Which of the following is th8b mbq; 1lln-re smallest unit of heat energy?

  The amount of heat nec 5icqk2wx, )6l x8kslwessary to raise the temperature of 1 gram of water by $1 \; ^{\circ}C$ is referred to as the

  The measure of the average kinetic energy of individual molecul z ef arxk7e-:3yl-yl+es is referred to asla fle e7xr k3+:yy-z-

  A cup of water is scooped up from a swimming pool of water. Cxw;1px49srp d2z-0h ua rvnj:ompare the temperature T and the internal energy U of the wrvx 0x;4nspwdj: r2-h azu91p ater, in both the cup and the swimming pool.

  The internal energy of a g1e3rh kg,1 c k8 1oz04siqo+mu0wltsn ideal gas depends on

  An ideal gas at STP i ozmx.ptw k: *1f*j3wbs first compressed until its volume is half the initial volume, and then it is allowed to expand until its pressure is halfz :mb.xkowp*wt 1f*j 3 the initial pressure. All of this is done while holding the temperature constant. If the initial internal energy of the gas is U, the final internal energy of the gas will be

  An ideal gas with internal enerq(ej4fc7mfmva;fp* 6gy U at $200 \; ^{\circ}C$ is heated to $400 \; ^{\circ}C$. Its internal energy then will be

  The reason ocean temperatures do not vary drastically : 5 5uk in; 9/zsmpdoi/vma4q6uc)ksqis that

  It is a well-known fact that water has a higher specific heat carb eve,g) huu u:11p:ipacity than iron. Now, consider equal masses of water and iron thu1ebg, 1v)rp:uue hi:at are initially in thermal equilibrium. The same amount of heat, 30 calories, is added to each. Which statement is true?

  A thermally isolated system is3 tq zyq9l ;v)io-x/t6z,awawku6u 4y made up of a hot piece of aluminum and a cold piece of copper; the alu/y6t 9iaq 6ztzkya u3-q;lo,x )uw w4vminum and the copper are in thermal contact. The specific heat capacity of aluminum is more than double that of copper. Which object experiences the greater magnitude gain or loss of heat during the time the system takes to reach thermal equilibrium?

  Phase changes occur

  The heat required to change a substance from the solid to the liquid state is r76xg5 e nihx4yeferr xe5iyn 4hg7x6ed to as the

  The heat required to change a substance from the ldr q gq.+fu.xq)ar79fiquid to the vapor state is referre7x)rf. . qa9ur+fg dqqd to as the

  If heat is added to a pure substance at a steady r r6j/f)3e1 ddhsivuq*ate,

  When a solid melts

  When a liquid freezenwb800 ;oq);dluk*wys7 gb 1q m9 hrkqs

  When a liquid evaporatesi t/2nipcj o hb1,q ylc/6vnn83 cbt,3

  When a vapor condensen8 ue r3f26nq p1d,quhs

  In a cloud formation, water vapor condenses into water dropletsmp+.09qi. g+bsf /g7kq e ghth which get bigger and bigger until it rains. This will cause the tempe.kf h/p70+q.bgh gegiq+9mts rature of the air in the clouds to

  Turning up the flame under a pan of b(sjvi1(w u;udk,j uq 1oiling water causes

  Equal masses of waterd m6,scx itew,la bz(bb( ;-dhc42n.g at $20 \; ^{\circ}C$ and $80 \; ^{\circ}C$ are mixed. What is the final temperature of the mixture?

  A chunk of ice ($T = -20 \; ^{\circ}C$) is added to a thermally insulated container of cold water ($T = 0 \; ^{\circ}C$). What happens in the container?

  The process whereby heat flows by means of molecular collily1+h2e 2vp b/leyyd* t. a2c-jvs eal*q0-fnsions is referred to as/ev- vq+fpl*l.syyal2b-he t 2nd2a yc01e* j

  By what primary heat transfer meta)bc;u f6 uw-4n j*pmchanism does one end of an iron bar become hot when the other end is placed ijb ) fc*uuta4 -nmpw;6n a flame?

  On a cold day, a piece of metal feels much c ,apxx1l)qc a3older to the touch than a piece of wood. This is due to the difference in which one of the following physical propertlca)13pxa, qx y?

  If you double the thickness of a wal0i8cokezd am ;hmb5(f8j+(lk l built from a homogeneous material, the rate of (e dimblf58;c8 a(kz0j +m ohkheat loss for a given temperature difference across the thickness will

  A layer of insulating material with t5u:vx(esg ddv ro007rs ds9d5hermal conductivity K is placed on a layer of another material of thermal conductivity 2K. The layers have equal thickness. What is the effective thermal co5d 79d5r0des x0vsvdgr sou(: nductivity of the composite sheet?

