Chapter 4 heat and temp psci – Flashcards

heat movement from any higher temperature region

high specific heat

3 times as much heat

less heat

solid

fluid

vacuum

radiation

might stay the same

latent heat

any temperature

constant temperature

latent heat of vaporization

second

no, the total entropy of the universe increases

freeze at a uniform low temperature

one btu is the amount of energy (or heat) needed to increase the temp of one pound of water 1 degree Fahrenheit

the metric unit of heat; defined as the amount of energy (or heat) needed to increase the temp of 1 gram of water 1 degree celsius

uses the freezing point and boiling point of water at normal atmospheric pressure, but it has different arbitrarily assigned values. The celsius scale identifies the freezing point of water as 0 degrees and the boiling point as 100 degrees celsius

a thermodynamic measure of disorder- (disorder means randomized, spread out, no patterns, arrangement..etc) Whenever energy freely transforms from one form to another, the direction of transformation is toward a state of greater disorder, and therefore toward on of greater entropy IOW- the greater the disorder, the higher the entropy "the total entropy in the universe continually increases" - The entropy of a system can decrease (more order- order means patterns and coherent arrangements), for example, when a heat pump cools and condenses the random, chaotically moving water vapor molecules into the more ordered state of liquid water When the energy source for the production, transmission, and use of electrical energy is considered, however, the 'total' entropy increases.

the total potential and kinetic energy go an everyday sized object

90

the energy supplied to a thermodynamic system in the form of heat, minus the work done by the system, is equal to the change in internal energy. Heat engine example: as the engine cycles to the original state of internal energy (U2-U1=0), all the external work accomplished must be equal to all the heat absorbed in the cycle. The heat supplied to the engine from a high temp (QH) is partly converted to work (W), and the rest is rejected in the lower temp exhaust (QL). The work accomplished is therefore the difference in the heat input and output (QH-QL) so the work accomplished represents the heat used: W- J(QH-Q1) J (joules) is the mechanical equivalence of heat you can increase the internal energy (produce heat) as long as you supply mechanical energy (do work). The first law of thermodynamics states that the conversion of work to heat is reversible, meaning heat can be changed to work

is concerned with internal energy (U), the total internal potential and kinetic energies of molecules making up a substance, such as the gases in the simple heat engine (a device that converts heat into mechanical energy). The variables of temperature, gas, pressure, volume, heat. etc, characterize the total internal energy, which is called the 'state' of the system; any two systems that have the same values of variables that characterize internal energy as said to be in the same state The state can be changed in two ways: 1- by heat flowing into (Qin) /out (Q out) of it, 2- by work (W out) being done on the system (W in).

the measure of the internal energy that has been absorbed or transferred from one body to another

the total kinetic and potential energy of the molecules of an object

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the amount of energy (or heat) needed to increase the temp of 1 kilogram of water 1 degree celsius

def- the heat involved in a solid-liquid phase change in melting or freezing. consider the changes that occur when ice is subjected to a constant source of heat. (p.100 figure 4.18) When the temp reaches the melting point (0 degrees), it stops increasing as the ice begins to melt. More and more liquid water appears as the ice melts, but the temp remains at 0 degree celsius even though heat is still being added at a constant rate. It takes a certain amount of heat to melt all the ice. Finally, when all the ice is completely melted, the temp increases again at a constant rate between melting and boiling points. Then at a constant temp the addition of heat produces another phase change, from liquid to gas. The quantity of heat involved in this phase changed is used in doing the work of breaking the molecule to molecule bonds in the solid, making a liquid with molecules that are now free to move about and rollover one another. Since the quantity of heat (Q) is absorbed without a temp change, it is called the latent heat of fusion (Lf)

potential energy This energy is "hidden" or latent since heat was absorbed but a temp increase did not take place. This same potential energy is given up when the molecules of the liquid return to the solid state. a melting solid absorbs energy and a freezing liquid releases the same amount of energy, warming the surroundings. Thus, you put ice in a cooler because the melting ice absorbs the latent heat of fusion from the beverage cans, cooling them. for water, the latent heat of fusion is 80.0 cal/g. This means that every gram of ice that melts in your cooler absorbs 80.0 cal of heat. Every gram of water that freezes releases 80.0 cal. The total heat involved in a solid-liquid phase change depends on the mass of the substance involved.

def- "the heat involved in a liquid-gas phase change where there is evaporation and condensation" --It is the energy gained by the gas molecules as work is done in overcoming molecular forces. This, escaping molecules absorb energy from the surroundings, and condensing gas/vapor releases this exact same amount of energy. for water the latent heat of vaporization is 540.0 cal/g. This means that every gram of water vapor that condenses on your bathroom mirror releases 540.0 cal, which watts the bathroom. The total heating depend on how much water vapor condensed.

