Introduction to Thermodynamics

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Questions and Answers

What type of thermodynamic system is a refrigeration cycle?

  • Isolated system
  • Closed system (correct)
  • Open system
  • None of the above

Which of the following is an example of a closed system?

  • A car engine (correct)
  • A boiling pot of water on a stove
  • A balloon filled with helium
  • A glass of water left out on a table

What is the main characteristic of an isolated system?

  • It can exchange mass but not heat with its surroundings.
  • It can exchange both heat and mass with its surroundings.
  • It cannot exchange either heat or mass with its surroundings (correct)
  • It can exchange heat but not mass with its surroundings.

A container of water completely sealed with no heat exchange allowed would be considered which type of system?

<p>Isolated system (C)</p> Signup and view all the answers

A system's boundary is best described as:

<p>All of the above (D)</p> Signup and view all the answers

What type of system is a coffee cup that is open to the air?

<p>Open system (C)</p> Signup and view all the answers

Consider a closed system like a sealed thermos flask. Which of the following can occur across its boundary?

<p>Only heat transfer (A)</p> Signup and view all the answers

Which of the following is NOT an accurate description of a thermodynamic system?

<p>It always has a fixed and rigid boundary. (A)</p> Signup and view all the answers

Which of the following is NOT an assumption of the ideal gas model?

<p>Ideal gas molecules undergo inelastic collisions with the walls of the container. (C)</p> Signup and view all the answers

What characteristic distinguishes extensive properties from intensive properties?

<p>Extensive properties are additive in nature, while intensive properties are not. (C)</p> Signup and view all the answers

In a two-phase system, what condition defines phase equilibrium?

<p>The mass of each phase remains constant over time. (B)</p> Signup and view all the answers

Why is the ideal gas model considered a simplification of real gas behavior?

<p>The ideal gas model neglects the interactions between gas molecules, which are present in real gases. (D)</p> Signup and view all the answers

Which of the following is an example of an intensive property?

<p>Density (B)</p> Signup and view all the answers

What is the primary reason for using the ideal gas model to study gases?

<p>The ideal gas model simplifies complex calculations by ignoring intermolecular forces. (D)</p> Signup and view all the answers

Which of the following is NOT considered a thermodynamic property?

<p>Velocity (C)</p> Signup and view all the answers

A system is considered to be in chemical equilibrium when:

<p>The chemical composition of the system does not change over time. (C)</p> Signup and view all the answers

According to Boyle's Law, what happens to the volume of a gas if the pressure is tripled while keeping the temperature constant?

<p>The volume is reduced to one-third. (D)</p> Signup and view all the answers

Which law describes the relationship between the pressure of a gas and its absolute temperature when the volume is kept constant?

<p>Gay-Lussac's Law (D)</p> Signup and view all the answers

What is the relationship between temperature and heat energy flow?

<p>Heat energy flows from a hotter body to a colder body. (A)</p> Signup and view all the answers

What is the main difference between extensive and intensive properties?

<p>Extensive properties depend on the quantity of matter, while intensive properties do not. (A)</p> Signup and view all the answers

Which of these temperature scales is recognized as the international standard for scientific temperature measurement?

<p>Kelvin (K) (B)</p> Signup and view all the answers

What is the relationship between the Celsius and Kelvin temperature scales?

<p>The Kelvin scale is obtained by shifting the Celsius scale by -273.15°. (A)</p> Signup and view all the answers

Which of the following is NOT a general use temperature scale?

<p>Rankine (°R) (B)</p> Signup and view all the answers

A thermodynamic process where no heat is exchanged between the system and its surroundings is called:

<p>Adiabatic process (D)</p> Signup and view all the answers

Which of the following is NOT a characteristic of a closed system?

<p>Can exchange both mass and energy with surroundings (A)</p> Signup and view all the answers

A system is said to be in thermal equilibrium when:

<p>Its temperature is constant throughout the system. (D)</p> Signup and view all the answers

Which of the following is a state function?

