How many CAL must be added to heat 300.0 g of water from -37.0°C to 50.0 °C ? Don't do the calculation, just indicate which conversion factors would be used specific heat of the solid, 0.504 cal/g°C specific heat of the liquid, 0.999 cal/g°C specific heat of the gas, 0.497 cal/g°C heat of fusion, 79.7 cal/g heat of vaporization, 539 cal/g a. used b. not used

How many CAL must be added to heat 300.0 g of water from -37.0°C to 50.0 °C ? Don't do the calculation, just indicate which conversion factors would be used specific heat of the solid, 0.504 cal/g°C specific heat of the liquid, 0.999 cal/g°C specific heat of the gas, 0.497 cal/g°C heat of fusion, 79.7 cal/g heat of vaporization, 539 cal/g a. used b. not used

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 19P: A 1.00-kg block of copper at 20.0C is dropped into a large vessel of liquid nitrogen at 77.3 K. How...

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A Styrofoam box has a surface area of 0.80 m and a wall thickness of 2.0 cm. The temperature of the inner surface is 5.0C, and the outside temperature is 25C. If it takes 8.0 h for 5.0 kg of ice to melt in the container, determine the thermal conductivity of the Styrofoam.
Compare the SI units of specific heat and latent heat and explain any differences.
A 1.00-kg block of copper at 20.0C is dropped into a large vessel of liquid nitrogen at 77.3 K. How many kilograms of nitrogen boil away by the time the copper reaches 77.3 K? (The specific heat of copper is 0.092 4 cal/g C, and the latent heat of vaporization of nitrogen is 48.0 cal/g.)
Please answer the question with steps … How much heat must be absorbed by ice of mass 378 gram to melt completely? Provide the answer in kJ with accuracy upto two decimal points. Consider the following: Specific Heat of ice as 2220 J/kg.K Heat of Fusion LF = 333 kJ/kg Heat of Vaporization Ly = 2256 kJ/kg
At a foundry, 22 kg of molten aluminum witha temperature of 660.4◦C is poured into amold.If this is carried out in a room containing150 kg of air at 25◦C, what is the temperatureof the air after the aluminum is completelysolidified? Assume that the specific heat capacity of air is 1.0×10^3J/kg ·◦C. The specificheat of aluminum is 899 J/kg ·◦ C and its latent heat of fusion is 3.97 × 10^5J/kg.Answer in units of ◦C
On a cold winter morning you step outside to get into your car and drive to work. Your car's windshield is covered with ice at −14.3°C. If the area of the windshield is 1.40 m2 and it takes 1.77 105 J of heat to melt the ice, how thick was the ice covering the windshield? The latent heat of fusion of ice is 334 kJ/kg, the specific heat of ice is 2092 J/(kg · °C) and its density is 917 kg/m3 (answer in m).
1. A cube of ice is taken from the freezer at -8.5 •C•C and placed in a 75-gg aluminum calorimeter filled with 330 gg of water at room temperature of 20.0 •C•C. The final situation is observed to be all water at 15.0 •C•C. The specific heat of ice is 2100 J/kg - CoJ/kg•Co, the specific heat of aluminum is 900 J/kg •CoJ/kg•Co, the specific heat of water is is 4186 J/kg• CoJ/kg•Co, the heat of fusion of water is 333 kJ/KgkJ/Kg. What was the mass of the ice cube? 2. When a 290-gg piece of iron at 180 •C•C is placed in a 95-gg aluminum calorimeter cup containing 250 gg of liquid at 10• C•C, the final temperature is observed to be 35 • CoC. The value of specific heat for iron is 450 J/kg •CoJ/kg •Co, and for aluminum is 900 J/kg-CoJ/kg-Co. Determine the specific heat of the liquid.
A 235-g sample of a substance is heated to 350 ∘C and then plunged into a 105-g aluminum calorimeter cup containing 185 gg of water and a 17-g glass thermometer at 11.5 ∘C. The final temperature is 35.0∘C. The value of specific heat for aluminium is 900 J/kg⋅C , for glass is 840 J/kg⋅C, and for water is 4186 J/kg⋅C∘ What is the specific heat of the substance? (Assume no water boils away.)
On a cold winter morning you step outside to get into your car and drive to work. Your car's windshield is covered with ice at −15.3°C. If the area of the windshield is 1.40 m2 and it takes 1.97 105 J of heat to melt the ice, how thick was the ice covering the windshield? The latent heat of fusion of ice is 334 kJ/kg, the specific heat of ice is 2092 J/(kg · °C) and its density is 917 kg/m3.
4. 100.0 g of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4180J/kg°C, calculate the amount of heat energy needed to cause this rise in temperature. 5. A 0.3 kg piece of copper is heated and fashioned into a bracelet. The amount of energy transferredby heat to the copper is 66,300 J. If the specific heat of copper is 390 J/kg celcius, what is the change of thecopper's temperature?
A student, who is trying to drink away memories of a physical science homework, decides to pour themselves a bourbon on the rocks. They put an ice cube of mass 508 g which is at -9.9 ˚C into their bourbon. How much heat is necessary to change 508 g of ice to water at 20°C? The specific heat of water is 4186 J/kg˚C, The specific heat of ice is 2090 J/kg˚C, and the specific heat of steam is 2010 J/kg˚C The latent heat of fusion for water is 3.33 x 105 J/kg and the latent heat of vaporization for water is 2.26 x 106 J/kg
The hot plate in your lab takes an average of 8minand 55sto boil 100mLof water. How long does the same hot plate take to boil 100mLof acetone? Express this time in units of min and s. Use the following information: •The temperature of the lab is 75◦F •The hot plate has a power rating of 283W •The boiling point of acetone is 56◦C •The specific heat capacity of water is 4.18J/(g◦C) •The specific heat capacity of acetone is 2.15J/(g◦C) •The specific gravity of acetone is 0.785