- Dynamic Equilibrium -
I will be able to explain the concept of chemical equilibrium and its relationship to the concentrations of reactants and products in a reaction
key vocabulary: chemical equilibrium, dynamic equilibrium, equilibrium position, reversible reaction explain factors that affect equilibria list types of equilibrium - solubility, phase, and chemical equilibrium identify the 5 experimental conditions that must be met for dynamic equilibria to occur
explain what it means if the percent yield is 99% or between 1%-99% identify classes of chemical reactions at equilibrium define reversible reaction use ice tables and reaction progress graphs to determine equilibrium concentrations of reactants and products
Dynamic a force of action, movement, and change Static stationary, not acting or changing
mIG1cEw mIG1cEw F6s F6s vXt4 vXt4
1)Temperature 2)Pressure 3)Addition of product or reactant to the reaction vessel
Type of Equilibrium Description SOLUBILITY A dynamic equilibrium between a solute and a solvent in a saturated solution in a closed system PHASE A dynamic equilibrium between different physical states of a pure substance in a closed system CHEMICAL REACTION A dynamic equilibrium between the products and reactants of a chemical reaction in a closed system
1)The system must be closed 2)The reaction must be reversible 3)The rate of the forward reaction must be equal to the rate of the backward 4)The concentration of the reactants and products must be constant but not necessarily equal 5)The macroscopic properties must be equal
Concentration at Equilibrium x 100 % Theoretical yield
Reaction favours the reactants very strongly Mixing reactants has no observable result
Reaction favours the products very strongly Reactions are observed to be complete (quantitative) “usually” written with a single arrow – reverse reaction is negligible
Reaction favours reactants (closer to 1%) or products (closer to 99%) If in a closed system, these reactions can achieve equilibrium