Which of the following is the smallest unit of heat energy?:tkdd0k )qm( d

  The amount of heat necessary to raise the temperature of 1 gram ofcl7go )cc./bc water by $1 \; ^{\circ}C$ is referred to as the

  The measure of the averanhu ;)sd v:gm2ge kinetic energy of individual molecules is referred tod :;)ng2vushm as

  A cup of water is scooped up from a swimming pool of w6 iu8u63lt2d smey(k n9zz8ru ocy 7y3ater. Compare the temperature T and the internal energz 7y r28t36eci8sdu y (ulkzmn6u39oyy U of the water, in both the cup and the swimming pool.

  The internal energy of an ideal gas depends omhe.rczj r6b uzo4.g ri ;7ap ,8is7i*n

  An ideal gas at STP is first compressed untysl)x 3t .pwz+w p5 cg2w*9.i qgsznn*il its volume is half the initial volume, and then it is allowed to expand until its pressure is half the initial pressure. All of this is done while holding the t5 cw2* +xs l9z*zwnqgi.pygtsw3.n p) emperature constant. If the initial internal energy of the gas is U, the final internal energy of the gas will be

  An ideal gas with intu5swp 4i+:8di2zy a rnernal energy 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 is that((0r2f(p3:k kyupddec-or ec

  It is a well-known fact te pd3sc-s8 vxpwgg 7bd5:w jps*lfz;7r 7ap:9 hat water has a higher specific heat capacity than iron. Now, consider equal masses of water and iron that are initially in thermal equilibrium. w3pbsavrj9xw5:*g s fp-ld;7p :ge7sc8 pz7d The same amount of heat, 30 calories, is added to each. Which statement is true?

  A thermally isolated system is made up of a hot piece of aluminum av z4inxe50*v)b g ;)i c8zvchmnd a cold piece of copper; the aluminum and the copper are in thermal contact. The specific heat capacity of aluminum is more than double that of copper. Wh;hv* bcci5 vig)04e mxn8)zv zich 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 pn( i, nhlsmt3dft3 :5a substance from the solid to the liquid state is referred hpml53 s t:t,inf3( dnto as the

  The heat required to change a substance fr .8xlwbrk.nf*3 hg (6rmaf2e qom the liquid to the vapor state is refekb hr mfa6.nfg83 *xlq.we2(rrred to as the

  If heat is added to a pure substance at a steady r3eft ci65*n(h 2 spezrate,

  When a solid melts

  When a liquid freezesmepbz0fl1r3-j ue42r

  When a liquid evaporat :mho4k8 n3-:uo mylcnes

  When a vapor condenseswhogt.wgz27p9g:w1yg( j x +x

  In a cloud formation, n1niv2qy aq*(water vapor condenses into water droplets which get bigger and bigger until it rains. This will cause1i( qvqnyn*a2 the temperature of the air in the clouds to

  Turning up the flame under a pan of boiling water cakq1* :pem8uqga4/ hkf uses

  Equal masses of wate4eb*h1d jy hjo- 7.bfv83opuc r 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 collisions is referred to kbh)9hvo6lu /y o24q dasdqo)u9 oyv/ h64l2bkh

  By what primary heat transfer mechanism does one end of an 9cm;.4we1elsy33u6t k9w k2nsusjb qt ;wzi+iron bar become hot whe 6 2wsq4ws ksicj9y19eubez mkuw t;nt+33;l.n the other end is placed in a flame?

  On a cold day, a piece of metal wtfw:c +y /g6hfeels much colder to the touch than a piece of wood. This is due to the difference in :cfw /gt+6hwywhich one of the following physical property?

  If you double the thickness of a wall buoif6 6; i ++woutrk0eiilt from a homogeneous material, the rate of heat loss for a given temperature difference acrof6 6or+k+iet; iwui 0oss the thickness will

  A layer of insulating material with thermal conductivity K t 2 mrti 86cdxiu-0*f4docux.sy*qh5 is placed on a layer of anoth*s0 cyt4xd thi c.625d uxm-f8uior*qer material of thermal conductivity 2K. The layers have equal thickness. What is the effective thermal conductivity of the composite sheet?

