Section 1
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chemical thermodynamics
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Cards (56)
Section 1
(50 cards)
chemical thermodynamics
the area of chemistry that deals with energy relationships
Enthalpy of reaction
heat of reaction
vibrational motion
the atoms in the molecule move periodically toward and away from one another
Exothermic
Releases heat
Fuel Value
the energy released when one gram of any substance is combusted
Enthalpy
heat; internal energy plus the product of pressure and volume
Standard enthalpy change
The total heat produced or absorbed by a system when reactants in their standard states change to products in their standard states under STP conditions.
Renewable energy sources
Are resources that can be replaced in a relatively short amount of time. This includes: hydroelectric, solar, geothermal, wind, biomass, and possibly nuclear fusion.
number of degrees of freedom
forms of motion available to the atoms
Pressure-Volume work
the work involved in the expansion or compression of a gas
first law of thermodynamics
energy is conserved
rotational motion
the molecule spins about an axis
Molar Heat capacity
Heat capacity per mol of substance
First Law of Thermodynamics
Sum of all Kinetic and Potential energies of the components of the system
ideal engine
an engine with the highest possible efficiency
entropy
the extent of randomness in a system or the extent to which energy is distributed among the various motions of the molecules of the system
Joule
SI unit for energy
Bomb calorimeter
measures caloric content of biological materials (sample is burned, heat released)
dispersion of energy
caused by an entropy increase which increases the number of ways the positions and energies of the molecules can be distributed throughout the system
irreversible process
a process that cannot simply be reversed to restore the system and its surroundings to their original states
Calorie
energy required to raise the temperature of 1 gram of water from 14.5 degrees Celsius to 15.5 degrees Celsuis i calorie = 4.184 joules
Enthalpy of formation
the enthalpy change for a reaction in which one mole of a compound is formed from its elements in their standard states
Standard enthalpy of formation
The change in Enthalpy that accompanies the formation of 1 mole of a compound from its elements with all substances in their standard states.
Specific heat
Amount of heat required to raise one gram of a substance by 1 degree Celsius or Kelvin; heat capacity.
broader distribution
the higher the temperature, the faster the molecules move and the more kinetic energy they possess, the hotter the system, the more broader distribution of molecular speeds
Fossil Fuels
A hydrocarbon deposit, such as petroleum, coal, or natural gas, derived from living matter of a previous geologic time and used for fuel.
isothermal process
the expansion of an ideal gas at constant temperature
translational motion
the entire molecule can move in one direction, which is the simple motion we visualize for an ideal particle and see in a macroscopic object like a thrown baseball
Energy
the capacity to do work or transfer heat
statistical thermodynamics
uses the tools of statistics and probability to link the microscopic and macroscopic worlds
second law of thermodynamics
any irreversible process results in an increase in the entropy of the universe, whereas any reversible process results in no change in the entropy of the universe
Work
energy used to cause an object to move against a force
spontaneous process
a process that proceeds on its own without any outside assistance
ThermoChemistry
relationships between chemical reactions and energy changes that involve heat
Endothermic
Absorbs heat
state functions
properties that define a state and do not depend on how we reach that state examples: temperature, internal energy, and enthalpy
State Function
a property of a system that is determined by specifying the systems conditions
Kinetic Energy
energy of motion
Standard State
The standard thermodynamic conditions (often 1 atm or 1 bar and 25 degrees Celsius) chosen for substances when listing or comparing thermodynamic date.
microstate
a single possible arrangement of the positions and kinetic energies of the molecules when the molecules are in a specific thermodynamic state
Calorimeter
an insulated device used to measure the absorption or release of heat in chemical or physical processes
Heat
energy used to cause the temperature of a system to fluctuate
Heat capacity
The amount of energy needed to raise the temperature of substance by one degree Celsius or Kelvin
Calorimetry
The measurement of heat flow (into or out of a system) as the result of a chemical reaction or physical process.
reversible process
a specific way in which a system changes its state, the system can be restored to its original condition with no net change to either the system or its surroundings
nonspontaneous process
the reverse of any spontaneous process
System
the reaction being observed
Thermodynamics
The study of energy and its transformations
Surroundings
everything that is not directly involved in the chemical reaction taking place. i.e: a thermometer measuring the temperature change of an exothermic neutralization between HCl and NaOH
Potential Energy
energy stored
Section 2
(6 cards)