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What is the state of a system where observable quantities like concentration, temperature, and pressure do not change with time?
What is the state of a system where observable quantities like concentration, temperature, and pressure do not change with time?
Equilibrium
Physical equilibrium involves chemical changes.
Physical equilibrium involves chemical changes.
False
What is the equilibrium state between solid and liquid states called?
What is the equilibrium state between solid and liquid states called?
The equilibrium between liquid and gaseous states is called ______.
The equilibrium between liquid and gaseous states is called ______.
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What is the equilibrium state between a solid and the solid dissolved in a solution called?
What is the equilibrium state between a solid and the solid dissolved in a solution called?
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What is the equilibrium state between a gas and a gas dissolved in a solution called?
What is the equilibrium state between a gas and a gas dissolved in a solution called?
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What is the relationship between the mass of a gas dissolved in a liquid and the pressure applied?
What is the relationship between the mass of a gas dissolved in a liquid and the pressure applied?
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Equilibrium is a static process.
Equilibrium is a static process.
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What is the constant that is equal to the ratio of the concentration of products to the concentration of reactants at equilibrium?
What is the constant that is equal to the ratio of the concentration of products to the concentration of reactants at equilibrium?
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Catalysts affect the equilibrium constant.
Catalysts affect the equilibrium constant.
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What is the law that states that the rate of a reaction is directly proportional to the product of the concentration of reactants and products, each raised to the power of their stoichiometry?
What is the law that states that the rate of a reaction is directly proportional to the product of the concentration of reactants and products, each raised to the power of their stoichiometry?
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What is the ratio of the product of the concentration of products to the product of the concentration of reactants, each raised to the power of their stoichiometry?
What is the ratio of the product of the concentration of products to the product of the concentration of reactants, each raised to the power of their stoichiometry?
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What is the relationship between Kp and Kc?
What is the relationship between Kp and Kc?
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The value of the equilibrium constant is constant for a reaction at a constant temperature.
The value of the equilibrium constant is constant for a reaction at a constant temperature.
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Reversing a reaction changes the value of the equilibrium constant to its inverse.
Reversing a reaction changes the value of the equilibrium constant to its inverse.
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Multiplying a reaction by a factor of two squares the value of the equilibrium constant.
Multiplying a reaction by a factor of two squares the value of the equilibrium constant.
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Dividing a reaction by two results in the square root of the original equilibrium constant.
Dividing a reaction by two results in the square root of the original equilibrium constant.
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A catalyst affects the value of the equilibrium constant.
A catalyst affects the value of the equilibrium constant.
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What is the type of equilibrium where all reactants and products are in the same phase?
What is the type of equilibrium where all reactants and products are in the same phase?
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What is the type of equilibrium where reactants and products are present in more than one phase?
What is the type of equilibrium where reactants and products are present in more than one phase?
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The concentration of pure solids and liquids is considered constant.
The concentration of pure solids and liquids is considered constant.
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What is the product of the molar concentrations of ions raised to the power of their stoichiometric coefficients in a saturated solution?
What is the product of the molar concentrations of ions raised to the power of their stoichiometric coefficients in a saturated solution?
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What is the principle that states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will shift in a direction that relieves the stress?
What is the principle that states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will shift in a direction that relieves the stress?
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Increasing the concentration of reactants shifts the equilibrium in the forward direction.
Increasing the concentration of reactants shifts the equilibrium in the forward direction.
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Increasing the concentration of products shifts the equilibrium in the backward direction.
Increasing the concentration of products shifts the equilibrium in the backward direction.
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Exothermic reactions are favored by which type of temperature change?
Exothermic reactions are favored by which type of temperature change?
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Adding an inert gas at constant volume does not affect the equilibrium.
Adding an inert gas at constant volume does not affect the equilibrium.
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Adding an inert gas at constant pressure shifts the equilibrium towards the side with a greater number of moles.
Adding an inert gas at constant pressure shifts the equilibrium towards the side with a greater number of moles.
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Catalysts change the equilibrium position.
Catalysts change the equilibrium position.
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What are substances that can donate a proton called?
What are substances that can donate a proton called?
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What are substances that can accept a proton called?
