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kinetic e
energy of motion
ex; flowing water
potential e
stored energy due to its position or state
ex: chemical bonds
thermal e
energy associated with temp of an object
chemical e
energy stored in chemical bonds
released during combustion
change in internal energy
ΔE=Efinal - Einitial
ΔE(-): EFinal < Einitial
if initial e is higher, e was released from the system into the surroundings
ΔE(+): EFinal > Einitial
If final e is higher e was absorbed from the surroundings into the system
Formula for energy of a system
ΔEsystem= q + w
q= heat added or released from system
w= work done on or by the system
if q is positive vs negative
positive: heat absorbed
negative: heat released
if w is positive or negative
positive: work done on the system
negative: work done by the system
heat capacity formula
amount of heat needed to change the temperature by a specific amount
q = C * ΔT where q is the heat added, C is the heat capacity (J/degrees Celcius), and ΔT is the change in temperature.
specific heat capacity
the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius
q = m x Cs x ΔT
q= heat in J either released - or absorbed +
m= mass in g
Cs= specific heat (J/g degrees Celc.)
ΔT= temperature change in degrees Celc. + heat absorbed - heat released
specific heat capacity of water
4.18 J/g °C
