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Questions and Answers
Chemical ______ is a state in which the concentrations of reactants and products in a chemical reaction remain constant over time.
Chemical ______ is a state in which the concentrations of reactants and products in a chemical reaction remain constant over time.
equilibrium
In a system at ______, the rates of forward and reverse reactions are equal.
In a system at ______, the rates of forward and reverse reactions are equal.
equilibrium
The ______ constant is a measure of the ratio of the concentrations of products to reactants at equilibrium.
The ______ constant is a measure of the ratio of the concentrations of products to reactants at equilibrium.
equilibrium
Homogeneous ______ occurs when reactants and products are in the same phase.
Homogeneous ______ occurs when reactants and products are in the same phase.
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According to ______ Principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change.
According to ______ Principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change.
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Increasing the concentration of a reactant or product will shift the ______ in the direction of the reaction.
Increasing the concentration of a reactant or product will shift the ______ in the direction of the reaction.
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Understanding chemical ______ is crucial in industries such as chemical manufacturing and pharmaceuticals.
Understanding chemical ______ is crucial in industries such as chemical manufacturing and pharmaceuticals.
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The ______ of a system is closed, meaning no substances can enter or leave the system.
The ______ of a system is closed, meaning no substances can enter or leave the system.
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The equilibrium is ______, meaning that reactions are still occurring, but at equal rates in both directions.
The equilibrium is ______, meaning that reactions are still occurring, but at equal rates in both directions.
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The equilibrium constant K is constant at a given ______, but changes with temperature.
The equilibrium constant K is constant at a given ______, but changes with temperature.
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Study Notes
Definition
Chemical equilibrium is a state in which the concentrations of reactants and products in a chemical reaction remain constant over time, with no net change in the composition of the system.
Characteristics
- The rates of forward and reverse reactions are equal.
- The concentrations of reactants and products are constant.
- The system is closed, meaning no substances can enter or leave the system.
- The equilibrium is dynamic, meaning that reactions are still occurring, but at equal rates in both directions.
Equilibrium Constant (K)
- A measure of the ratio of the concentrations of products to reactants at equilibrium.
- Represented by the symbol K.
- K is constant at a given temperature, but changes with temperature.
Types of Equilibrium
- Homogeneous equilibrium: reactants and products are in the same phase (e.g. gas, liquid).
- Heterogeneous equilibrium: reactants and products are in different phases (e.g. solid and gas).
Le Chatelier's Principle
- If a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change.
- This principle helps predict the direction of the equilibrium shift in response to changes in the system.
Factors Affecting Equilibrium
- Concentration: increasing the concentration of a reactant or product will shift the equilibrium in the direction of the reaction.
- Temperature: increasing the temperature will shift the equilibrium in the direction of the endothermic reaction.
- Pressure: increasing the pressure will shift the equilibrium in the direction of the reaction that produces fewer moles of gas.
Importance of Equilibrium
- Understanding chemical equilibrium is crucial in industries such as chemical manufacturing, pharmaceuticals, and environmental science.
- Equilibrium concepts are used to design and optimize chemical reactions, and to predict the outcome of reactions.
Definition of Chemical Equilibrium
- Chemical equilibrium is a state where the concentrations of reactants and products remain constant over time.
- The composition of the system remains unchanged, with no net change.
Characteristics of Chemical Equilibrium
- Forward and reverse reaction rates are equal.
- Concentrations of reactants and products are constant.
- The system is closed, meaning no substances can enter or leave.
- The equilibrium is dynamic, with reactions still occurring at equal rates in both directions.
Equilibrium Constant (K)
- K is a measure of the ratio of product concentrations to reactant concentrations at equilibrium.
- K is represented by the symbol K.
- K is constant at a given temperature, but changes with temperature.
Types of Equilibrium
- Homogeneous equilibrium: reactants and products are in the same phase (e.g., gas, liquid).
- Heterogeneous equilibrium: reactants and products are in different phases (e.g., solid and gas).
Le Chatelier's Principle
- If a system at equilibrium is subjected to a change, the equilibrium will shift to counteract the change.
- The principle helps predict the direction of the equilibrium shift in response to changes.
Factors Affecting Equilibrium
- Concentration: increasing the concentration of a reactant or product shifts the equilibrium in the direction of the reaction.
- Temperature: increasing the temperature shifts the equilibrium in the direction of the endothermic reaction.
- Pressure: increasing the pressure shifts the equilibrium in the direction of the reaction that produces fewer moles of gas.
Importance of Chemical Equilibrium
- Understanding chemical equilibrium is crucial in industries such as chemical manufacturing, pharmaceuticals, and environmental science.
- Equilibrium concepts are used to design and optimize chemical reactions and to predict the outcome of reactions.
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Description
Understand the concept of chemical equilibrium, its characteristics and how it works in a closed system. Learn about the rates of forward and reverse reactions and the constant concentrations of reactants and products.
