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Chemistry: Chapter 17.2 Measuring and Expressing Enthalpy Changes
Terms in this set (9)
The precise measurement of the heat flow into or out of a system for chemical and physical processes.
How is the heat released by the related to the heat absorbed in a system? (and vice versa)
In calorimetry, the heat released by the system is equal to the heat absorbed by its surroundings.
Conversely, the heat absorbed by a system is equal to the heat released by its surroundings.
The insulated device used to measure the absorption or release of heat in chemical or physical processes.
The heat content of a system at constant pressure. Because the reactions in the textbook occur at constant pressure.
(The terms heat and enthalpy change are used interchangeably. q = ∆H)
How can the enthalpy change be written in a chemical equation?
In a chemical equation, the enthalpy change for the reaction can be written as either a reactant or a product.
A chemical equation that includes the enthalpy change.
Chemistry problems involving enthalpy changes are similar to stoichiometry problems.
(The amount of heat released or absorbed during a reaction depends on the number of moles of the reactants involved)
Heat of reaction
The enthalpy change for the chemical equation exactly as written.
Other than the moles of reactants, what else must be stated in an equation?
Physical states of the reactants and products in a thermochemical reaction must also be stated.
(The amount of heat to vaporize liquid requires more than to vaporize gas)
Heat of combustion
The heat of reaction for the complete burning of one mole of a substance
Like other heats of reaction, heats of combustion are reported as the enthalpy changes when the reaction are carried out at 101.3 kPa of pressure and the reactants and products are in their physical states at 25ºC.
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