Chemical Equilibria Flashcards
What can cause imbalances in a chemical reaction?
- Temperature.
- Pressure.
- Energy.
- Concentration.
Systems at equilibrium are ________ and ________.
dynamic, reversible
What two states of matter CANNOT be used in equilibrium equations and why?
- Solids and liquids.
- Pure substances do not change concentration.
What is Kforward?
Products over reactants.
What is Kreverse?
Reactants over products.
What is Kc dependent on?
Temperature.
What are the units of K?
K is unitless.
If Kc > 1, what is the equation said to be?
Product favored because there will be more product molecule than reactant molecules.
If Kc<1, what is the equation said to be?
Reactant favored because there will be more reactant molecules than product molecules.
What is the conversion of Kp to Kc?
Kp= Kc x (RT)^mols. prod. - mols. reac.
When is Kp=Kc?
When delta n is zero.
Q=K.
Equilibrium.
Q<K.
The system shifts to the products.
Q>K.
The system shifts to the reactants.
If reactants increase, which way does the reaction shift?
To the products.
If reactants decrease, which way does the reaction shift?
To the reactants.
If products increase, which way does the reaction shift?
To the reactants.
If products decrease, which way does the reaction shift?
To the products.
As pressure increases or volume decreases, which side is shifted towards?
The side with fewer gas moles or towards the reactants.
As pressure decreases or volume increases, which side is shifted towards?
The side with more gas moles or towards the products.
If the moles of gases are equal, which side is shifted towards?
Neither, no shift occurs.
When the reaction is exothermic, where is heat placed?
On the products side.
When the reaction is endothermic, where is heat placed?
On the reactants side.
Do catalysts affect the equilibrium position of a system?
No.