<p>Pressure (A), Volume (B)</p> Signup and view all the answers

In an isochoric process:

<p>There is no change in volume. (A)</p> Signup and view all the answers

Which of these processes is NOT a reversible process?

<p>Adiabatic (B)</p> Signup and view all the answers

What is the relationship between the amount of substance (n) and the volume (V) for an ideal gas at constant temperature and pressure?

<p>n is directly proportional to V. (D)</p> Signup and view all the answers

Which of the following statements BEST describes the relationship between state variables and state functions?

<p>State functions are always state variables. (A)</p> Signup and view all the answers

In the context of Charles's Law, what does the constant 'k' represent?

<p>The ratio of the volume of the gas to its temperature. (B)</p> Signup and view all the answers

What is the significance of the Kelvin scale in Charles's Law?

<p>It allows for the calculation of the volume of a gas at absolute zero. (B)</p> Signup and view all the answers

What is the molar fraction (Xi) of a component in a gas mixture?

<p>The number of moles of the component divided by the total number of moles in the mixture. (B)</p> Signup and view all the answers

How is the average molar mass of a gas mixture calculated?

<p>It is the weighted average of the molar masses of each component based on their molar fractions. (B)</p> Signup and view all the answers

Which of the following is NOT true of an ideal mixture?

<p>The components of the mixture have a strong chemical attraction for each other. (C)</p> Signup and view all the answers

What is the relationship between the partial pressure of a component (Pi) and its molar fraction (Xi) in a mixture?

<p>They are directly proportional. (C)</p> Signup and view all the answers

What is the relationship between the total pressure of a gas mixture, the volume of the mixture, and the total number of moles of gas in the mixture?

<p>The total pressure is inversely proportional to the volume but directly proportional to the number of moles. (B)</p> Signup and view all the answers

According to Dalton's Law, how is the total pressure of a gas mixture (PTotal) calculated?

<p>By adding the partial pressures of all the components in the mixture. (A)</p> Signup and view all the answers

Flashcards

Isolated System

A thermodynamic system where no mass or energy is exchanged with the environment.

Open System

A thermodynamic system that can exchange both mass and energy with its surroundings.

Closed System

A thermodynamic system that can exchange energy but not mass with its surroundings.

State Variables

Measurable properties of a system required to describe its state, such as pressure, temperature, or volume.

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State Function

A property that does not depend on the path taken, such as internal energy or enthalpy.

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Path Function

A property that depends on the path taken to reach a specific state, like work or heat.

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Adiabatic Process

A thermodynamic process with no heat exchange between the system and its surroundings.

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Thermal Equilibrium

A state when the temperature remains constant throughout the system and no net heat flow occurs.

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Thermodynamics

A branch of chemistry that studies heat flow.

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Thermodynamic System

A specific portion of matter defined for analysis.

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Surroundings

Everything outside the system that affects it.

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Boundary

A closed surface defining the limits of a system.

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Examples of Systems

Specific instances like balloons, flasks, and humans.

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Mechanical Equilibrium

A state where pressure does not vary at any point in the system.

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Chemical Equilibrium

A condition where the chemical composition of a system remains constant over time.

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Phase Equilibrium

Occurs in a two-phase system when the mass of each phase stabilizes at an equilibrium level.

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Thermodynamic Properties

Characteristics of a system that help describe its state, can be extensive or intensive.

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Intensive Properties

Properties independent of a system’s size, such as temperature and pressure.

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Extensive Properties

Properties that depend on system size, like mass and volume, and are additive.

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Ideal Gas Model

A theoretical model to simplify the understanding of gas behavior under certain conditions.

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Assumptions of Ideal Gas

Four key assumptions about ideal gases: point-like molecules, random motion, elastic collisions, no intermolecular forces.

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Kelvin scale

A temperature scale starting at absolute zero, where molecular motion stops.

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Charles's Law

States that the volume of a gas is directly proportional to its temperature in Kelvin.

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Ideal gas mixture

A gas mixture where particles have only elastic collisions and no interactions.