If a molecule of water that has an exceptionally high energy is near the surface and is headed in the righ direction, it may overcome the attractive forces of the other water molecules and escape the liquid to become a gas. This process is called evaporation. It reduces a volume of liquid water as molecules leave the liquid state to become water vapor in the atmosphere. Note: molecules that evaporate move about in all directions, and some will return, striking the liquid surface

The same forces that the molecules escaped from earlier capture the molecules, returning them to the liquid state. This process is called condensation. It is the opposite of evaporation-- in evaporate, more molecules are leaving the liquid state than are returning. In condensation, more molecules are returning to the liquid state than are leaving. When the condensation rate equals the evaporation rate, the air above the liquid is said to be 'saturated' Note: there is no net energy flow when the air is saturated, since the heat carried away by evaporate is returned by condensation. This is why you fan your face when you are hot. The moving ir from the fanning action pushes away water molecules from the air near your skin, preventing the adjacent air from becoming saturated, thus increasing the rate of evaporation.

the smallest particle of a compound or gaseous element that can exist and still retain the characteristic properties of that substance.

when a solid, liquid, of gas changes from one phase to another= phase change it absorbs or releases a quantity of heat that is not associated with temperature change. Since the quantity of heat associated with a ohase change is not associated with a temp change, it is called 'latent heat' latent heat= "hidden" energy of phase hanges, which is energy (heat) that goes into or comes out of internal potential energy

1-solid-liquid 2-liquid- gas 3-solid-gas --Solid -liquid phase change occurs when a solid melts to a liquid or a liquid freezes to a solid. Ice melting and water freezing to ice are examples of phase change and its two directions. They both occur at a temp called "the freezing point" or the "melting point" depending on the direction of the phase change. In either case, the freezing and melting points are the same temp --liquid gas phase change also occurs in two diff directions. The temp at which a liquid boils and changes to a gas (or vapor) is called the "boiling point." The temp at which gas or vapor changes back to liquid is called the "condensation point."(boiling and condensation points are same temp)- other conditions liquids may turn to gas phase change is evaporation and condensation. solid-gas on other card

solid-gas phase change takes...a phase change that takes a solid directly to a gas or vapor is called "sublimation" mothballs and dry ice (solid CO2) are common examples of materials that undergo sublimation; frozen water or common ice also sublimates under certain conditions ex: ice cubes in a freezer become smaller with time as a result of sublimation. The frost that forms in a freezer, on the other hand is an example of a solid-gas phase change that takes place in the other direction. In this case, water vapor forms the frost without going through the liquid state, a solid gas phase change that takes place in an opposite direction to sublimation. ex: consider the changes that occur when ice is subjected to a constant source of heat. (p.100 figure 4.18) When the temp reaches the melting point (0 degrees), it stops increasing as the ice begins to melt. More and more liquid water appears as the ice melts, but the temp remains at 0 degree celsius even though heat is still being added at a constant rate. It takes a certain amount of heat to melt all the ice. Finally, when all the ice is completely melted, the temp increases again at a constant rate between melting and boiling points.

heat flows from objects with a higher temp to objects with a cooler temp. IOW- if you want heat to flow from a colder region to a warmer one, you must 'cause' it to do so by using energy (work) ex: heat pump (moves heat in the opposite direction) Never flows from cold to hot unless work is done on the system or energy is added from another source as in heat pumps and air conditioners

1- the observable external energy 2- the internal energy of the molecules, or particles that make up an object ex: a ball has kinetic energy after it is thrown through the air, and the entire system of particles making up the ball acts as a single massive particle as the ball moves.

1-a coherent motion- where the move together 2-an incoherent motion- chaotic motion of individual particles. -Work on an object is associated with coherent motion, while heating an object is associated with its internal incoherent motion.

the amount of coherent motion

high quality is energy with high order and coherence; can be easily converted to work low quality is energy with less order and coherence; less able to do work

transformation of high quality energy to low quality energy. energy becomes less and less available to do work. Eventually the upgraded mechanical energy will degrade to heat, and the increased heat will disperse through the processes of heat flow.

the amount of heat needed to increase the temp of 1 gram of a substance 1 degree celsius

measure of the average kinetic energy of the molecules making up the substance

-Increase the temperature of the liquid Average molecular KE increases More molecules have sufficient KE to escape -Increase the surface area of the liquid exposed to the space above -Decrease the number of molecules of substance in gaseous phase in the space above Molecules in liquid phase are encouraged to repopulate space above -Decrease the overall pressure of all gases in the space above Pressure creates a force acting against molecules escaping liquid phase. Lower pressure lower force

the measure of internal energy that has been absorbed or transferred from one body to another. The process of increasing internal energy is called heating; the process of decreasing internal energy is called cooling.