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Equilibrium graph graph example 2example Equilibrium 2 Equilibrium graph example 3 Summary: - the rate of the fwd reaction is guided by the reactants and the rate of the rvs reaction is guided by the products - the higher the concentration the higher the rate - reaction rates of forward and reverse reactions are equal at equilibrium - the reactions continue to create reactant and product at equilibrium - equilibrium is the spot on the graph where concentration lines run parallel - concentrations of reactant and product are not necessarily equal at equilibrium (more to come on this....) At the beginning of a chemical reaction, there is nothing but reactant the speed of a reaction is determined by the concentration of: - reactants for the forward reaction - products for the reverse reaction So at the beginning of a reaction the rate of the forward reaction is fast and the reverse reaction is non-existent/very slow. As the reaction progresses and reactants turn into products, the concentration of products starts to increase. This makes the rate of the reverse reaction increase Eventually the concentrations of reactant and product are equal meaning the rate of the forward and reverse reactions are equal as well. This is when equilibrium is established (reaction keeps going) Misconceptions about equilibrium: 1. at equilibrium, concentrations of reactants and products are equal 2. the reaction must be finished because the concentrations aren't changing What equilibrium equations tells us: - each cat fights with one dog and each dog fights with one cat - a fight consists of 1 dog and 1 cat - fighting couples form and break up What equilibrium equations do not tell us: - how many cats in total vs. how many dogs in total - how many current single dogs and cats vs. how many fights Equilibrium graph example 1 Unit 2: Chemical Equilibrium Big Idea: Consider qualitatively and quantitatively the characteristics and applications of equilibrium systems in chemical reactions What do you know about valence equilibrium? https://www.youtube.com/watch?v=dUMmoPdwBy4 Indicator: Discuss why most chemical reactions do not proceed to completion Some chemical reactions proceed to completion: CH4 + O2 ---> CO2 + H2O Combustion reaction goes until all of the reactant is converted to product Most reactions do not go to completion: instead they approach an equilibrium state in which both reactants and products are present This occurs because the reaction is reversible the products formed by the reaction can themselves react to form the original reactants Reversible reactions can reach equilibrium Equilibrium: for a reversible reaction, a dynamic state in which the rate of the forward reaction is exactly equal to the rate of the reverse reaction Equilibrium equation 2 way arrow = reversible reaction Indicator: Discuss criteria for equilibrium Requirements for equilibrium: 1. can only occur in a closed system 2. rates of the forward reactions is the same as the rate of the reverse reaction 3. constancy or properties for the chemicals involved (ex: colour stays the same) When a reactions reaches equilibrium: 1. the rates of the forward and reverse reactions are equal 2. the concentrations of the reactants and products are constant (not necessarily equal) How does a reaction get there?