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Energy
The capacity to work or transfer heat.
Work
The energy used to cause an object with mass to move against a force.
Heat
The energy used to cause the temperature of an object to increase.
Joules (J)
The SI base unit of energy.
Kinetic Energy (EK)
The energy of motion.
Thermal Energy
The internal energy of an object based on its temperature, associated with the kinetic energy of the object.
Potential Energy
Energy that is stored; includes forms like electrostatic and chemical energy.
First Law of Thermodynamics
States that energy is conserved in any process; it cannot be created or destroyed.
System
The substances or objects being studied.
Surroundings
Everything outside the system.
Internal Energy (E)
The sum of the kinetic and all potential energies of a substance or object.
Exothermic Reaction
A reaction where the system loses energy, producing heat and transferring it to the surroundings.
Endothermic Reaction
A reaction where the system gains energy, absorbing heat from the surroundings.
Enthalpy Diagrams
Visual representations showing the change in enthalpy during a reaction or process.
Kinetic Energy Formula
The kinetic energy of an object can be calculated using the formula EK = ½ mv².
Thermochemistry
A field of thermodynamics that examines the energy changes in chemical reactions.
Potential Energy Diagrams
Diagrams that show the change in energy from reactants to products in a chemical reaction.
State Function
Property of substance determined by its condition and not how it became in that state
Change in Enthalpy
Constant change of pressure in internal energy
Enthalpy
Measure of energy in thermodynamic system
Constant Pressure Calorimeter
Pressure is same as atmospheric pressure and amount of heat transferred is equal to change in enthalpy
Constant Volume Calorimeter
Measures heat released or absorbed during chemical reaction that occurs at constant volume
Electrostatic Potential Energy
Interaction between two charged objects
Chemical Energy
Energy stored in substances due to arrangement of atoms
Temperature
Average Kinetic Energy of particles in a substance.
Open System
Exchange both energy and matter within surroundings
Closed System
Exchanges only energy within surroundings, not matter
Isolated Systems
Does not exchange either energy or matter within system
Coffee Cup Calorimeter
Activation Energy
Minimum energy needed for successful collision
What affects rate of reaction
Changing temperature of reactants
Changing concentration of reactants
Changing physical state of reactants
Adding catalyst
Activated Complex
collides with enough energy to form a complex that can form products
Concentration
increases number of reactant particles and collisions in a given volume
Physical State
Increasing surface area will increase number of available molecules to collide with
Catalysts
Increases number of successful collisions by decreasing amount of energy required during each collision
Biological Catalyst
Enzymes that control rate of reactions in all living things
Reaction Mechanism
step-by-step sequence of elementary reactions by which overall chemical process occurs
Elementary Reactions
one--step reactions, occur in a single event or collision
Reaction Intermediate
produced in earlier step but consumed in a later step
Unimolecular reactions
reaction that involves single reactant molecule
Bimolecular reactions
reactions that involves two reactant molecules
Termolecular reactions
involves three reactant molecules but are very rare
Hess’ Law
Independent to number of steps taken
Supports conservation of energy because it covers initial and final
