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12 Cards in this Set
- Front
- Back
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Isothermic Process
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Temperature is constant
change in thermal energy = 0 Horizontal line on PV Diagram |
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Isobaric Process
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Pressure is constant
Internal energy is constant (system heats up) |
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Isochoric Process
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Volume is constant
No work being done by the system since there is no area under the PV diagram. eErtical line on PV diagram. |
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Adiabatic Process
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No heat in or out of system
PV graph is steeper than isothermic graph |
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Ideal Gas Law
PV=nRT |
P=Pressure (Pa)
V=Volume (m^3) n=# of moles R=universal gas constant 8.314 J/(mole*K) T= Temperature (K) |
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State Variables
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temperature, volume, pressure
# of moles, thermal energy, and entropy |
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Pressure Equation
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P=F/A
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Change in Entropy Equation
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ΔS=Q/T
Q= Heat flowing in (Joules) T=temp (K) |
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Power Equation
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P=W/ΔT
W= Watt T= Time Interval |
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Change of Thermal Energy Equation
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ΔE=Q+T
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Entropy Equation
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S=k*ln(Ώ)
k= Boltzmann's constant: (1.38×10−23 J/K) Ώ= # of microstates |
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ϵ=W(out)/Q(in)
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Efficiency = work output/Heat transferred in (K)
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