Chem_Sheet_2_1 - Equilibrium a forward reaction and a...

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Equilibrium : a forward reaction and a reverse reaction proceed at equal rates, and the concentrations of reactants and products remains constant K c = [G] g [H] h … / [A] a [B] b When the equation for a chemical reaction for which the equilibrium constant is K c is reversed : K’ c = 1/K c When the coefficients of an equation are multiplied by a common factor n to produce a new equation: K’ c = (Kc) n When we add the equations for individual reactions, the equilibrium constants are multiplied K p = (P G ) g (P H ) h … / (P A ) a (P B ) b where P is a Partial Pressure K p = K c (RT) Δngas Δngas = (g + h + …) – (a + b + …) R= .08206 L atm mol -1 K -1 A very large K c or K p signifies that a reaction essentially goes to completion (not reversible) A very small K c or K p signifies that the forward reaction only occurs to a slight extent Q = [G] g in [H] h in … / [A] a in [B] b in If Q < K c : a net change occurs in the forward direction If Q > K c : a net change occurs in the reverse direction Le Chatelier’s Principle : When any change in concentration, temperature, pressure, or volume is imposed on a system at equilibrium, the system responds by attaining a new equilibrium condition that minimizes the impact of the imposed change When the external pressure is increased (volume reduced) equilibrium shifts in direction producing the smaller number of moles
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