introduction to Thermodynamics

2. INTRODUCTION TO THERMODYNAMICS
Thermodynamics began as a way to evaluate the potential of steam
engines to provide work.
Thermodynamics deals with those systems irrespective of their
atomic and molecular properties and doesn't relates microscopic
properties with macroscopic properties. For example
temperature, pressure, volume and entropy.

3. INTRODUCTION TO THERMODYNAMICS
Macroscopic refers to bulk systems that are readily
observable.
Microscopic refers to regions that are smaller than those
observable by the naked eye, but which contain
sufficient numbers of molecules.

4. INTRODUCTION TO THERMODYNAMICS
Measured quantities for a thermodynamic process are
Pressure (P)
Volume (V)
Temperature (T)
Number of moles of a substance (n)

5. INTRODUCTION TO THERMODYNAMICS
The universe is all of space.
While the laws of thermodynamics could be applied to the universe,
it is usually more convenient to break that space up into:
1. System
2. Surroundings
The system is the region of space that is of interest in the problem.
The surroundings is all of the space which is not contained within
the system.

6. INTRODUCTION TO THERMODYNAMICS
The system is enclosed by a boundary.
system can be open, closed, or isolated.

7. INTRODUCTION TO THERMODYNAMICS
An open system is one where both mass and energy may
cross the boundaries of the systems. Examples: pipes,
turbines
A closed system is one where only energy may cross the
boundaries (that is, mass cannot cross the boundary).
Examples:
an oven, this classroom
An isolated system is one which does not allow mass or
energy to cross its boundaries.

8. INTRODUCTION TO THERMODYNAMICS
The thermodynamic state of a system is the condition in
which it is currently in. Knowing the state fixes all of
the system's intensive properties.
A process is the act of bringing a system from one state
to another.