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| Front-side | Reverse-side |
|---|---|
| An amount of heat dQ absorveb by a body causes a rise dT in its temperature given by | dQ = CdT, where C is heat capacity. |
| An equation of state f(p,v,t)=0 describes a surface in (pvt) space. A reversible transformation can be represented by a continuous path _ the surface; an irreversible transformation can be represented cannot. | On |
| Definition: adiabatic process | a process which proceeds without transfer of heat |
| Definition: Carnot Cycle | PV cycle bounded by two isotherms and two adiabatic lines |
| Definition: Extensive quantities | Quantities proportional to the amount of matter present |
| Definition: intensive quantities | Quantities independent of the amount of matter present |
| Entropy, in terms of dS | dS = dQ/T |
| Equation: Helmholz free energy | A = U – TS |
| First law of thermodynamics | dU = dQ – dW U internal energy Q heat W == work done |
| Ideal gas law equation | PV=NkT k : Boltzmann’s constant T: Ideal gas temp, in K |
| In a PV diagram, the work done in one cycle of a closed path is… | ...the area enclosed by the path. |
| N (number of particles) = n(R/k), where n is _ and R/k is _ | Number of moles, and Avogadro’s Number |
| Second law of thermodynamics | "heat does not flow uphill" (there does not exist a thermodynamic transformation whose SOLE effect is to deliver heat from a reservoir of lower temperature to a reservoir of higher temperature) |
| Third law of Thermodynamics | The entropy of a system at absolute zero is a universal constant, which may be taken to be zero. |