The Laws of Thermodynamics
Two bodies in thermal equilibrium are at the same temperature
Energy can not be created or destroyed
ΔE=q+W
The total entropy of the universe (system and surroundings) must increase in every spontaneous process.
ΔS(total)=ΔS(system)+ΔS(surroundings) > 0
The entropy (s) of a pure, perfectly crystalline compound at T=0K is zero. (no disorder)
S(T=0)=0
Unit Conversions
Celsius to Kelvin
T(K)=T(C)+273.15
Symbol | Meaning | Additional |
|---|
T | Temperature | Average kinetic energy of all particles in a substance |
S | Entropy | The measure of a system’s thermal energy per unit temperature that is unavailable for doing useful work. As work is obtained from ordered molecular motion, it is also a measure of the molecular disorder of a system. |
E | Energy | |
Δ | Change in | |
q | Heat | |
W | Work | |
Kinetic Theory
All matter is made up of particles that are in constant, random motion (or maybe energy, unclear)
Specific Heat Capacity
The amount of energy needed to raise the temperature of 1kg by 1°C
Q=mcΔT
Symbol | Meaning | |
|---|
Δ | change in | |
Q | energy transferred | |
m | mass of water | |
c | specific heat capacity | |
T | Temperature | |
Thermal Equilibrium
When two objects are in thermal equilibrium, there is no net flow of heat between them.
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