IB Chemistry - Equilibrium (7)

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Chemistry

Equilibrium

Chemistry (SL)

11th

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24 Terms

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Arrhenius equation
k = Ae^(-Ea/RT)
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Arrhenius equation rearranged
lnk = -Ea/R * 1/T + lnA
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Catalyst effect on equilibrium
no effect
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Le Chatelier's Principle
when stress is applied to a system at equilibrium, the system changes to relieve the stress
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HEAT reaction mixture
Position of equilibrium shifts in the endothermic direction (to take up the heat)
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COOL reaction mixture
Position of equilibrium shifts in the exothermic direction
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Increase pressure of mixture
Equilibrium moves towards the direction with fewer gas molecules
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Effect of concentration on equilibrium
Adding product: equilibrium shifts towards the reactantsAdding reactant: equilibrium shifts towards the products
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equilibrium constant expression
\[products]/[reactants]
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What is the use of the equilibrium constant?
An equilibrium constant provides information about how far a reaction proceeds at a particular temperature
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The reaction quotient (Q)
The ratio for the concentrations of the reactants and products (raised to the appropriate powers) at any point in time.
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If Q
reaction proceeds to the right in favour of products
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If Q\>Kc
reaction proceeds to the left in favour of reactants
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What affects the equilibrium constant?
temperature only
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Increasing temperature on an exothermic reaction
the value of equilibrium constant decreases
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Increasing temperature on an endothermic reaction
the value of equilibrium constant increases
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Low Gibbs free energy
High entropy
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The relationship between equilibrium and Gibbs free energy
The position of the equilibrium corresponds to the mixture of reactants and products that produces the minimum value of Gibbs free energy and the maximum value of entropy
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Equilibrium constant (Gibbs free energy)
∆G = -RT*lnk
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The relationship between partial pressure and concentration can be worked out using
PV = nRT = P = n/V*RT
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partial pressure of a gas
\[concentration]*RT
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Equilibrium constant of gas
Kp = Kc * (RT)^ ∆n, where ∆n is the number of molecules of a gas on the right side of the equation minus the number of molecules of gas on the left side
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Explaining the effect of changes in concentration on the position of equilibrium
The value of the equilibrium constant is not affected by a change in concentration
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state of equilibrium
Q = Kc