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Equilibrium Concepts and Applications: Le Chatelier’s Principle, Solubility, and RICE Tables

Explore the principles of equilibrium in chemistry through concepts such as Le Chatelier’s Principle, solubility, and RICE tables. Understand how to calculate equilibrium concentrations, predict equilibrium shifts, and determine the formation of precipitates. Learn how disturbances affect equilibrium and how to solve problems related to equilibrium constants, concentrations, and reactions. Discover the common ion effect and how to use the reaction quotient to assess saturation. Practice applying theoretical knowledge to solve equilibrium problems effectively.

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Equilibrium Concepts and Applications: Le Chatelier’s Principle, Solubility, and RICE Tables

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  1. Lessons 5-10Equilibrium CDT Clothier CDT Selleck

  2. Agenda • Objectives • Equilibrium constant/equilibrium concentration • RICE tables • Le Chatelier’s Principle • Solubility • Problem • Question and Answer

  3. Objectives • Understand the relationship between K and Q and how to use them • Use RICE tables to calculate the equilibrium concentration of reactants or products • Predict the effect on equilibrium for certain disturbances using Le Chatelier’s Principle • Predict if a precipitate will form in a reaction

  4. Equilibrium • Q<K, product favored Q>K, reactant favored Q=K, equilibrium

  5. RICE Table H2(g) + I2(g) Used to solve for equilibrium concentrations If given K, make reaction quotient expression and solve for x Remember that you can assume x away and check to see if the assumption is justified (<5% error)

  6. Le Chatelier’s Principle • When a chemical system at equilibrium is disturbed, it re-attains equilibrium by undergoing a net reaction that reduces the effect of the disturbance. • Concentration: no effect on K but if there is an increase/decrease in reactant the net direction of reaction is toward the product and vice-versa. • Pressure: no effect on K but an increase in P decreases V which causes formation of fewer moles of gas and vice-versa. • Temperature: K changes by van’t Hoff equation and an increase in T moves the reaction toward absorption of heat and vice-versa.

  7. Solubility • Determine solubility with a RICE table • Common Ion effect: the presence of a common ion decreases the solubility of a slightly soluble ionic compound. • Qsp=Ksp, solution is saturated, no change Qsp>Ksp, precipitate forms until saturated Qsp<Ksp, solution unsaturated, no precipitate

  8. Problem • Calculate the new equilibrium concentrations of [Ag] and [CN] when 5.00 moles of silver cyanide, AgCN decomposes in a 3 L container if the temperature is raised from 300 degrees Celsius to 500 degrees Celsius. Kc at 300 degrees Celsius is .068 and the standard heat of reaction is -126.05 kj/mol. • Note: all values are made up.

  9. Questions?

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