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I Review | Constants | Periodic Table The equilibrium-constant expression Learning Goal: The equilibrium-constant expression is used to describe the concentration of reactants and products for a reaction in dynamic equilibrium. For ideal gases and ideal solutions in homogeneous equilibria, where all reactants and products are in the same phase, the extent to To understand the form and meaning of the equilibrium-constant expression. which a particular chemical reaction proceeds to products is given by the equilibrium equation Chemical reactions are usually not one-way trips from reactant to product. In fact, most chemical reactions are reversible to at least some extent. Products formed by the forward reaction may react with each other to regenerate aA + bB - cC + dD. K = the reactants. When reactants are mixed, they will begin to react at a forward reaction rate particular to that chemical reaction. As reactants are depleted and products are formed, however, the rate of the forward reaction begins to slow, and the rate of the reverse reaction begins to increase. where K is the equilibrium constant and the right-hand side of the equation is known as the equilibriu n-constant expression. Eventually, the forward and reverse reaction rates will be identical. Equilibrium is dynamic, meaning that it is a The concentration of each product raised to its coefficient is divided by the concentration of each reagent raised to its coefficient according the the balanced chemical equation. Therefore, the higher the concentration of products, the larger the value of K will be. balance of continuous forward and reverse reactions. To indicate this dynamic nature of equilibrium, chemical equations of reactions with measurable reverse reaction rate are written using a double-headed arrow: aA + bB - cC + dD Part A Understanding the magnitude of K By analyzing the equilibrium-constant expression we can determine that a larger concentration of products in the numerator of the expression will result in larger values for K. Greater values of K are associated with reactions running toward completion, whereas smaller values of K are associated with a larger concentration of reactants. Value of K Reaction favors Reaction lies to K 1 products right Note that reaction stoichiometries with a large difference e number of moles of reactants and products may not strictly follow these general guidelines. Part B Part C Where does the equilibrium of this reaction lie? View Available Hint(s) O To the left O To the right O To neither the left nor the right Submit