Thermochemistry (Calorimetry)

Thermochemistry

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