  The process whereby heat flows by the mass moveme*jaqr;z.y 1n vnt of molecules from one place tozq*1r. v an;yj another is referred to as

  By what primary heathfa; o2z6n bm0e+r 4hq transfer mechanism is a pot of water heated on a stove?

  Convection can occurxzv* ng q/. hx2w bc+/aaq71fd

  Which of the following best explains why sweating is imp *nu x5u3g wx5:fmidx.ortant to humans in maintaining suitabl5n3:fig5 * x dwm.xuxue body temperature?

  A spaceship is drifting in an envirtn5b3h clud8;onment where the acceleration of gravity is essentially zero. As the air on one side of the cabin is heated by an electric heater, what t8n3udbhc5; lis true about the convection currents caused by this heating?

  Consider two neighboring rectangular u g z7wjaed(vsfqjd0, gajimm,t,.:u0 7 45if houses built from the same materials. One of the houses has twice the length, width, and height of the other. Under identical climatic conditions, what would be true about the rate that heat would have to be supplied to maintain the same inside temperature on a colaf47j0,,jm7s i0eam:itqgjgu5 udw zdvf ( .,d day? Compared to the small house, the larger house would need heat supplied at

  If the absolute temperature of a radiatoryz/6( urn svii9q)t.w is doubled, by what factor does the raqv6yn. irt9w s)z/(iudiating power change?

  The process whereby heat flows in thd-0j a j *rhtx +ao98*thcm;g-lfgu0 ve absence of any medium is referred to as

  By what primary heat transfer mechanism does the Sun wau0z8j47y b; k7hgkdrb rm the Earth?

  1700 J of work is equivalent to hu3y m1k7ho-ireq a)g/ow much heat?

  16.5 kcal of heat issu(4m)ig a)imm euw e820l5pu equivalent to how much work?

  Gasoline yields $4.8 \times 10^{7} \; joules$ per kg when burned. The density of gasoline is approximately the same as that of water, and 1 gal = 3.8 L. How much energy does your car use on a trip of 100 mi if you get 25 mi per gallon?

  How much heat is needed to raise the temperature of 100 g of l6(c yf,z21edntj ( lbuead ($c = 0.11 \; kcal/kg \cdot ^{\circ}C$) by $15 \; ^{\circ}C$?

  If 40 kcal of heat is added to 2.0 kg of water, what is the resul2 nz0t5mgn lzpg w,,7fting temperature cha,,flgzn 7gnpw2m0 5z tnge?

  A 4.0-kg aluminum block ii **d1i9on*h jgm0nk-i j 9tyes originally at $10 \; ^{\circ}C$. If 160 kJ of heat is added to the block, what is its final temperature?

  150 kcal of heat raises the temperat inz . 0k;wr/bjl( ps9k2nd3xture of 2.0 kg of material by $400 ^{\circ}F$. What is the material's specific heat capacity?

  A person tries to heat up her bath water m2-4dxs6uu9ti x sua g4i:lh4 by adding 5.0 L of water at $80 \; ^{\circ}C$ to 60 L of water at $30 \; ^{\circ}C$. What is the final temperature of the water?

  A machine part consists of 0.10 kg of iron and 0.16 kg of copper. H9 3bvj4u +v* v1vpxzy-zi+mziow much heat is added to the *ziv+ +-z jmbpi31z u9vy4 xvvgear if the temperature increases by $35 \; ^{\circ}C$?

  50 g of lead ($c = 0.11 \; kcal/kg \cdot ^{\circ}C$) at $100 \; ^{\circ}C$ is put into 75 g of water at $0 \; ^{\circ}C$. What is the final temperature of the mixture?

  A 0.600-kg piece of metal is heatedsq2 n4abs kz-5nf.cfd m41 e:b to $100 \; ^{\circ}C$ and placed in an aluminum can of mass 0.200-kg which contains 0.500 kg of water initially at $17.3 \; ^{\circ}C$. The final equilibrium temperature of the mixture is $20.2 \; ^{\circ}C$, what is the specific heat of the metal?

  A 0.10-kg piece of copper, inicjrn8)6hr:z o tially at $95 \; ^{\circ}C$, is dropped into 0.20 kg of water contained in a 0.28-kg aluminum can; the water and aluminum are initially at $15 \; ^{\circ}C$. What is the final temperature of the system?

  If 50 g of material at a 2- jvv 0asdtv3s j9q),p5mieu::zww$100 \; ^{\circ}C$ is mixed with 100 g of water at $0 \; ^{\circ}C$, the final temperature is $40 \; ^{\circ}C$. What is the specific heat of the material?

