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Questions and Answers
Which type of system allows the exchange of both energy and matter with its surroundings?
Which type of system allows the exchange of both energy and matter with its surroundings?
An isolated system can exchange energy with its surroundings.
An isolated system can exchange energy with its surroundings.
False
What is the difference between extensive and intensive properties?
What is the difference between extensive and intensive properties?
Extensive properties depend on the amount of matter in the system, while intensive properties do not.
A system that exchanges energy but not matter with the surrounding is called a ______.
A system that exchanges energy but not matter with the surrounding is called a ______.
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Match the following properties with their classifications:
Match the following properties with their classifications:
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What happens during an adiabatic process?
What happens during an adiabatic process?
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In an isoboric process, the pressure of the system changes.
In an isoboric process, the pressure of the system changes.
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What is the First Law of Thermodynamics?
What is the First Law of Thermodynamics?
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The change in internal energy of a gas in a free expansion is _____
The change in internal energy of a gas in a free expansion is _____
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Match the following processes with their characteristics:
Match the following processes with their characteristics:
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What is the equation for calculating enthalpy?
What is the equation for calculating enthalpy?
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Heat absorbed by the system is considered negative.
Heat absorbed by the system is considered negative.
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What is heat capacity?
What is heat capacity?
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What type of heat capacity refers to the heat capacity of one mole of a system?
What type of heat capacity refers to the heat capacity of one mole of a system?
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Lattice enthalpy is the enthalpy change associated with the complete combustion of a substance.
Lattice enthalpy is the enthalpy change associated with the complete combustion of a substance.
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What does Hess's Law state about the enthalpy change in a reaction?
What does Hess's Law state about the enthalpy change in a reaction?
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The enthalpy change when one mole of a liquid is converted into a gas is known as __________.
The enthalpy change when one mole of a liquid is converted into a gas is known as __________.
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Match the type of enthalpy with its description:
Match the type of enthalpy with its description:
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Which of the following is an example of a spontaneous process?
Which of the following is an example of a spontaneous process?
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Entropy is a measure of the degree of __________ of a system.
Entropy is a measure of the degree of __________ of a system.
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A non-spontaneous process always occurs without any external help.
A non-spontaneous process always occurs without any external help.
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Study Notes
System and Surroundings
- A system is a part of the universe where observations are made.
- The surroundings are the rest of the universe, excluding the system.
- The universe is the combination of the system and its surroundings.
Types of Systems
- Open system: Exchanges both energy and matter with its surroundings (e.g., hot coffee in an open vessel).
- Closed system: Exchanges energy but not matter with its surroundings (e.g., hot coffee in a closed vessel).
- Isolated system: Exchanges neither energy nor matter with its surroundings (e.g., hot coffee in a thermos).
Properties of a System
- Extensive properties: Depend on the amount of matter in the system. Examples include energy, internal energy, volume, enthalpy, mass, and entropy.
- Intensive properties: Independent of the amount of matter in the system. Examples include density, pressure, temperature, molar volume, specific heat capacity, viscosity, and refractive index.
State and Path Functions
- State function: Depends only on the initial and final state of the system (e.g., temperature, internal energy, volume, enthalpy, mass, entropy).
- Path function: Depends on the path taken to reach a particular state (e.g., heat, work).
Thermodynamic Processes
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Thermodynamic process: A process where the temperature of the system remains constant.
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Adiabatic process: A process where no heat transfer occurs between the system and its surroundings (Q = 0).
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Isochoric process: A process where the volume of the system remains constant (ΔV = 0).
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Isobaric process: A process where the pressure of the system remains constant (ΔP = 0).
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Sign Conventions
- Heat absorbed by the system: positive
- Heat released from the system: negative
- Work done by the system: negative
- Work done on the system: positive
Internal Energy
- Internal energy is the total energy of a system in a specific state.
- Internal energy is a state function.
First Law of Thermodynamics
- Energy can't be created or destroyed; it can only change forms.
Free Expansion
- In a free expansion, the work done is 0, the heat is 0, and the change in internal energy is 0.
Enthalpy
- Enthalpy is the total heat content of a system (H = U + PV).
Heat Capacity
- Heat capacity is the amount of heat required to raise the temperature of a system by 1 degree or 1 Kelvin (C = Q / ΔT).
Types of Heat Capacity
- Molar heat capacity: Heat capacity of 1 mole of a system.
- Specific heat capacity: Heat capacity of a unit mass of a system.
Hess's Law
- The enthalpy change of a reaction is the same whether it occurs in one step or multiple steps.
Thermochemical Equations
- A thermochemical equation is a balanced chemical equation that includes the enthalpy change of the reaction.
Spontaneous and Non-Spontaneous Processes
- Spontaneous process: Occurs naturally without external intervention.
- Non-spontaneous process: Needs external energy or intervention to occur.
Entropy
- Entropy is a measure of the disorder or randomness of a system.
Second Law of Thermodynamics
- The entropy of the universe always increases in a spontaneous process.
Gibbs Free Energy
- Gibbs free energy is the maximum amount of useful work a system can perform at a constant temperature and pressure (ΔG = ΔH – TΔS).
Third Law of Thermodynamics
- The entropy of a perfectly ordered crystalline substance approaches zero as the temperature approaches absolute zero.
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Description
Test your knowledge on the principles of thermodynamics, including systems, properties, and processes. This quiz covers topics like energy exchange, extensive and intensive properties, and the First Law of Thermodynamics. Challenge yourself with matching properties and understanding adiabatic and isoboric processes.
