Thermodynamics and Energy

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Questions and Answers

Which of the following best describes thermochemistry?

  • The study of nuclear reactions and radioactive decay.
  • The study of the relationships between chemical reactions and energy changes involving heat. (correct)
  • The study of the motion of objects at high speeds.
  • The study of the properties of matter at absolute zero.

A bicyclist is coasting on a flat road and begins to go up a hill without pedaling. What happens to the bicyclist's kinetic and potential energy?

  • Kinetic energy increases, potential energy decreases.
  • Kinetic energy decreases, potential energy increases. (correct)
  • Both kinetic and potential energy decrease.
  • Both kinetic and potential energy increase.

Which of the following is the correct formula for kinetic energy?

  • $E_k = mv$
  • $E_k = \frac{1}{2}mv$
  • $E_k = mv^2$
  • $E_k = \frac{1}{2}mv^2$ (correct)

Electrostatic potential energy between two charged particles is affected by which of the following factors?

<p>Both the charge of the particles and the distance between them. (C)</p> Signup and view all the answers

According to the formula for electrostatic potential energy, what happens to the energy ($E_{el}$) as the distance (d) between two oppositely charged particles increases?

<p>$E_{el}$ approaches zero. (D)</p> Signup and view all the answers

What is the process that converts chemical energy to thermal energy?

<p>Burning (A)</p> Signup and view all the answers

Which unit is equivalent to the SI unit of energy, the joule (J)?

<p>kg⋅m²/s² (A)</p> Signup and view all the answers

If 1 calorie is exactly 4.184 J, how many joules are in a nutritional Calorie (1 Cal)?

<p>4184 J (B)</p> Signup and view all the answers

In a chemical reaction within a flask, what constitutes the 'system' according to thermodynamics?

<p>Both the reactants and products. (C)</p> Signup and view all the answers

A student performs a reaction in an open beaker. Identify the type of system present.

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

Consider a reaction occurring within a closed cylinder fitted with a piston. Energy can be exchanged with the surroundings as heat or work, but matter cannot enter or leave. What type of system is this?

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

A perfectly sealed, insulated container prevents any exchange of heat or matter with its surroundings. What kind of system is this?

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

A scientist studies a reaction in a bomb calorimeter, a closed system, and observes a significant temperature increase. What can be concluded about the reaction?

<p>The reaction is exothermic. (C)</p> Signup and view all the answers

In thermodynamics, what distinguishes an 'open system' from a 'closed system'?

<p>An open system can exchange both matter and energy with its surroundings, while a closed system can only exchange energy. (A)</p> Signup and view all the answers

Concerning human beings, which type of thermodynamic system, is most accurate?

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

What is the definition of 'work' in the context of energy transfer?

<p>The energy transferred when a force makes an object move a distance. (B)</p> Signup and view all the answers

How is 'heat' defined in thermochemistry?

<p>The energy transferred from a hotter object to a colder one. (A)</p> Signup and view all the answers

Using the formula $w = F \times d$, if a force of 50 N is applied to move an object 10 meters, how much work is done?

<p>500 J (B)</p> Signup and view all the answers

A bowler lifts a 5.4-kg bowling ball from the ground to a height of 1.6 m. Assuming the work done to raise the ball is converted to potential energy, what happens to the ball's potential energy as it is raised?

<p>The potential energy increases. (C)</p> Signup and view all the answers

Three objects move at different speeds. Object A (500-kg) moves at 100 km/h, Object B (1,000-kg) moves at 50 km/h and Object C (1,500 kg) moves at 30 km/h. Which object has the greatest kinetic energy?

<p>Object A (A)</p> Signup and view all the answers

What determines whether a system is classified as open, closed, or isolated?

<p>The system's ability to exchange energy and matter with the surroundings. (B)</p> Signup and view all the answers

Why is a boiling pot of water on a stove considered an open system?

<p>It exchanges both matter (water vapor) and energy (heat) with the surroundings. (C)</p> Signup and view all the answers

Which of the following best describes an isolated system?

<p>A system that cannot exchange either energy or matter with its surroundings. (C)</p> Signup and view all the answers

What is the primary difference between kinetic and potential energy?

<p>Kinetic energy is energy in motion, while potential energy is stored energy. (C)</p> Signup and view all the answers

What happens to the electrostatic potential energy when two positively charged particles move closer to each other?