  The process whereby heat flows by the mass movement of molecules6 4fw/tb3utl:cky) ul eg)7 rp from one place to another is referred to3kl6pu 7u) /c) t yb4etlwgr:f as

  By what primary heat transfer mechanism is a pot uju9mz+v+0/) 8k jf xjvt )upoof water heated on a stove?

  Convection can occurq (bj tw*swwbm 8c0l+v w0d*t+

  Which of the following bex.vog*tjo w)a m 2l84pst explains why sweating is important to humans in maintaining suitable*w )4ma g.2p o8xtlvjo body temperature?

  A spaceship is drifting in an environment qe;nvo +- fdv)where the acceleration of gravity is essentially zero. As the air on onnvv- ; qeo)df+e side of the cabin is heated by an electric heater, what is true about the convection currents caused by this heating?

  Consider two neighboring rectade 13 dgxl/hy jrgu(s7p.4 en*ngular 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 cold day? Compared to the small house, the largee (l gu sxj ddr4ey.*np37/h1gr house would need heat supplied at

  If the absolute temperature of a radiator is doubled, by what factor does( -gqryj q5ip5 6xhw+h the radiating po 5x 56qyqw(-r+ghjp hiwer change?

  The process whereby heat fl )tz cxjj2 8.t l4/8rkgr zy:e0lhtx-eows in the absence of any medium is referred to as

  By what primary heatlm x8t s5(vt tbaj8t9+ transfer mechanism does the Sun warm the Earth?

  1700 J of work is equivalent to how 2 kxgk(+0yc/n dybh5 ef:j( .aez*wf gmuch heat?

  16.5 kcal of heat is equivalent to3oi/*lg b j)yb 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:lqe*3yosr5) c99pggsm -yok the temperature of 100 g of lead ($c = 0.11 \; kcal/kg \cdot ^{\circ}C$) by $15 \; ^{\circ}C$?

  If 40 kcal of heat is added to 2.0 kg of wat8wr yy)*8jp0xib pm 8ber, what is the resulting temperature change?jbm8 yx)p r80i8 p*wyb

  A 4.0-kg aluminum bl3g 3jnt3-l qwxag b:9mock is 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 te gtw 7zti8ou2, mhz,65ms*: cq xhd;ecmperature 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 by adding 5.0 hv )b; f/dgm 6l0czvclng 76df*,wen,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 co :km5jvg)os8e pper. How much heat is added to thes m8 g:v)eo5kj gear 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 metalr4f:k g)c lzeaebf w6r8 0,l+eg+w z, hpuod)4 is heated 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, initialss x5n)-uq/d; zl6p iyly 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 j+ vpns21 o3qjat $100 \; ^{\circ}C$ 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 isolatedy1ijxraldoq:( q9*9v +ypx +f from its surroundings. One object has an initial temperao 9fv+:rxq*+ylxj(q p 9di1y ature 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 explorkpe;s.puk2 q 8oo40ngvb s-;ve the relationships between various forms of energy by measuring the rise of temperature of water which had fallen down a waterfall on Mount Blanc. What maximum temuvevsg kk 2o;b np8qsop.0-4;perature rise would one expect for a waterfall with a vertical drop of 20 m?

  The water flowing over Niagara Falls drops a distance of *ey /(0k7q ; *msc+d /eskckloswoi m;50 m. Assuming that all the gravitatisw*+ c70s m;d/cly/ik;sk (ekqem *o oonal energy is converted to thermal energy, by what temperature does the water rise?

  A 200-L electric water heater uses 2 kW. Assuming no heat lossz p ;a 7jv-,9rrjog4y2d bjxw3, how long would it take to heat water in this tank frr;9brxy 2zj3j g,4w vapojd7 -om $23 \; ^{\circ}C$ to $75 \; ^{\circ}C$?

