A gas burner transfers 9.20 × 105 J into a block of ice with a mass of 2.29 kg and an initial temperature of 0°C. (a) How much of the energy (in J) supplied by the burner goes into melting all the ice into liquid water? (Enter you answer to at least three significant figures.) 769440 ✓ Melting is a phase change from solid to liquid and requires an energy transfer of Q = mL, where Lf latent heat of fusion. Freezing is a phase change from liquid to solid and requires an energy transfer of Q = -mLp In freezing, the energy transfer is negative because energy is removed from the substance. J (b) How much of the energy (in J) supplied by the burner goes into raising the temperature of the liquid water? (E your answer to at least three significant figures.) 1.57E+5 Think about conservation of energy. The total energy supplied is known, and you found in part (a) the energy goes into melting. How much is left over? J (c) What is the final temperature of the liquid water in degrees Celsius? 15.65 Use the energy found in part (b). How does it relate to mass, specific heat, and temperature change? What is initial temperature? °C

A gas burner transfers 9.20 × 105 J into a block of ice with a mass of 2.29 kg and an initial temperature of 0°C. (a) How much of the energy (in J) supplied by the burner goes into melting all the ice into liquid water? (Enter you answer to at least three significant figures.) 769440 ✓ Melting is a phase change from solid to liquid and requires an energy transfer of Q = mL, where Lf latent heat of fusion. Freezing is a phase change from liquid to solid and requires an energy transfer of Q = -mLp In freezing, the energy transfer is negative because energy is removed from the substance. J (b) How much of the energy (in J) supplied by the burner goes into raising the temperature of the liquid water? (E your answer to at least three significant figures.) 1.57E+5 Think about conservation of energy. The total energy supplied is known, and you found in part (a) the energy goes into melting. How much is left over? J (c) What is the final temperature of the liquid water in degrees Celsius? 15.65 Use the energy found in part (b). How does it relate to mass, specific heat, and temperature change? What is initial temperature? °C

Principles of Physics: A Calculus-Based Text

5th Edition

ISBN:9781133104261

Author:Raymond A. Serway, John W. Jewett

Publisher:Raymond A. Serway, John W. Jewett

Chapter17: Energy In Thermal Processes: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 69P: An aluminum rod 0.500 m in length and with a cross-sectional area of 2.50 cm2 is inserted into a...

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Consider the latent heat of fusion and the latent heat of vaporization for H2O, 3.33 105 J/kg and 2.256 106 J/kg, respectively. How much heat is needed to a. melt 2.00 kg of ice and b. vaporize 2.00 kg of water? Assume the temperatures of the ice and steam are at the melting point and vaporization point, respectively. (a). UsingEq21.9, Q = mLF = (2.00 kg) (3.33l05 J/kg) = 6.66105 J (b).UsingEq21.10. Q = mLV = (2.00kg) (2.256106 J/kg) = 14.51106 J
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?
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.)
An ideal gas initially at 300 K undergoes an isobaric expansion at 2.50 kPa. If the volume increases from 1.00 m3 to 3.00 m3 and 12.5 kJ is transferred to the gas by heat, what are (a) the change in its internal energy and (b) its final temperature?
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