What are substances that can accept a proton called?
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Amphoteric substances can act as both acids and bases.
Amphoteric substances can act as both acids and bases.
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What are substances that can accept a lone pair of electrons called?
What are substances that can accept a lone pair of electrons called?
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What are substances that can donate a lone pair of electrons called?
What are substances that can donate a lone pair of electrons called?
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The ionic product of water is represented by Kw.
The ionic product of water is represented by Kw.
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PH is a way of expressing hydronium ion concentration.
PH is a way of expressing hydronium ion concentration.
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PH can be calculated as the negative logarithm of hydronium ion concentration.
PH can be calculated as the negative logarithm of hydronium ion concentration.
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The pH of a strong acid can be calculated as the negative logarithm of its concentration.
The pH of a strong acid can be calculated as the negative logarithm of its concentration.
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The solubility product (Ksp) of an electrolyte is the product of the molar concentrations of its ions, each raised to the power of its stoichiometric coefficient.
The solubility product (Ksp) of an electrolyte is the product of the molar concentrations of its ions, each raised to the power of its stoichiometric coefficient.
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Study Notes
Equilibrium
- Equilibrium is a state where observable properties like concentration, temperature, and pressure remain constant over time.
- Equilibrium can be represented by an equals sign (=).
- Equilibrium can be physical or chemical.
Types of Equilibrium
-
Physical Equilibrium
- Involves no chemical change, only physical processes like melting, freezing, evaporation, condensation.
- Solid-Liquid Equilibrium: Equilibrium between a solid and liquid state (e.g., ice melting). Rate of melting = Rate of freezing of water.
- Liquid-Gas Equilibrium: Equilibrium between a liquid and gaseous state (e.g., evaporation of water). Rate of evaporation = Rate of condensation of water.
- Solid-Solution Equilibrium: Equilibrium between a solid and the dissolved solid in a solution (e.g., sugar dissolving in water). Rate of dissolving = Rate of precipitation
- Gas-Solution Equilibrium: Equilibrium between a gas and the dissolved gas in a solution (e.g., CO2 dissolving in water). Rate of dissolving = Rate of evolution
-
Chemical Equilibrium
- Involves chemical changes or chemical reactions.
- Reversible Reactions: Reactants forming products, and products reforming reactants (e.g., PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)).
- Irreversible Reactions: Reactants forming products, but products do not form reactants. These reactions do not show equilibrium (e.g.,CH4 + 2O2 → CO2 + 2H2O).
Law of Mass Action
- The rate of a reaction is directly proportional to the product of the concentration of reactants, each raised to the power of its stoichiometric coefficient. This is a principle for describing the concentrations of the substances in chemical equilibrium
Equilibrium Constants
- Equilibrium constant (Kc) is the ratio of product of concentration of products to the product of concentration of reactants, each raised to the power of its stoichiometric coefficient.
- Equilibrium constant (Kp) is similar but calculates using partial pressures when all reactants and products are gaseous.
- The value of the equilibrium constant (Kc & Kp) remains constant at a fixed temperature for a reaction.
Factors Affecting Equilibrium
- Concentration: Increasing the concentration of reactants shifts the equilibrium towards the products, while increasing the products shifts it towards the reactants.
- Temperature: Exothermic reactions are favoured at low temperatures, while endothermic reactions favour high temperatures.
- Pressure: Equilibrium shifts toward the side with fewer moles of gas when pressure increases.
- Catalysts: Catalysts have no effect on the equilibrium position, only the rate at which equilibrium is attained.
- Addition of inert gases: At constant volume, adding inert gases has no effect on equilibrium, but at constant pressure, this may change the equilibrium position.
Equilibrium Constants Characteristics
- Constant at a specified temperature.
- Reversed reactions have inverse constants.
- Multiplied reactions have constants raised to the corresponding power.
- Divided reactions have constants raised to the corresponding reciprocal power.
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Description
This quiz explores the concept of equilibrium, focusing on its definition and various types including physical and chemical equilibria. Covering examples such as solid-liquid, liquid-gas, and gas-solution equilibria, it helps deepen your understanding of how different states of matter interact. Test your knowledge on the rates of changes and observable properties in equilibrium.
