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| Front-side | Reverse-side |
|---|---|
| 1st law of thermodynamics | change U= Q-W (work done by system) heat added TO system *Work done on system is negative |
| adiabatic | no heat transfer |
| conduction | contact |
| convection | movement in currents of fluids |
| elastic collision | energy conserved |
| heat | energy (Joules) transferred from hotter to colder objects. If no transfer of energy then NO HEAT!! Q |
| heat | transfer of energy—> allowed when there is a difference in temperature |
| heat equation Q= | mc (change in T) AND mL |
| ideal gas | particles are under low pressure and don’t interact much with each other, but interact with sides of container in elastic collisions |
| ideal gas law | PV=nRT—> used to make comparisions while keeping one element constant |
| internal energy (U) | PE + KE |
| isobaric | constant pressure |
| isochoric | constant V |
| isothermal | constant temperature |
| Pressure = | Force/Area |
| Pressure constant Gas law | V1/T1 = V2/T2 |
| PV diagram what does area represent? | Work |
| radiation | transfers with infared, above a fire |
| temperature | measures translational kinetic energy |
| Temperature Constant | (P1)(V2) = (P2)(V2) |
| Volume Constant | P1/T2 = P2/T2 |