The Relationship between the Equilibrium Constant and the Reaction Quotient The reaction quotient, Q, is an expression that is identical to the equilibrium constant expression, but its value is calculated using concentrations that are not necessarily those at equilibrium. aA + bB
cC + dD
Q = [C]c [D]d [A]a [B]b When Q < K, the system will move to the right, favoring products. When Q > K, the system will move to the left, favoring reactants. When Q = K, the system is at equilibrium. Example: The reaction below takes place inside a cylinder with a movable piston: 2NO2 (g)
N2O4 (g)
At STP, the equilibrium concentrations inside the cylinder are [NO2] = 0.0206 M and [N2O4] = 0.0724 M. a) Calculate Keq.
b) Calculate the concentration of each gas at the moment that the piston is used to half the volume of the reacting mixture. Assume that the temperature remains constant.
c) Determine the value of Q when the volume is halved.
d) Predict the direction in which the reaction will proceed to re-establish equilibrium.
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requires a ______ ______ where nothing leaves or enters the system. - No net change in concentration of reactants or products occurs. - Quantities of reactants and products are usually not equal (only the speeds of the. forward and reverse reactions
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