  A 5000-W heater is used to he0r-blmjj0c lf6wmo4 fkx0 4 b3at water. How long will it take to heat 20 kg of wmj -4bl6f3r0b4l0 om 0fjkwxcater from $20 \; ^{\circ}C$ to $100 \; ^{\circ}C$?

  An aluminum kettle (mass 1000 5jxt.t9ahp j 5g, $c = 0.22 \; kcal/kg \cdot ^{\circ}C$) 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 blade (specific heatbf:-j:3rrtb( (i zuqu = $0.11 \; cal/g \cdot ^{\circ}C$), 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 from steam to change itpv2wks5 -q2zy:xufn ) to liquid?

  Ice has a latent heat/a4cg7 rj6wl,-uw dyj of fusion of 80 kcal/kg. How much heat is required to melt 200 6d-wwg 7yrl/4aj, c jug of ice?

  How much heat energy is needed to chanz,dn iprytb4d u 8/(5fge 10 kg of ice at $-20 \; ^{\circ}C$ to water at $50 \; ^{\circ}C$?

  How much heat needs t,qioqh8 w 8w:9spnlk6o be removed from 100 g of $85 \; ^{\circ}C$ water to make $-5 \; ^{\circ}C$ ice?

  The heat of fusion of g 5it6/t(8vsoig y0wsice is 80 kcal/kg. When 50 g of ice at $0 \; ^{\circ}C$ is added to 50 g of water at $25 \; ^{\circ}C$, what is the final temperature?

  Eight grams of water initially at td uuxj(3h6s;xqd t,3 $100 \; ^{\circ}C$ 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 at vk;kqy/ 2 9yyc6kgxl e6b-sx +tlp3s 1$0 \; ^{\circ}C$ is to be vaporized, how much heat must be added?

  How much heat energy is needed to chkq:z1i*a/eorxfg ; f)ange 10 kg of water at $50 \; ^{\circ}C$ to steam at $120 \; ^{\circ}C$?

  How much heat is required to change one gram so1m)0gu3g da :v y:epof $0 \; ^{\circ}C$ ice to $120 \; ^{\circ}C$ steam?

  How much heat is required togzx8a5o rdk2w m 0t4y4 change 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 acg2g dlu63kjgr35gx /t $80 \; ^{\circ}C$. 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 the heat of vaporization ;26fs48/romou5b not tl ,qta is 207 kcal/kg, and its melting pot5tr4o,m/a ntq oo 6l2sb; uf8int 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 t r szr+4/mwhgpv* n6h(,tl /y/plg+jk bt4 a0is $0.8 \; W/m \cdot ^{\circ}C$ 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 ngbn i-s)a7l(l ht 3o h90nt;xaluminum is twice that of brass. Two rods (one aluminum and the other brass)9)n3tt0a7o h;il hs-x(gnnlb are joined together end to end in excellent thermal contact. 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 dimensions of 3r ihhpa; yd 2 ctu-8i3sz)*)rr.0 m by 1.5 m. If the outside temperature irr-;a) 2 h u8sitd hy*3rpci)zs $-10 \; ^{\circ}C$ 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 dimeny)/k*htsz0gp sions of 3.0 m by 1.5 m. If the outside tempe*z)kt/hypgs 0rature 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 1.0 hoi*l:(e rgkpfhh)m t;0 ur through a 2.0 m x 2.0 m section of concrete *h m0)p figh;ke( l:tr($k = 2.0 \times 10^{-4} \; kcal/s \cdot m \cdot ^{\circ}C$) 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/qq p6 p4o5zvd cal of heat through 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 tempera1rlv4i0 kfri7: xj3ct ture if 4000 kcal 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 fo:x:z1imzpz oq (ks)w 4r refining steel, the temperature is monitored by meaiq s)o:p(w1:kz zzx 4msuring the radiant power emitted through a small 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 human bod8s o-cicym(n1 u )u2; uvz,brcy 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 solar collector (effective collectiond-jz 30f 7+vd*pkv dxn 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.