| Question | Answer |
| Heat Transfer | Q = mcΔT
c= specific heat |
| Phase Change | Q = mL
L= latent heat ( fusion or vaporization) |
| Linear Expansion | Δl = α lo ΔT
α = coefficient of linear expansion
lo = original length |
| Volume Expansion | ΔV = β Vo ΔT
β = Coefficient of volume
Vo = original volume |
| Rate of Heat Transfer | H = Q/t or H = (k A ΔT) / L
k = thermal conductivity
A = Cross sectional area
L = Distance Between ends |
| Ideal Gas Law | PV= nRT
P = pressure
V= Volume
n= number of moles
R= Universal Gas Constant
T = Temperature |
| Average Molecular Kinetic Energy | K = 3/2 k T
k = Boltzman's Constant |
| Root-mean-squared velocity | v rms = √(3 k T / m) |
| 0th Law of Thermodynamics | When A & B are in equilibrium with C. A & B are in Equilibrium with each other. |
| 1st law of Thermodynamics | ΔU = ΔQ + W
U= Internal Energy
Q = Heat Transferred to a System
W= Work done on the gas ( if work done by the gas it is negative) |
| Work done by or on a gas | W = -PΔV or W = PΔV |
| Change in internal energy | ΔU = 3/2 NkΔT |
| Efficiency | e = W/ QH
W = Output
QH = Input |
| Heat Input | QH = W + QL
QL = Heat that flows out |
| Ideal Efficiency | e ideal = TH - TL / TH
TH = High Temp
TL = Low Temp |
| Change in Entropy | ΔS = Q/T
Q= Heat added |
| 2nd Law of Thermodynamics | The total entropy of any system plus that of its environment increases as a result of any natural process
ΔS > 0
ΔS = ΔSs + ΔS env |
| 3rd Law of Thermodynamics | The entropy of a pure perfect crystal is zero (0) at zero Kelvin (0° K). |