<p>It increases. (C)</p> Signup and view all the answers

How does the concept of 'work' relate to the change in potential energy of an object?

<p>Work is the energy transferred to change an object's potential energy. (B)</p> Signup and view all the answers

Which statement accurately describes the relationship between heat and temperature?

<p>Heat is the energy transferred, while temperature is a measure of the average kinetic energy of molecules. (B)</p> Signup and view all the answers

Which of the following is essential to classify a thermodynamic system as 'isolated'?

<p>The system exchanges neither mass nor energy with its surroundings. (B)</p> Signup and view all the answers

A chemical reaction occurs in a solution where the system absorbs heat from the surroundings. Which of the following statements is true?

<p>The reaction is endothermic. (B)</p> Signup and view all the answers

Flashcards

Thermodynamics

The study of energy and its transformations.

Thermochemistry

The branch of thermodynamics dealing with the relationships between chemical reactions and energy changes involving heat.

Energy

The capacity to do work or transfer heat.

Kinetic Energy

Energy due to motion.

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Potential Energy

Energy due to position relative to other objects; stored energy from attractions and repulsions.

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Electrostatic Potential Energy

A form of potential energy that arises from the interactions between charged particles.

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Chemical Energy

Potential energy stored in the arrangements of atoms in a fuel.

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Thermal Energy

Energy associated with temperature.

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Joule (J)

The SI unit for energy.

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Calorie (cal)

The amount of energy required to raise the temperature of 1g of water from 14.5 to 15.5 °C; now defined in terms of the joule.

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System

The limited and well-defined part of the universe under study or investigation.

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Surroundings

Everything else (other than the system).

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Open System

A system that can exchange matter and energy with the surroundings.

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Closed System

A system that can exchange energy but not matter with the surroundings.

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Isolated System

A system that cannot exchange matter nor energy with the surroundings.

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Work

Energy transferred when a force moves an object.

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Heat

Energy transferred from a hotter object to a colder one.

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Force

A push or pull exerted on an object.

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Study Notes

  • Thermodynamics is the study of energy and its transformations, stemming from the Greek words "thérme" (heat) and "dy'namis" (power).
  • Thermochemistry is the area of thermodynamics concerning the relationships between chemical reactions and the energy changes, specifically those involving heat.
  • Energy is the capacity to do work or transfer heat.
  • Kinetic energy is the energy resulting from motion.

Potential Energy

  • Potential energy is energy due to an object's position relative to other objects and can be considered stored energy.
  • Electrostatic potential energy (Eel) arises from interactions between charged particles.
  • Eel = kQ1Q2/d, where k is a constant (8.99 x10^9 J-m/C^2), Q represents electrical charges, and d is the distance between them.
  • A coulomb (C) is the unit of electrical charge, and a joule (J) is the unit of energy.
  • For charged particles at finite separation distances, Eel is positive for like charges (repulsion) and negative for opposite charges (attraction).
  • As particles move farther apart, their electrostatic potential energy approaches zero.
  • Chemical energy is the potential energy stored in the arrangement of atoms in a fuel.
  • Thermal energy is the energy associated with temperature.

Units of Energy

  • The SI unit for energy is the joule (J), named in honor of James Joule (1818-1889).
  • 1 J equals 1 kgm²/s.
  • Kilojoules (kJ) are often more practical due to the small size of a joule.
  • A calorie (cal) was originally defined as the energy to raise 1 g of water from 14.5 to 15.5 °C.
  • 1 cal = 4.184 J (exactly).
  • A nutritional Calorie (C) is equal to 1000 cal or 1 kcal.

Thermodynamic Systems

  • The system is the specific part of the universe under study.
  • The surroundings include everything outside the system.
  • In a chemical reaction, reactants and products are the system.
  • The container and everything beyond it form the surroundings.

Types of Systems

  • An open system exchanges both matter and energy with its surroundings.
  • A closed system exchanges energy but not matter with the surroundings.
  • An isolated system exchanges neither matter nor energy with its surroundings.

Work and Heat

  • Work (w) occurs when energy is transferred as a force moves an object.
  • A force is any push or pull exerted on an object.
  • The magnitude of work is the product of the force (F) and the distance (d) over which the object moves.
  • Work = F x d
  • Heat is energy transferred from a hotter object to a colder one.

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