Laws of Thermodynamics-Report(1234).pptx

# Laws of Thermodynamics - Report

## Introduction
The laws of thermodynamics form a foundational framework in physics, defining the principles governing energy transformations and the behavior of systems. These laws are pivotal in various fields such as physics, chemistry, engineering, and even biology, playing a crucial role in understanding how energy transfers and transformations occur in natural and artificial processes. This report delves into the four fundamental laws of thermodynamics, exploring their implications, applications, and the principles underlying each law.

## Zeroth Law of Thermodynamics

### Statement
The Zeroth Law of Thermodynamics establishes the concept of temperature and thermal equilibrium. It states:
"If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other."

### Explanation
This law essentially means that if system A is in thermal equilibrium with system B, and system B is in thermal equilibrium with system C, then system A and system C must also be in thermal equilibrium. This transitive property forms the basis for the definition of temperature. It implies that temperature is a fundamental and measurable property that can indicate whether systems are in thermal equilibrium.

### Implications
The Zeroth Law allows for the creation and use of thermometers. By bringing a thermometer into thermal equilibrium with a system, the temperature of the system can be measured. It provides a basis for temperature scales and ensures that temperature is a consistent and reliable measure of thermal energy.

### Applications
- **Temperature Measurement**: Enables the use of thermometers to measure temperature.
- **Calibration of Instruments**: Ensures that temperature scales and instruments are standardized.
- **Thermal Equilibrium Studies**: Forms the basis for studying and understanding thermal equilibrium in various systems.

## First Law of Thermodynamics

### Statement
The First Law of Thermodynamics, also known as the Law of Energy Conservation, states:
"Energy cannot be created or destroyed in an isolated system. The total energy of an isolated system is constant, although energy can be transformed from one form to another."

### Explanation
This law emphasizes the conservation of energy. It asserts that the change in the internal energy of a system equals the heat added to the system minus the work done by the system on its surroundings. Mathematically, it is expressed as:
\[ \Delta U = Q - W \]
where:
- \(\Delta U\) is the change in internal energy of the system.
- \(Q\) is the heat added to the system.
- \(W\) is the work done by the system.

### Implications
The First Law implies that energy transformations within a system, such as from thermal to mechanical energy or chemical energy to electrical energy, do not result in a net gain or loss of energy. Instead, energy is merely converted from one form to another.

### Applications
- **Heat Engines**: Design

1. Laws of Thermodynamics Biochemistry Gabriel M. Alvarez Austin T. Escol BSED-SCI SC22

2. What is Thermodynamics? Thermodynamics is a branch of physics that deals with heat, work, and temperature, and their relation to energy, entropy, and the physical properties of matter and radiation.

3. First Law of Thermodynamics 01

4. First Law of Thermodynamics Energy is always conserved; it cannot be created or destroyed.

5. Enthalpy − heat transfer between the system and its surroundings under constant pressure − it is a guide to whether a reaction is likely to proceed − it is not the only factor that determines whether a reaction proceeds. Enthalpy is the measure of total heat present in the thermodynamic system where the pressure is constant.

6. Spontaneous Processes Occur without outside intervention. Have a definite direction. - The reverse process is not spontaneous. Temperature has an impact on spontaneity. - Ex: Ice melting or forming; hot metal cooling at room temp.

7. Reversible & Irreversible Reversible: System changes state and can be restored by reversing original process. Irreversible: System changes state and must take a different path to restore to original state

8. Second Law of Thermodynamics 02

9. Second Law of Thermodynamics The entropy of the universe always increases in a spontaneous process and remains unchanged in an equilibrium process.

10. Entropy (S) A measure of randomness or disorder S = entropy in J/ K·mole Increasing disorder or increasing randomness is increasing entropy. Three types of movement can lead to an increase in randomness.

11. Molecules exhibit several types of motion: Translational – Movement of the entire molecule from one place to another. Vibrational – Periodic motion of atoms within a molecule. Rotational – Rotation of the molecule on about an axis or rotation about pi bonds.

12. Entropy (S) Entropy is a state function Change in entropy of a system; Δ S = S final - S initial Depends only on initial and final states, and not the pathway. Negative (-) Δ S indicates a more ordered state (think: < disorder or - disorder) Positive (+) Δ S = less ordered state (think: > disorder or + disorder)

13. Entropy (S) Processes that lead to an increase in Entropy When a solid melts. When a solid dissolves in solution. When a solid or liquid becomes a gas. When the temperature of a substance increases. When a gaseous reaction produces more molecules. If no net change in # of gas molecules, can be + or -, but small.

14. Third Law of Thermodynamics 03

15. Third Law of Thermodynamics States that the entropy of a perfect crystalline substance is zero at absolute zero.

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