  Two equal mass objects make up a system that is thermally isolated from nsn)u;b ngq3fyovw, otd: k 9p/sj;1 7its surro,u:;9;w 1/gnj)yp 7s vbto 3ofqndksnundings. One object has an initial temperature of $100 \; ^{\circ}C$ and the other has an initial temperature of $0 \; ^{\circ}C$. What is the equilibrium temperature of the system, assuming that no phase changes take place for either object? (The hot object has a specific heat capacity that is three times that of the cold object.)

  On his honeymoon, James Joule attempted to explore the relationships beeytt- s94u5s0fdb g .utween various forms of energy by measuring the rise of temperature of water which had fallen down a waterfall on Mount Blanc. What maximum temperature rise would one expect for a waterfall wiest9.f 0s t5d-g4yuub th a vertical drop of 20 m?

  The water flowing over Niagara Falls dr 4iqcx,-gsmkz 2f,z4sg2,g7h ndk s)oops a distance of 50 m. Assuming that all the gravitational energy is converted to thermal energy, b c2,g,k qm4hsgif4,)do2sn7 kx gz- zsy what temperature does the water rise?

  A 200-L electric water heater uses 2 kW. dt59 ,vs2j dzpyh yd3/Assuming no heat loss, how long would it take to heat water is2,h/ dyz 3yjt5 vd9dpn this tank from $23 \; ^{\circ}C$ to $75 \; ^{\circ}C$?

  A 5000-W heater is used to heat water. How long will it take to heat 20 k( pm,g2q0zwp 1 paqic;g of water f0mpp(pgq;,q 2zwa i1c rom $20 \; ^{\circ}C$ to $100 \; ^{\circ}C$?

  An aluminum kettle (8u7,/ (rq4odqoav,jybd; l md mass 1000 g, $c = 0.22 \; kcal/kg \cdot ^{\circ}C$) holds 400 g of pure water at $20 \; ^{\circ}C$. The kettle is placed on a 1000 W electric burner and heated to boiling. Assume that all the heat from the burner heats the kettle and its contents, and that a negligible amount of water evaporates before boiling begins. Calculate the amount of time required to bring the water to boil.

  In grinding a steel knife bla2 hognp cbnlo4c3/r .3w s,tcs*16hwxde (specific heat = $0.11 \; cal/g \cdot ^{\circ}C$), the metal can get as hot as $400 \; ^{\circ}C$. If the blade has a mass of 80 g, what is the minimum amount of water needed at $20 \; ^{\circ}C$ if the water is not to rise above the boiling point when the hot blade is quenched in it?

  How much heat must be removed 0ez1u76 dslw qfrom steam to change it to liquid?

  Ice has a latent heat of fusioh4;*te5a jxnoh4f-ron of 80 kcal/kg. How much heat is required to melt 200 g of ic4hf*5 t-o xjar4n; heoe?

  How much heat energy is needed to change 10 kg of9+ v1usw6wyrs ice at $-20 \; ^{\circ}C$ to water at $50 \; ^{\circ}C$?

  How much heat needs to be removed fromp f ipl4rov-9. 100 g of $85 \; ^{\circ}C$ water to make $-5 \; ^{\circ}C$ ice?

  The heat of fusion of ice is 80 kcal/kg. When 50 g of i zjb cbj1d;)u ie*:9,0 lrxtemce at $0 \; ^{\circ}C$ is added to 50 g of water at $25 \; ^{\circ}C$, what is the final temperature?

  Eight grams of water in1rko g2l7)p2ric ;ot+ ()yk ep9 nwdhvuxvh5 /itially at $100 \; ^{\circ}C$ are poured into a cavity in a very large block of ice initially at $0 \; ^{\circ}C$. How many g of ice melt before thermal equilibrium is attained?

  A block of ice at $0 \; ^{\circ}C$ is added to a 150-g aluminum calorimeter cup that holds 200 g of water at $10 \; ^{\circ}C$. If all but 2.00 g of ice melt, what was the original mass of the block of ice?

  If 2.0 kg of water a*fuk ;h )fv/xz p ;n*u/0ecloqt $0 \; ^{\circ}C$ is to be vaporized, how much heat must be added?

  How much heat energy is needed to change(6-vu l+ kgid5ry)rax dq/wy cq3ka6. 10 kg of water at $50 \; ^{\circ}C$ to steam at $120 \; ^{\circ}C$?

  How much heat is required to ch(r*rot dvl7f(e-:ouxqk8 5s xange one gram of $0 \; ^{\circ}C$ ice to $120 \; ^{\circ}C$ steam?

