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Thermochemistry (Calorimetry) in Chemistry Engineers 1.
Thermochemistry
heat changes during chemical reactions
Energy
the capacity to do work and produce heat
Kinetic Energy
energy of motion
Potential Energy
stored energy
Temperature
measure of kinetic energy/particles in motion of a substance
Heat
ENERGY that object gives or absorbs due to a temperature change
Exothermic
from system to surroundings, heat loss T1>T2
Endothermic
from surroundings to system, heat gained T1<T2
Heat (Q) unit
Joule (J)
Temperature (T) unit
Celsius (°C) or Kelvin (K) 1°C=273.15K
measure of TOTAL kinetic energy of all molecules in a substance
Heat (Q)
measure of the AVERAGE kinetic energy of all molecules in a substance
Temperature (T)
Heat Capacity [C]
heat/energy required to raise temp. to a unit degree
Specific Heat Capacity [c]
heat/energy required to raise the temp. of 1 gram of substance
formula for Heat (Q)
Q=m*c*(Tf-Ti)
Law of Conservation of Energy (heat)
Heat Loss = Heat Gained
Calorimetry
used to determine the amount of heat transferred during a chemical process.
Constant Pressure calorimeter
for non-combustion reactions
Constant Volume
for combustion reactions
formula for Heat of Combustion Enthalpy (deltaH combustion)
deltaH = -qfuel / moles of fuel
Note 
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