Heat Capacity and Calorimetry

Calorimetry

The measurement of the quantity of heat exchanged during a chemical or physical process.

Specific Heat Capacity (c)

The amount of energy needed to raise the temperature of one gram of a substance by1^C (or 1^K).

Units for Specific Heat

J/(gC) or J(g\cK).

Heat (q)

A form of energy that flows between two samples of matter because of their difference in temperature.

Heat Transfer Equation

q = mc/Delta T (Heat = mass *specific heat * change in temp).

Delta T (Delta T)

Final Temperature - Initial Temperature.

Law of Conservation of Energy (Calorimetry)

Heat lost by the system = Heat gained by the surroundings (-qlost = qgained).

Molar Heat Capacity (C_m)

The amount of energy needed to raise one mole of a substance by one degree Celsius.

High Specific Heat Capacity

Requires a lot of energy to change temperature (e.g., Water); heats up and cools down slowly.

Low Specific Heat Capacity

Requires little energy to change temperature (e.g., Metals); heats up and cools down quickly.

Exothermic Dissolution

Temperature of the mixture increases; energy is released to the solution (surroundings).

Endothermic Dissolution

Temperature of the mixture decreases; energy is absorbed from the solution (surroundings).

Energy Conversion (Calories)

1 calorie = 4.184 Joules.

Calorimeter

An insulated device used to measure the absorption or release of heat in chemical or physical processes.