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joule
SI unit for energy?
calorie (cal)
common unit of energy used for heat?
The amount of energy required to raise the temperature of 1 g of water by 1 degree C
thermal energy
the sum of all the kinetic energy of the molecules in a system
temperature
proportional to the average of the kinetic energy of the molecules in a system
conservation of energy
energy itself can neither be created nor destroyed
yes
Can energy change forms? (kinetic to potential, etc)
yes
Can energy be transferred from one system to another?
state function
a physical property for which the value does not depend on the path taken to get that value
state function
is energy a state function or a path function?
path function
a physical property for which the value depends on the path taken to get that value
system
a collection of atoms, molecules, or both, of interest
surroundings
anything that isn’t part of the system
positive
is change in energy positive or negative when energy enters a system?
negative
is change in energy positive or negative when energy leaves a system?
work
force applied to move an object over a distance
pressure volume work
the energy associated with the change in size of a gas-filled container
heat
the transfer of energy resulting from a temperature difference between two objects
high to low
which direction does heat flow?
heat capacity
the amount of heat required to raise the temperature of an object by 1 degree C
specific heat capacity
heat capacity divided by a substance’s mass
thermodynamics
the branch of science that studies changes in energyt
thermochemistry
the specific application of the study of energy in chemical processes
first law of thermodynamics
all changes in energy are done by way of heat or work
calorimetry
an experimental technique where the heat absorbed/released by the surroundings is measured in order to determine the heat released/absorbed by the system
bomb calorimeter
an instrument that can be used to measure energy changes arising from combustion reactions under constant volume conditions
enthalpy
the heat released or absorbed by a system under constant pressure, symbolized by delta h
thermochemical equation
a chemical equation that indicates how much heat is required or produced during the course of a chemical reaction
endothermic
a process that absorbs heat (positive delta h)
HEAT ENTERS
exothermic
process that releases heat (negative delta h)
HEAT EXITS
Hess’s Law
Law that states that the net change of enthalpy of a series of chemical reactions in sequence is equal to the sum of the enthalpy changes in each individual reaction
standard enthalpies of formation
the enthalpy change associated with forming a compound from its elements in their standard states
bond energy
the amount of energy required to break a particular bond
