Thermochemistry
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50 flashcards covering key terms and definitions related to thermochemistry.
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46 Terms
Thermochemistry
The study of the relationships between chemistry and energy.
Internal Energy (E)
The sum of the kinetic and potential energies of all particles in a system.
Conservation of Energy
Energy can neither be created nor destroyed, only transformed.
System
The part of the universe being studied, such as chemicals in a beaker.
Surroundings
Everything outside the system that can exchange energy with it.
Open System
Exchanges both energy and matter with its surroundings.
Closed System
Exchanges energy but not matter with its surroundings.
Isolated System
No exchange of energy or matter occurs with the surroundings.
Joule (J)
The SI unit of energy, defined as 1 kg·m²/s².
Calorie (cal)
The amount of energy required to raise the temperature of 1 g of water by 1°C.
Kilowatt-hour (kWh)
A large unit of energy commonly used for home energy costs.
Heat (q)
The energy exchanged between a system and its surroundings due to a temperature difference.
Work (w)
The energy exchange resulting when a force moves an object through a distance.
First Law of Thermodynamics
The change in internal energy is the sum of heat transferred and work done.
Enthalpy (H)
The total energy of a system, defined as the sum of internal energy and the product of pressure and volume.
Specific Heat Capacity (Cs)
The amount of heat required to raise the temperature of 1 g of a substance by 1°C.
Heat Transfer
The movement of thermal energy from hotter to cooler matter.
Calorimetry
The measurement of heat exchange during chemical reactions.
Thermal Equilibrium
The state reached when two substances at different temperatures equalize in temperature.
Pressure-Volume Work
Work done by a system during a volume change against an external pressure.
Exothermic Reaction
A chemical reaction that releases heat, indicated by a negative change in enthalpy.
Endothermic Reaction
A chemical reaction that absorbs heat, indicated by a positive change in enthalpy.
Thermochemical Equation
An equation that shows the heat absorbed or released based on the stoichiometric amounts of reactants or products.
Standard Enthalpy of Formation (ΔH°f)
The change in enthalpy when one mole of a substance is formed from its constituent elements.
Hess's Law
The change in enthalpy for a stepwise process is the sum of the enthalpy changes of the steps.
Change in Internal Energy (ΔE)
The difference in internal energy between products and reactants.
Heat Capacity (C)
The amount of heat required to change a system’s temperature by 1°C.
Molar Heat Capacity
The amount of heat required to raise the temperature of one mole of a substance by 1°C.
Kinetic Energy
Energy due to the motion of particles.
Potential Energy
Energy stored due to the position of particles.
Calorimeter
An instrument used to measure the heat absorbed or released during a chemical reaction.
Isothermal Process
A process that occurs at constant temperature.
Adiabatic Process
A process in which no heat is exchanged with the surroundings.
Thermal Energy
The total kinetic energy of particles in a substance.
Temperature (T)
A measure of the average kinetic energy of particles in a sample.
Specific Heat (c)
The amount of heat needed to raise the temperature of a unit mass of a substance by one degree.
Chemical Bonding
The force that holds atoms together in a compound.
Reaction Coordinate
A hypothetical parameter that represents the progress of a chemical reaction.
Heat of Reaction (ΔHrxn)
The change in enthalpy during a chemical reaction.
Stoichiometric Coefficients
Numbers that represent the proportions of reactants and products in a chemical reaction.
Thermochemical Tables
Reference tables that provide standard enthalpies of formation for different substances.
Change in Enthalpy (ΔH)
The difference in enthalpy between the products and reactants of a reaction.
System Expansion
The increase in volume of a system, often associated with energy changes.
System Contraction
The decrease in volume of a system, often associated with energy changes.
Joule's Law
The law stating that the internal energy of an ideal gas depends only on its temperature.
Latent Heat
The heat energy required for a phase change in a substance without changing its temperature.