Unit 6: Equilibrium in Physical and Chemical Processes

15 Questions

What is the equilibrium constant denoted by when expressed in terms of partial pressures?

Which concept classifies substances as acids or bases?

Arrhenius concept

What is the ionic product constant for water?

What plays a crucial role in the transport and delivery of O2 from our lungs to our muscles?

Equilibria involving O2 molecules and hemoglobin

Which equilibrium state depends on concentration of the electrolyte and that of the common ion?

Degree of ionization

What do buffer solutions help to maintain?

Stable pH levels

What gives rise to a constant vapour pressure in a closed container when a liquid evaporates?

Number of molecules leaving the liquid equals the number returning to liquid from the vapour

In a dynamic equilibrium stage, what happens to the rates of the forward and reverse reactions?

The rates become equal

What does the double half arrows in H2O (l) H2O (vap) represent?

Simultaneous processes of evaporation and condensation

What is the name given to the mixture of reactants and products in the equilibrium state?

Equilibrium mixture

Which factor is important in optimizing operational conditions for favorable equilibrium in industry and laboratory?

Temperature

What does it mean when a reaction proceeds nearly to completion?

Negligible concentrations of the reactants are left

In which group are the reactions where only small amounts of products are formed and most of the reactants remain unchanged at equilibrium stage classified?

Group (ii)

How do the concentrations of reactants and products vary at equilibrium in reactions belonging to Group (iii)?

Concentrations of reactants and products remain unchanged

What is significant for optimizing operational conditions for favorable equilibrium towards desired products in industry and laboratory?

Concentration of products, temperature, and nature of reactants

Study Notes

Equilibrium is a crucial concept in chemistry, important for biological and environmental processes.
At equilibrium, a system reaches a state where the number of molecules leaving a liquid equals the number returning, resulting in constant redistribution and no net change.
Equilibrium can be established for physical processes (like evaporation) and chemical reactions.
In a chemical reaction, the reactants and products reach a dynamic equilibrium when the rates of the forward and reverse reactions are equal.
The extent of a reaction in equilibrium varies depending on experimental conditions like concentrations and temperature.
Equilibrium can be classified into three groups based on the extent of the reaction: reactions that proceed nearly to completion, reactions in which only small amounts of products are formed, and reactions where the concentrations of reactants and products are comparable.
Optimizing experimental conditions is essential in industry and lab settings to favor the desired product's formation.
Chemical equilibria are essential for various processes like O2 transport in the body and CO toxicity.
The law of equilibrium states that the concentrations of reactants and products in a reaction mixture are constant once equilibrium is reached.
Equilibrium constants (Kc and Kp) can be used to express the relationship between reactants and products at equilibrium.
Factors like temperature, pressure, and presence of catalysts can affect the equilibrium state of a reaction.
Acids and bases can be classified according to different theories (Arrhenius, Bronsted-Lowry, Lewis) and can be weak or strong based on their ionization constants.
The degree of ionization of an electrolyte depends on the concentration of the common ion and the electrolyte itself.
The pH scale is used to represent hydrogen ion concentration.
Water plays a dual role as an acid and a base due to its ionization.
The ion product constant (Kw) and pKw represent the equilibrium constant for water's ionization.
Buffer solutions are used to resist changes in pH.
The solubility product constant is used to describe the equilibrium between a solute and its saturated solution.

Test your understanding of the dynamic nature of equilibrium, the law of equilibrium, equilibrium constants, factors affecting the equilibrium state of a reaction, and classification of substances as acids or bases according to Arrhenius and Bronsted-Lowry theories.

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