| What is a Reversible Reaction? | -This is when the Reactants can React to make the Products AND the Products can react together to make the Reactants
-It just goes Both Ways |
| What is Equilibrium? How can this be Reached? | -Equilibrium is when the Reactions of both the Reactants [Forward] and the Products [Backwards] are at the Same Rate.
-As the Reactants react, their Concentration will Fall, therefore the Rate will Fall, but then more Products will be made, Increasing their Concentration and therefore Rate
-It will then Balance out, making an Equilibrium where No Overall Effect is taking Place [Dynamic Equilibrium] |
| What does Equilibrium need for it to Occur? | -It just needs a Closed System, that's it |
| So if a Reaction is at Equilibrium, does this mean the amount of Products and Reactants are Equal? | -No, It only affects the Rate and Concentration. The Amount of Product doesn't have to equal the Reactants [and Vice Versa] |
| What happens if the Position of the Equilibrium is on the Right? | -This means more of the Products, and Less of the Reactants - Concentration of Products > Concentration of Reactants |
| What happens if the Position of the Equilibrium is on the Left? | -This means more of the Reactants and Less of the Products -
Concentration of Reactants > Concentration of Products |
| What are the Three Things that can affect the Position of Equilibrium? | -Temperature
-Pressure [Gases only]
-Concentration |
