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Equilibrium (IB)
Equilibrium (IB)
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25 Terms
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Reversible Reaction
A chemical reaction that can proceed in both forward and reverse directions.
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Dynamic Equilibrium
A state in which the rates of the forward and reverse reactions are equal, resulting in no net change in concentrations.
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Equilibrium Constant (Kₓ)
The ratio of the concentrations of products to reactants at equilibrium, constant at a given temperature.
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Le Chatelier’s Principle
The principle stating that an equilibrium system will adjust to counter changes in concentration, temperature, or pressure.
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Reaction Quotient (Q)
A measure of the relative concentrations of reactants and products at any point in a reaction.
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Condition for Equilibrium
A closed system where reactants and products are contained, allowing reactions to operate without interference.
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Single Arrow (→)
Indicates a non-reversible reaction that proceeds only in one direction.
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Double Arrow (⇌)
Indicates a reversible reaction in a state of dynamic equilibrium.
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Factors Affecting Equilibrium Position
Concentration, temperature, pressure, and the presence of catalysts.
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Homogeneous Equilibrium
An equilibrium where all reactants and products are in the same phase.
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Heterogeneous Equilibrium
An equilibrium where reactants and products are in different phases.
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Phase Equilibrium
The state of balance between phases, such as liquid and gas, within a system.
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Vapor Pressure
The pressure exerted by a gas in equilibrium with its liquid phase at a given temperature.
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Catalyst
A substance that increases the rate of chemical reactions without being consumed, not affecting equilibrium position.
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Exothermic Reaction
A reaction that releases heat, favoring products at lower temperatures.
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Endothermic Reaction
A reaction that absorbs heat, favoring products at higher temperatures.
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Effect of Temperature on Equilibrium
Changes in temperature can shift equilibrium positions and alter the value of Kc.
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Effect of Pressure on Equilibrium
Changing pressure affects equilibrium in gaseous reactions based on the number of gas molecules.
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Effects of Concentration Changes
Adding or removing reactants or products affects the equilibrium position but not Kc.
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Equilibrium Law
At a given temperature, the expression for the equilibrium constant is determined by the stoichiometry of the balanced equation.
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Kc Expression Example
For the reaction aA + bB ⇋ cC + dD, Kc = [C]^c [D]^d / [A]^a [B]^b.
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Phase Changes at Equilibrium
At equilibrium, phase changes like evaporation and condensation occur at equal rates.
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Impact of Doubling Coefficients
Doubling the coefficients in a reaction results in the new equilibrium constant being raised to the power of two.
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Impact of Halving Coefficients
Halving the coefficients results in the equilibrium constant being the square root of the original Kc.
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Direction Prediction Using Q
Comparing Q to Kc helps predict if the reaction will shift forward or backward to reach equilibrium.
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