# Test 2- Ch. 17 Equilibrium State and Constant

Flashcard maker : Thomas Alday
 Equilibrium
 Reactant and product concentrations stop changing because the forward and reverse rates have become equal rate(fwd) = rate(rev)
 Equilibrium Constant K
 K = (kfwd/krev) = [NO2]^2eq/[N2O4]eq
 Law of Chemical Equilibrium/ Law of Mass Action
 At a given temperature, a chemical system reaches a state at which a particular ratio of reactant and product concentrations has a constant value. Also, for a particular system and temp, the same equilibrium state is attained regardless of how the reaction is run
 Reaction Quotient (Q)
 The particular ratio of concentration terms that is written for a given reaction At equilibrium: Q = K
 Form of Q for an Overall Reaction
 If an overall reaction is the sum of two or more reactions, the overall reaction quotient (K) is the product of the reaction quotients(K or Q) for the steps: Koverall = K1 * K2 * K3*…
 Relation of Q/K fwd and Q/K rev
 Qc(fwd) = 1/Qc(rev)
 Q for a Reaction w/ Coefficients multiplied by a common factor
 If all the coefficients of the balanced equation are multiplied by some factor, that factor becomes the exponent for relating the reaction quotients and the equilibrium constants
 Reactions Involving Pure Liquids or Solids
 -concentration of a pure solid and pure liquid is constant -since the concern is only w/ concentrations that change as they approach equilibrium these solid and liquid concentrations are not included in the reaction quotient
 Qp- reaction quotient
 The equilibrium constant obtained when all components are present at their equilibrium partial pressures is designated Kp, the equilibrium constant based on pressures
 Relation of Kp and Kc
 -the exponent of the RT term equals the change in the amount (mol) of gas (delta(n) gas) from the balance equation, -1 Kp = Kc(RT)^(delta(n)gas)
 Simplifying Assumption for Finding and Unknown Quantity
 -if a reaction has a relatively small k and relatively large initial concentration, the concentration change ‘x’ can often be neglected – if the assumption results in a change that is less than 5% the original concentration, the error is not significant, and the assumption is justified
 Le Chatelier’s Principle Applied
 When a disturbance occurs, we say that the equilibrium; position shifts, which means that concentrations(or pressures) change in a way that reduces the disturbance, and the system attains a new equilibrium position (Q = K again)
 Effect of; Change in Concentration
 Whenever the concentration of a component changes, the equilibrium system reacts to consume some of the added substance or produce some of the removed substance -note: the value of Kc does not change at given temp
 Effect of an Inert Gas on Equilibrium Pressures
 No effect on equilibrium
 Effect of Pressure on Equilibrium
 If pressure increases, reaction shifts to the side with fewer moles of gas – change in volume results in change in concentration but does not change Kc
 Effect of; Temperature on Equilibrium Position
 -A temperature increase(adding heat) favors the endothermic direction while a temperature decrease (removing heat) favors the exothermic direction -Temp rise will increase K for a system with a positive deltaH of reaction -Temp rise will decrease K for a system with a negative deltaH of reaction
 Van’t Hoff Equation
 ln(K2)-ln(K1) = -(deltaH of reaction/R)*((1/T2)-(1/T1))
 Effect of a Catalyst
 No effect on equilibrium position, just increases rate