The work done by a gas when expanding can be calculated by:
☐ the area under the curve representing the
process in the P-T diagram
☑ the area under the curve representing the
process in the P-V diagram
☐ the area under the curve representing the
process in the T-V diagram
The first law of thermodynamics is a statement of:
☑ conservation of energy
☐ conservation of (regular) momentum
☐ conservation of angular momentum
☐ conservation of mass
The second law of thermodynamics says for a heat engine:
☐ You get more work energy out than you put in as heat
☐ You get the same work energy out as you put in as heat
☑ You get less work energy out than you put in as heat
Ralph is confused because in class Dr. Colton mentioned that when you
compress gases, they tend to heat up. (Think of bicycle pumps.) Yet section 12.3
talks about "isothermal" processes where the temperature doesn't change. How are
such processes possible?? How can you compress a gas without its temperature
increasing?
Just take away some heat at the same time, by (for example) surrounding the gas with something cold.