Section 1
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Specific heat for liquid H2O
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Section 1
(50 cards)
Specific heat for liquid H2O
4.184 J/g . K
Radiation
Transfer of energy by electromagnetic waves e.g. Sun keeps earth warm
thermodynamics
a branch of physics concerned with heat and temperature and their relation to energy and work. It defines macroscopic variables, such as internal energy, entropy, and pressure, that partly describe a body of matter or radiation.
plasma
an ionized gas consisting of positive ions and free electrons in proportions resulting in more or less no overall electric charge, typically at low pressures (as in the upper atmosphere and in fluorescent lamps) or at very high temperatures (as in stars and nuclear fusion reactors).
First law of thermodynamics
The change in the total internal energy of a system is equal to the amount of energy transferred in the form of heat to the system, minus the amount of energy transferred from the system in the form of work
heat engine
a device for producing motive power from heat, such as a gasoline engine or steam engine.
Four special types of thermodynamic systems in which a given variable is held constant
Isothermal, Adiabatic, Isobaric, Isobaric, Isovolumetric
Heat of transformation
During a phase change, heat energy causes changes in PE and energy distribution, but not KE. No change in temp
Heat of transformation equation
q= amount of heat gained or lost from substance m= mass L= heat of transformation
conduction
the process by which heat or electricity is directly transmitted through a substance when there is a difference of temperature or of electrical potential between adjoining regions, without movement of the material.
absolute zero
the lowest temperature that is theoretically possible, at which the motion of particles that constitutes heat would be minimal.
Thermodynamics
Flow of energy in the universe, as the flow relates to work, heat, entropy, and the different forms of energy
Closed systems
System capable of exchanging energy, but not matter, with the surrounding e.g. gas in vessels with movable pistons
Zeroth law of thermodynamics
Objects are in thermal equilibrium when they are at the same temperature, transitive property in thermal systems (a=b, b=c, a=c)
Heat gained or lost by an object
q= heat gained or lost by an object m= mass c= specific heat of substance delta T= change in temp
Convection
Transfer of heat by the physical motion of a fluid over a material e.g. Fans circulate hot air inside oven
Entropy
Measure of how much energy has spread out or how spread out energy has become
Carnot cycle
an ideal reversible closed thermodynamic cycle; back to it's original state
deposition
when an object goes from a gas straight to solid, without going through a liquid phase
heat
a form of energy associated with the movement of atoms and molecules in any material.
Carnot engine
most efficient heat engine, uses two isothermal and two adiabatic processes
Specific heat (c) of a substance
The amount of heat energy required to raise one gram of a substance by one degree Celsius or one unit Kelvin
radiation
the emission of energy as electromagnetic waves or as moving subatomic particles, especially high-energy particles that cause ionization.
Adiabatic process
No heat is exchanged
Isothermal process
T is constant, change in internal energy= 0
Isovolumetric (isochoric) process
V is constant, work done on or by system = 0
Thermal expansion
delta L= change in length alpha= coefficient of linear expansion L= original length delta T= change in temperature
Heat
The transfer of thermal energy from a hotter object(higher temp/energy) to a colder object (lower temp/energy)
Second law of thermodynamics
In a closed system, energy will spontaneously and irreversibly go from being localized to being spread out
internal energy
the energy in a system arising from the relative positions and interactions of its parts.
Thermal equilibrium
No heat flows between two objects in thermal contact
Kelvin to Celsius equation
Fahrenheit to Celsius equation
convection
the movement caused within a fluid by the tendency of hotter and therefore less dense material to rise, and colder, denser material to sink under the influence of gravity, which consequently results in the transfer of heat.
First law of thermodynamics equation
delta U= internal energy Q= heat W= work
Conduction
Direct transfer of energy from molecule to molecule through molecular collisions e.g. metal pan to chicken, gases are poor conductors
Isolated systems
System not capable of exchanging energy or matter with their surrounding; total change in internal energy is zero e.g. bomb calorimeter
State functions
Thermodynamic properties that are a function of only the current equilibrium state of a system e.g. pressure, density, temperature, volume, enthalpy, internal energy, Gibbs free energy, entropy
isothermal
a change of a system, in which the temperature remains constant
Entropy and heat
delta S= change in entorpy Q rev= heat gained or lost in reversible process T= temperature
Three means by which heat can transfer energy
Conduction, Convection, Radiation
Open systems
Systems can exchange both matter and energy with the environment e.g. Boiling pot of water
entropy
lack of order or predictability; gradual decline into disorder. // a thermodynamic quantity representing the unavailability of a system's thermal energy for conversion into mechanical work, often interpreted as the degree of disorder or randomness in the system.
Temperature
A physical property of matter that relates the average kinetic energy of the particles in a substance
sublimation
a transition of a substance directly from the solid to the gas phase without passing through the intermediate liquid phase
Isobaric process
P is constant
adiabatic
relating to or denoting a process or condition in which heat does not enter or leave the system concerned.
mole
the SI unit of amount of substance, equal to the quantity containing as many elementary units as there are atoms in 0.012 kg of carbon-12.
Entropy of universe
This total entropy of the universe is always increasing
isochoric
a thermodynamic process during which the volume of the closed system undergoing such a process remains constant.
Section 2
(7 cards)