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energy
the capacity to do work
work
a directed energy change resulting from a process
kinetic energy
the energy produced by a moving object
radiant energy
solar energy
thermal energy
the energy associated with the random motion of atoms and molecules
chemical energy
stored within the structural units of chemical substances
potential energy
energy available by virtue of an object’s position
law of conservation of energy
the total quantity of energy in the universe is assumed constant
system
the specific part of the universe that is of interest to us
surroundings
the rest of the universe outside of the system
isolated system
cannot exchange mass or energy with the surroundings
closed system
can exchange energy
open system
can exchange mass and energy with the surroundings
exothermic process
any process that gives off heat (system→ surroundings)
endothermic process
any process that absorbs heat (surroundings→ system)
thermodynamics
the scientific study of the interconversion of heat and other kinds of energy
state of a system
the values of all relevant macroscopic properties (composition, energy, temperature, pressure, volume, mass, length); all are important because they can have an effect on the outcome of reactions
first law of thermodynamics
energy can be converted from one form to another, but cannot be created or destroyed
enthalpy
used to describe heat changes taking place at constant pressure
enthalpy of a reaction
the difference between the enthalpies of the products and the enthalpies of the reactants
thermochemical equation
show the enthalpy changes as well as the mass relationships; just like a regular equation but with a delta H term usually at the end
specific heat (sometimes c or s)
the amount of heat required to raise the temperature of one gram of the substance by one degree Celsius (J/gC)
heat capacity (C)
the amount of heat required to raise the temperature of a given quantity of the substance by one degree Celsius (J/C)
standard enthalpy of formation
the heat change that results when one mole of a compound is formed from its elements in their standard states (1 atm, 25C)
standard enthalpy of reaction
the enthalpy of a reaction carrued out at 1 atm and 25C
Hess’s Law
when reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
heat of solution
heat generated or absorbed when a certain amount of solute dissolves in a certain amount of solvent
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