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EQUILBRIUM TIERS 1 & 2

EQUILBRIUM TIERS 1 & 2. Describe what is meant by a reversible reaction Define forward reaction Define reverse reaction Describe a system that has reached dynamic equilibrium Define equilibrium position Define equilibrium expression Define equilibrium constant Describe a closed system.

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EQUILBRIUM TIERS 1 & 2

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  1. EQUILBRIUMTIERS 1 & 2 • Describe what is meant by a reversible reaction • Define forward reaction • Define reverse reaction • Describe a system that has reached dynamic equilibrium • Define equilibrium position • Define equilibrium expression • Define equilibrium constant • Describe a closed system

  2. Reversible Reactions Theoretically, every reaction can proceed in two directions, forward and reverse. Essentially all chemical reactions are considered to be reversible under suitable conditions. A chemical reaction in which the products can react to re-form the reactants is called areversible reaction. • A reversible chemical reaction is in chemical equilibriumwhen the rate of its forward reaction (reactants to products) equals the rate of its reverse reaction( products back to reactants) and the concentrations of its products and reactants remain unchanged. • A state of dynamic equilibrium has been reached when the amounts of products and reactants remain constant. • Both reactions continue, but there is no net change in the composition of the system.

  3. Reversible Reactions, continued The chemical equation for the reaction at equilibrium is written using double arrows to indicate the overall reversibility of the reaction. FORWARD REACTION 2HgO (s) 2Hg (l) + O2 (g) REVERSE REACTION 2Hg (l) + O2 (g) 2HgO

  4. The Equilibrium Expression GIVEN THE FOLLOWING REACTION THE EQUILIBRIUM EXPRESSION IS: THE EQUILIBRIUM EXPRESSION IS DEFINED AS THE RATIO OF THE CONCENTRATION OF THE PRODUCTS TO THE REACTANTS WHERE EACH CONCENTRATION IS RAISED TO THE POWER EQUAL TO ITS COEFFICIENT • After equilibrium is reached, the individual concentrations of A, B, C, and D undergo no further change if conditions remain the same. • A ratio of their concentrations should also remain constant. • The equilibrium constant is designated by the letter K.

  5. The Equilibrium Expression • The constant K is independent of the initial concentrations. • This means that there can be a infinite number of equilibrium positions but only one equilibrium constant at a particular temperature • Equilibrium position refers to the physical change in the equilibrium if it is disturbed. The concentrations may change but the ratio between products and reactants remain constant. • Kis dependent on the temperature of the system. The Equilibrium Constant • The numerical value of K for a particular equilibrium system is obtained experimentally. The equilibrium constant, K, is the ratio of the mathematical product of the concentrations of substances formed at equilibrium to the mathematical product of the concentrations of reacting substances. Each concentration is raised to a power equal to the coefficient of that substance in the chemical equation.

  6. FOR A REACTION TO REACH EQUILIBRIUM, IT MUST TAKE PLACE IN A CLOSED SYSTEM A CLOSED SYSTEM IS A SYSTEM THAT PREVENTS THE EXCHANGE OF MATTER WITH THE SURROUNDING EXAMPLES WOULD BE: STOPPED FLASK, SEALED JAR ETC.

  7. THE END

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