  How much heat is required to change bmophe/wox- 5(gyh2: 100 g of $-10 \; ^{\circ}C$ ice to $150 \; ^{\circ}C$ steam?

  A person makes ice tea by adding ice to 1.8 kg of hot tea, initially ar. brp) +hg h9d7.flqxra. 0cbt $80 \; ^{\circ}C$. How many kilograms of ice, initially at $0 \; ^{\circ}C$, are required to bring the mixture to $10 \; ^{\circ}C$?

  The heat of fusion of lead is 5.9 kcal/kg, and thezc9z(:/c dkhnkp zd+6 heat of vaporization is 207 kcal/kg, and its:kdnc+zh6 (zp k/cd z9 melting point is $328 \; ^{\circ}C$. How much heat is required to melt 50 g of lead initially at $23 \; ^{\circ}C$? (The specific heat of lead is $0.031 \; kcal/kg \cdot ^{\circ}C$)

  The thermal conductivity of concrete :j b-kk+z 4zyumy22i cis $0.8 \; W/m \cdot ^{\circ}C$ and the thermal conductivity of wood is $1.1 \; W/m \cdot ^{\circ}C$. How thick would a solid concrete wall have to be in order to have the same rate of flow through it as an 8-cm thick wall made of solid wood? (Assume both walls have the same surface area.)

  The thermal conductivity of al-gg,i 4z mlc4xuminum is twice that of brass. Two rods (one aluminum and the other brass) are joined together end to end in excellent thermal contamgi,4 zlg4xc -ct. The rods are of equal lengths and radii. The free end of the brass rod is maintained at $0 \; ^{\circ}C$ and the aluminum's free end is heated to $200 \; ^{\circ}C$. If no heat escapes from the sides of the rods, what is the temperature at the interface between the two metals?

  A window glass 0.50-cm thick has di u uvlo4dlm8(3odd9a mnn (u(-mensions of 3.0 m by 1.5 m. If the outside temp( uavd(odul89-d uoml 4n3(nmerature is $-10 \; ^{\circ}C$ and the inside temperature $20 \; ^{\circ}C$, what is the rate of heat conduction through the window?

  A window glass 0.50-cm thick has dimensh3 jpp.+ frd;427jsl; ss qwazions of 3.0 m by 1.5 m. If the outside temperad4a 2l.qjpws3rsj;;+ p7h zfsture is $-10 \; ^{\circ}C$ and the inside temperature is $20 \; ^{\circ}C$, how much heat flows through the window in one hour by conduction only?

  How much heat will flow in 11qfks,1qipcb-li 94utz t :/w .0 hour through a 2.0 m x 2.0 m section of concrete (:iqtkuw ,z/1tc 4if-lqp s b91$k = 2.0 \times 10^{-4} \; kcal/s \cdot m \cdot ^{\circ}C$) 10 cm thick if the inside temperature is $21 \; ^{\circ}C$ and the outside temperature is $4 \; ^{\circ}C$?

  How long will it take to transfer 1,000,000 cal of heat through b5jls0:nv cw *a $2.0 \; m^{2}$ pane of 0.30 cm thick glass ($k = 2.0 \times 10^{-4} \; kcal/s \cdot m \cdot ^{\circ}C$) if the temperature differential is $10 \; ^{\circ}C$?

  What is the outside temperature if 4000 k0osvsw,thb l 2q3 ,f:9w0kqq vcal of heat is lost through a $4.0 \; m^{2}$ pane of 0.30 cm thick glass ($k = 2.0 \times 10^{-4} \; kcal/s \cdot m \cdot ^{\circ}C$) in one hour from a house kept at $20 \; ^{\circ}C$?

  In an electric furnace used for refining steel, the temperature is monifu 7jsof3 czb1/j bng q+ud637tored by measuring the radiant power emitted through a smalnj 7/bz3usb6jqf du7 co13f+gl hole of area $0.5 \; cm^{2}$. The furnace acts like a blackbody radiator. If it is to be maintained at a temperature of $1650 \; ^{\circ}C$, at what level should the power radiated through the hole be maintained?

  At what rate is the re lbm4 :6(zzohuman body radiating energy when it is at $33 \; ^{\circ}C$? Take the body surface area to be $1.4 \; m^{2}$, and approximate the body as a blackbody.

  What temperature exists inside a 8*xd2yr,f-qfaf 1z1 tcuv wt9solar collector (effective collection area of $15 \; m^{2}$) on a bright sunny day when the outside temperature is $+20 \; ^{\circ}C$? Assume that the collector is thermally insulated, that the Sun radiates the collector with a power per unit area of $600 \; W/m^{2}$, and that the collector acts as a perfect blackbody.