Thermochemistry Concept Map
Energy
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Potential Energy
stored energy
SUBSETS
Chemical Energy
Elastic Energy
Nuclear Energy
Gravitational Energy
Kinetic Energy
SUBSETS
energy of movement
Thermal Energy
Mechanical Energy
Electrical Energy
Magnetic Energy
Sound Energy
Light Energy
System
change
exothermic
endothermic
in the lab
macroscopic
temperature
releasing heat
absorbing heat
greater ΔH
smaller ΔH
experimental
system
surroundings
everything outside of system
whatever is being studied, you define system
open
closed
isolated
mass transfer & heat transfer
only heat transfer
no mass transfer or heat transfer
Heat Equation
HEAT vs TEMPERATURE
form of thermal energy
flows from hotter region to cooler region
degree of hotness and coldness of a body
total kinetic energy of all particles
extensive property
Joules (J) & calories (cal)
calorimeter
related to average kinetic energy
intensive property
Kelvin (K) & Celcius (C)
thermometer
Q = mcΔT
Q = heat (cal or J)
m = mass (g)
c = specific heat
ΔT = change in temperature
J/g ^degree^ C
quantity of energy it takes to raise the temp of 1 g of a material by 1 degree C
