Chemistry Lecture on Calorimetry and Heat Transfer

This set of flashcards covers key vocabulary terms and concepts discussed in the chemistry lecture on calorimetry, heat transfer, and stoichiometry.

Calorimetry

A technique used to measure the heat absorbed or released during a chemical reaction or physical change.

Molarity

A measure of concentration representing the number of moles of solute per liter of solution.

Limiting Reactant

The reactant that is completely consumed in a chemical reaction, limiting the amount of product formed.

Specific Heat

The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.

First Law of Thermodynamics

Energy cannot be created or destroyed, only transformed from one form to another.

Exothermic Reaction

A reaction that releases heat to the surroundings.

Endothermic Reaction

A reaction that absorbs heat from the surroundings.

Thermal Equilibrium

The state in which two substances in contact no longer transfer heat, resulting in equal temperatures.

q = mcΔT

The formula used to calculate the heat change in a substance, where q = heat energy, m = mass, c = specific heat, and ΔT = change in temperature.

Coffee Cup Calorimetry

An experimental setup used to measure heat changes at constant pressure, usually involving a Styrofoam cup as an insulator.

ΔH (Enthalpy Change)

The amount of heat content lost or gained during a chemical reaction, measured in joules or kilojoules per mole.