||Heat capacity and calorimetry are defined and explained. The use of calorimetry to measure heat capacity is described.
||The heat capacity of an entire calorimeter system is determined.
|Heat Capacity of a Calorimeter
||Specific heat capacity is defined and explained. The calorimeter system is divided into components, in this example the calorimeter itself and the water in the calorimeter. A heat balance equation is written for the calorimeter system.
||The heat capacity of the calorimeter is determined.
|Specific Heat Capacity of Ethanol
||The heat balance equation is written for a calorimeter containing ethanol. A graphical strategy is described for analyzing calorimetric data to simultaneously determine both the heat capacity of the calorimeter and the specific heat capacity of ethanol.
||The heat capacity of the calorimeter and the specific heat capacity of ethanol are determined.
|Specific Heat Capacity of Copper
||In this calorimetry experiment, the components do not all have the same initial temperature. The mathematical handling of this situation is explained.
||In the first experiment, the heat capacity of the calorimeter is determined using a metal (iron) with a known specific heat capacity. In the second experiment, the specific heat capacity of copper is determined.
|Heat of Solution of Ammonium Nitrate
||In this experiment, a chemical reaction serves as a source of heat in the heat balance equation. The molar enthalpy of reaction is defined and explained.
||The molar heat of solution of ammonium nitrate is determined.
|Heat of Neutralization
||The neutralization reaction is explained. There are two reactants in the neutralization reaction; thus the limiting reactant must be identified in order to determine the molar enthalpy of neutralization.
||The molar enthalpy of neutralization is determined.
|Heat of Solution of Sulfuric Acid
||The nonideal loss and gain of heat during a calorimetry experiment is discussed. A graphical strategy for experimentally compensating for heat loss or gain is explained.
||The heating or cooling rates of the calorimeter before and after an experiment are determined graphically. The molar enthalpy of solution of sulfuric acid is determined.
|Heat of Combustion of Methane
||The combustion reaction for methane is explained and used to calculated the standard molar enthalpy of formation of methane.
||The molar enthalpy of methane is determined and used to determine the standard molar enthalpy of formation of methane. The amount of methane that undergoes combustion is determined using the pressure of methan and the ideal gas law.
|Heat of Solution of Calcium Hydroxide
||Strategies are discussed for studying systems in which two chemical reactions occur simultaneously.
||The molar enthalpy of solution of calcium hydroxide is determined. Nonideal heat loss/gain is modeled graphically.