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Test 2- Ch. 17 Equilibrium State and Constant
chem 2 test 2
22
Chemistry
Undergraduate 1
03/27/2011

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Term
Equilibrium
Definition

Reactant and product concentrations stop changing because the forward and reverse rates have become equal

rate(fwd) = rate(rev)

Term
Equilibrium Constant K
Definition
K = (kfwd/krev) = [NO2]^2eq/[N2O4]eq
Term

Law of Chemical Equilibrium/

Law of Mass Action

Definition

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

Term
Reaction Quotient (Q)
Definition

The particular ratio of concentration terms that is written for a given reaction

At equilibrium: Q = K

Term
Form of Q for an Overall Reaction
Definition

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*...

Term
Relation of Q/K fwd and Q/K rev
Definition
Qc(fwd) = 1/Qc(rev)
Term
Q for a Reaction w/ Coefficients multiplied by a common factor
Definition
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
Term
Reactions Involving Pure Liquids or Solids
Definition

-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

Term
Qp- reaction quotient 
Definition
The equilibrium constant obtained when all components are present at their equilibrium partial pressures is designated Kp, the equilibrium constant based on pressures
Term
Relation of Kp and Kc
Definition

-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)

Term
Simplifying Assumption for Finding and Unknown Quantity
Definition

-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

Term
Le Chatelier's Principle Applied
Definition
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)
Term
Effect of  Change in Concentration
Definition

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

Term
Effect of an Inert Gas on Equilibrium Pressures
Definition
No effect on equilibrium
Term
Effect of Pressure on Equilibrium
Definition

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

Term
Effect of  Temperature on Equilibrium Position
Definition

-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

Term
Van't Hoff Equation
Definition
ln(K2)-ln(K1) = -(deltaH of reaction/R)*((1/T2)-(1/T1))
Term
Effect of a Catalyst
Definition
No effect on equilibrium position, just increases rate
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