Segment E: Calorimetry Lab
Segment E: Calorimetry Lab
The students perform the coffee cup calorimetry experiment, gathering data to determine what compounds work best to create hot and cold packs.
Obtain, evaluate, and communicate information about the chemical and physical properties of matter resulting from the ability of atoms to form bonds.
Develop a model to illustrate the release or absorption of energy (endothermic or exothermic) from a chemical reaction system depends upon the changes in total bond energy.
Obtain, evaluate, and communicate information about how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.
Plan and carry out an investigation to determine that a new chemical has been formed by identifying indicators of a chemical reaction (e.g., precipitate formation, gas evolution, color change, water production, and changes in energy to the system).
Obtain, evaluate, and communicate information about the Kinetic Molecular Theory to model atomic and molecular motion in chemical and physical processes.
Plan and carry out an investigation to calculate the amount of heat absorbed or released by chemical or physical processes.
Obtain, evaluate, and communicate information to explain transformations and flow of energy within a system.
Plan and carry out investigations to describe how molecular motion relates to thermal energy changes in terms of conduction, convection, and radiation.
Analyze and interpret specific heat data to justify the selection of a material for a practical application (e.g., insulators and cooking vessels).
Analyze and interpret data to explain the flow of energy during phase changes using heating/cooling curves.
absolute zero - the temperature at which all molecular motion stops and entropy is zero.
calorimetry - a method of measuring the quantity of heat transferred in a process.
chemical thermodynamics - the study of energy changes that accompany chemical reactions or physical changes in the state of matter; also known as thermochemistry.
endothermic - describes a process that takes in or absorbs energy from its surroundings.
enthalpy - a thermodynamic quantity equivalent to the total heat content of a system.
entropy - the measurement of energy dispersal.
exothermic - describes a process that produces or gives off energy to its surroundings.
first law of thermondynamics - the amount of energy in the universe is a constant. Energy can be transferred from one substance to another or transformed into other forms of energy, but it cannot be created or destroyed.
heat - the transfer of energy from a warmer object to a cooler object; also known as thermal energy.
joule - the SI unit of measure for energy, abbreviated J.
second law of thermodynamics - energy always disperses from a more usable form of energy to a less usable form.
specific heat capacity - the heat needed to raise the temperature of one gram of a substance by one degree Celcius.
surroundings - everything around the system, i.e. air, water, packaging, etc...
system - the chemical reaction or physical process being monitored.
temperature - a measurement of the average kinetic energy or molecular movement in an object or system.
thermal conductivity - a measure of the ability of a material to transfer heat.
third law of thermodynamics - the entropy of a system at absolute zero is zero.
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