PV Diagrams. THERMODYNAMICS. A Generic Thermodynamic Process. Start with some internal energy due to a starting T, P, and V. Heat is added or taken away, work is done on or by the gas. You end up with an new amount of internal energy, with new T, P, and V.
Start with some internal energy due to a starting T, P, and V
Heat is added or taken away, work is done on or by the gas
You end up with an new amount of internal energy, with new T, P, and V
A cylinder is tube and a piston is a solid cylindrical device that exactly fits into the cylinder so that there is very little gap between the piston and the side of the cylinder.
If you add heat to the cylinder, the gas expands and pushes the piston upwards, doing work on it. We make a major assumption – that the pressure stays constant. This is actually reasonable. The area on the top of the piston doesn’t change, so the force exerted on it by the atmosphere is constant. When the piston rises to some position, the force pushing down is still the same, so the force inside pushing up must be the same as well. Since this force comes from the pressure, the pressure must still be the same.
What a P-V Diagram would look like
F = PA
The area under the curve is equal to the work that is done.
This is also true for any graph of pressure vs volume. The area under the curve is always equal to the work.
note that in a cyclic process the gas is taken through a cycle of operations and brought back to the original state. If the cycle is clockwise as in the present case, work is done by the gas. So the work is negative. Further, the area enclosed by the closed curve gives the work done during one cycle.
This means that V is zero. If V is zero, then the work must also be zero.
What the P-V diagram looks like
During this process heat can enter and leave the gas but the total energy in the gas will not change. ∆U=ZERO
What the P-V diagram looks like
In an adiabatic process, heat is neither added or taken away from the system.
This means that the first law can be simplified:
What this means is that work is done by the system at the expense of internal energy.
1. The system can be insulated so that heat can neither enter nor leave. Joule’s “heat equivalent” experiment was adiabatic. The tub of water was insulated so the water would not absorb heat from its surroundings. Instead the work done on the water by the paddles increased the internal energy of the system - the temperature went up.
2. The other way to have an adiabatic process (this is actually called a “near adiabatic process”) is to have it happen very quickly. The process happens so fast that there is no time for heat to be transferred.
1. a gas that is adiabatically expanded will lose internal energy (U ) and become cooler.
2. a gas that is adiabatically compressed will gain U and become warmer.
Compress air from your lungs by puckering your lips. When it leaves your mouth, it expands adiabatically, thus it cools
One mole of monatomic ideal gas is enclosed under a frictionless piston. A series of processes occur, and eventually the state of the gas returns to its initial state with a P-V diagram as shown below. Answer the following in terms of P0, V0, and R.
1. Find the temperature at each vertex.
2. Find the change in internal energy for each process.
3. Find the work by the gas done for each process.
Use the gas law to find the temperatures at A, B, C
Since the internal energy depends only on temperature, the change in internal energy for each process depends only on the temperature difference that occurs during the process:
To find the work done by the gas, find the area under each segment, remembering the sign convention.