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CSU CHEM 113 - Expressing Equilibria

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CHEM 113 1st Edition Lecture 12 Outline of Last Lecture I. How to represent K and QOutline of Current Lecture - K and Q for heterogeneous equilibrium- Expressing equilibria with pressure terms- Determining the direction of a reaction.Current Lecture- K and Q for heterogeneous equilibriumo A heterogeneous equilibrium involves reactants and/or products in different phaseso A pure solid or liquid always has the same concentration, or the same number of moles per liter of solid or liquid.o The expressions for Q and K include only species whose concentrations change asthe reaction approaches equilibrium. Therefore, pure solids and liquids are omitted from the expression for Q and K - Expressing equilibria with pressure termso K for a reaction may be expressed using partial pressures of gaseous reactants instead of molarity. This is used because gas pressure because it is easier to measure. The following is the equation for k expressed as partial pressure and can be derived from the ideal gas law  If the amount (mol) of gas does not change in the reaction, then K of partial pressure equals K of concentration.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- Determining the direction of reactionoo The value of q indicated the direction in which a reaction must proceed to reach equilibrium If Q< K the reactants must increase and the products decrease If Q> K the reactants must decrease and the products increase If Q=K, the system is at equilibrium and no further net change takes


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CSU CHEM 113 - Expressing Equilibria

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