning the denominator (where reactants go in Kp + Kc) would decrease
- Increasing the equilibrium constant
How does pressure affect the equilibrium constant?
Pressure has no effect on equilibrium constant
How does concentration affect the equilibrium constant?
Concentration has no effect on equilibrium constant
How does adding a catalyst affect the equilibrium constant?
Adding a catalyst has no effect on the equilibrium constant
