A substance has a melting point of 20°C and a heat of fusion of 3.9 x 104 J/kg. The boiling point is 150°C and the heat of vaporization is 7.8 x 104 J/kg at a pressure of 1.0 atm. The specific heats for the solid, liquid, and gaseous phases are 600 J/(kg-K), 1000 J/(kg-K), and 400 J/(kg-K), respectively. The quantity of heat required to raise the temperature of 3.80 kg of the substance from -6°C to 128°C at a pressure of 1.0 atm, is closest to

A substance has a melting point of 20°C and a heat of fusion of 3.9 x 104 J/kg. The boiling point is 150°C and the heat of vaporization is 7.8 x 104 J/kg at a pressure of 1.0 atm. The specific heats for the solid, liquid, and gaseous phases are 600 J/(kg-K), 1000 J/(kg-K), and 400 J/(kg-K), respectively. The quantity of heat required to raise the temperature of 3.80 kg of the substance from -6°C to 128°C at a pressure of 1.0 atm, is closest to

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter3: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 66P: One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of...

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One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?
For a temperature increase of 10 at constant volume, what is the heat absorbed by (a) 3.0 mol of a dilute monatomic gas; (b) 0.50 mol of a dilute diatomic gas; and (c) 15 mol of a dilute polyatomic gas?
A 100-g piece of copper, initially at 95.0C, is dropped into 200 g of water contained in a 280-g aluminum can; the water and can are initially at 15.0C. What is the final temperature of the system? (Specific heats of copper and aluminum are 0.092 and 0.215 cal/g C, respectively.) (a) 16C (b) 18C (c) 24C (d) 26C (e) none of those answers
An aluminum rod 0.500 m in length and with a cross-sectional area of 2.50 cm2 is inserted into a thermally insulated vessel containing liquid helium at 4.20 K. The rod is initially at 300 K. (a) If one-half of the rod is inserted into the helium, how many liters of helium boil off by the time the inserted half cools to 4.20 K? Assume the upper half does not yet cool. (b) If the circular surface of the upper end of the rod is maintained at 300 K, what is the approximate boil-off rate of liquid helium in liters per second after the lower half has reached 4.20 K? (Aluminum has thermal conductivity of 3 100 W/m K at 4.20 K; ignore its temperature variation. The density of liquid helium is 125 kg/m3.)
You mix mI = 1.2 kg of ice at TI = -21°C with mW = 4.8 kg of water at TW = 72°C in an insulated container. The specific heats of ice and water are cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively, and the latent heat of fusion for water is Lf = 3.34 × 105 J/kg. Enter an expression for the final equilibrium temperature of the mixture in terms of the defined quantities.
Water with a mass of mW = 0.400 kg and temperature of TW = 18.5°C is poured into an insulated bucket containing mI = 0.11 kg of ice at a temperature of TI = -18°C. Assume the specific heats of ice and water are constant at cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively. The latent heat of fusion for water is Lf = 334×103 J/kg. What is the final temperature of the mixture, in degrees Celsius?
A 405-g sample of lead with specific heat cPb = 128 J/(kg · °C) at 87.0°C and a 220-g sample of silver with specific heat cAg = 230.0 J/(kg · °C) at 38.0°C are added to 0.500 kg of water at 22.0°C where specific heat of water cW = 4190 J/(kg · °C) in an insulated container. Assuming the system is thermally isolated, what is its final equilibrium temperature?
A thirsty nurse cools a 2.40 L bottle of a soft drink (mostly water) by pouring it into a large aluminum mug of mass 0.249 kg and adding 0.122 kg of ice initially at -14.3 ∘C. If the soft drink and mug are initially at 21.0 ∘C, what is the final temperature of the system, assuming no heat losses? Express your answer in degrees Celsius.
Initially you have mwater=4.2kg of water at Twater=66 degrees celcius in a insulated container. You add ice at T ice= -18 degrees celcius to the container and the mix reaches a final, equillibrium temperature of Tf=27 degrees celcius. The specific heat of ice and water are c ice= 2.10×10^3 J/kg×°C) and c water= 4.19×10^3, respectivly, and the latent heat of fusion of water is Lf= 3.34×10^5 J/kg. A.) What is the expression for the mass of ice you added, in terms of the defined quantities? B.) What is the mass of ice, in Kg?
3 moles of an ideal polyatomic gas initially with a volume of 2 m3 and a temperature of 3000C is compressed isothermally to 1/3rd its initial volume. How much heat must be added to the system during this compression? a) 15.7 kJ b) -15.7 kJ c) 8.2 kJ d) – 8.2 kJ
The specific heats of aluminum and iron are 0.214 and 0.107 calories per gram degrees Celsius [cal/(g °C)] respectively. If we add the same amount of energy to a cube of each material (of the same mass) and find that the temperature of the aluminum increases by 27 degrees Fahrenheit [°F], how much will the iron temperature increase in degrees Fahrenheit [°F]?
A thermal window, with an area of 6.0m ^ 2, is constructed of two layers of glass, each 4.0mm thick, separated from each other by a 5.0mm air gap. If the inner surface is at 20.0 ° C and the outer surface is at -5.0 ° C, what is the rate of energy transfer by conduction through the window? The thermal conductivity of glass is 0.8 W⁄ (m. ° C) and that of air is 0.023 W⁄ (m. ° C)