Chemical Equilibrium Concepts

A state where opposing forces balance each other out, resulting in no net change. In a chemical reaction, it means the rates of the forward and reverse reactions are equal.

A state where a chemical reaction and its reverse reaction proceed at the same rate, resulting in constant concentrations of reactants and products.

The point at which a system reaches equilibrium where the forward and reverse reactions occur at the same rate, leading to constant reactant and product amounts.

The ratio of product concentrations to reactant concentrations at equilibrium, raised to the power of their stoichiometric coefficients.

The rate of a chemical reaction is directly proportional to the concentration of reactants raised to their stoichiometric coefficients, denoted by 'k' and is specific to each reaction.

The rate at which a chemical reaction proceeds in the forward direction, denoted by 'k_f'.

The rate at which a chemical reaction proceeds in the reverse direction, denoted by 'k_r'.

The expression that relates the concentrations of reactants and products at equilibrium, showing the ratio of products to reactants raised to their stoichiometric coefficients, equal to the equilibrium constant (K).

A numerical value that represents the ratio of product concentrations to reactant concentrations at equilibrium, raised to the power of their stoichiometric coefficients.

The reaction proceeds to a greater extent, meaning more products are formed at equilibrium.

The reaction proceeds to a lesser extent, meaning less product is formed at equilibrium.

It indicates that the reaction will favor the formation of products, and will proceed mostly to completion before equilibrium is reached.

It indicates that the reaction favors the reactants, and will not proceed significantly to completion before equilibrium is reached.

They can start with different initial concentrations of reactants and products, and will still reach the same equilibrium position.

The ratio of product concentrations to reactant concentrations at equilibrium, raised to the power of their stoichiometric coefficients.

The rate of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.

The Haber process involves the industrial production of ammonia (NH3) from nitrogen gas (N2) and hydrogen gas (H2). The reaction is reversible and reaches equilibrium.

The equilibrium constant expression for the Haber process depends on the stoichiometry of the balanced chemical equation. The concentrations of the products and reactants are raised to the power of their respective stoichiometric coefficients.

The equilibrium constant (Kc or Kp) does not depend on the initial concentrations of reactants or products. The same equilibrium position will be reached regardless of the starting conditions.

The rate law describes the rate of a chemical reaction in terms of the concentrations of reactants. However, the equilibrium constant is determined by the ratio of product and reactant concentrations at equilibrium, not the rate of the reaction.

For a general reaction aA + bB ⇌ dD + eE, the equilibrium constant Kc is expressed as: Kc = [D]^d[E]^e / [A]^a[B]^b

The equilibrium constant is a measure of the relative amounts of reactants and products at equilibrium. It is a constant value for a given reaction at a specific temperature.

The ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of its stoichiometric coefficient.

The equilibrium constant expressed in terms of partial pressures of reactants and products.

The change in the number of moles of gas between products and reactants. Dn = (moles of gaseous products) - (moles of gaseous reactants).

The reaction strongly favors product formation at equilibrium, with products dominating.

The reaction strongly favors reactant formation at equilibrium, with reactants dominating.

A technique used to calculate equilibrium concentrations of reactants and products by setting up a table based on initial concentrations and changes determined by stoichiometry.

The process of finding equilibrium concentrations using an ICE table.

A calculation of equilibrium concentrations using an ICE table, given initial conditions and Kc.

The change in concentration of a reactant or product at equilibrium, represented by 'x'.

A method for solving for the equilibrium concentrations of reactants and products, involving setting up an ICE table and using the equilibrium constant expression.

A principle stating that if a system at equilibrium is disturbed, it will shift in a direction that relieves the stress.

The stress that can be applied to a system at equilibrium, including changes in temperature, pressure, or concentration.

The direction a reaction shifts to relieve the stress caused by a disturbance, either favoring the products or reactants.

The value of the equilibrium constant remains unchanged even after a disturbance.

Adding a reactant to a system at equilibrium will cause the system to shift to consume some of the added reactant, while removing a reactant will cause the system to shift to produce more of that reactant. The equilibrium constant (K) remains unchanged.

Increasing the volume of a system at equilibrium or decreasing its pressure will cause the system to shift towards the side with more moles of gas. Decreasing volume or increasing pressure will shift the system towards the side with fewer moles of gas. K remains the same.

Adding heat to an endothermic reaction shifts the equilibrium toward product formation, increasing the value of K. Adding heat to an exothermic reaction shifts the equilibrium toward reactant formation, decreasing the value of K.

A catalyst speeds up the rate of both the forward and reverse reactions, reaching equilibrium faster. The equilibrium composition remains unchanged. Catalysts lower the activation energy, allowing equilibrium to be achieved at lower temperatures.

A reaction is considered to be at equilibrium when the rates of the forward and reverse reactions are equal. This results in constant concentrations of reactants and products.