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Molar fraction

The ratio of the amount of a specific component to the total amount of all components in a mixture.

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Average molar mass of a mixture

The weighted average of the molar masses of the components in a gas mixture.

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Volumic mass

The mass per unit volume of a gas mixture.

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Dalton's Law

The total pressure of a gas mixture equals the sum of the partial pressures of each gas.

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Ideal Gas Law

PV = nRT describes the relationship between pressure, volume, and temperature of gas.

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Boyle's Law

Volume of gas inversely varies with pressure at constant temperature.

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Boyle's Law Equation

Mathematically, Boyle's law is expressed as P×V = k.

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Gay-Lussac Law

Pressure of gas directly varies with absolute temperature at constant volume.

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Gay-Lussac Law Equation

Mathematically expressed as P₁/T₁ = P₂/T₂.

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Charles's Law Equation

Expressed as V₁/T₁ = V₂/T₂.

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Universal Gas Constant (R)

R = 8.314 J/(K·mol) is the constant in the Ideal Gas Law.

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Definition of Temperature

Temperature measures hotness or coldness, indicating heat flow direction.

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Intensive Property

A property independent of the amount of matter, like temperature.

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Fahrenheit Scale

Temperature scale used mainly in the U.S., noted in degrees F (°F).

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Celsius Scale

Standard temperature scale in metric countries, noted in degrees C (°C).

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Study Notes

Thermodynamics Introduction

  • Thermodynamics is a branch of chemistry that studies the flow of heat.

Thermodynamic System

  • A thermodynamic system is a specific portion of matter with a defined boundary.
  • The boundary can be real or imaginary, fixed or deformable.
  • Surroundings are anything outside the system that influences its behavior.
  • A boundary is a closed surface around the system, allowing energy or mass to enter or exit.

Types of Systems

  • Isolated System: Cannot exchange energy or mass with its surroundings. Examples include a thermos flask.
  • Closed System: Can exchange energy but not mass. Examples include refrigerators, piston-cylinder assemblies.
  • Open System: Can exchange both energy and mass. Examples include a steam turbine, a pot of water boiling in an open vessel.

State Variables

  • They are measurable properties of a system.
  • Examples include pressure (P), temperature (T), volume (V), and amount of substance (n).
  • At least two independent state variables are needed to describe a system's state.

State Function

  • A state function's value is independent of the path taken to reach that state.
  • Path functions depend on the path taken.

Thermodynamic Processes

  • A thermodynamic process is an energy shift within a system, correlating with changes in pressure, volume and internal energy.
  • Examples include:
    • Adiabatic: No heat transfer.
    • Isochoric: No change in volume.
    • Isobaric: No change in pressure.
    • Isothermal: No change in temperature.

Thermodynamic Equilibrium

  • All properties of a system remain constant.
  • When isolated, no change occurs in the value of its attributes.
  • Thermal equilibrium: Constant temperature throughout the system.
  • Mechanical equilibrium: No pressure variation in the system.
  • Chemical equilibrium: System's composition stays constant over time.
  • Phase equilibrium: Mass is at an equilibrium level in systems with multiple phases.

Thermodynamic Properties

  • Intensive properties are independent of the system's size (mass), examples are temperature, pressure and density.
  • Extensive properties depend on the system's size (mass), examples are volume, total energy, and mass

Ideal Gas Model

  • An idealized representation of gases, neglecting intermolecular forces.
  • Assumptions include:
    • Point-like molecules.
    • Random motion.
    • Elastic collisions.

Ideal Gas Law

  • PV = nRT where:
    • P = pressure
    • V = volume
    • n = number of moles
    • R = ideal gas constant
    • T = absolute temperature

Dalton's Law of Partial Pressures

  • Total pressure of a gas mixture equals the sum of partial pressures of individual gases.

Clapeyron Diagram

  • A diagram showing various thermodynamic processes.

Temperature

  • A measure of hotness or coldness.
  • Three common scales: Fahrenheit, Celsius and Kelvin.
  • Kelvin is the absolute scale (zero Kelvin is absolute zero)

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