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College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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Calculate the amount of heat necessary to change 2.5 kg of ice at 0°C into steam?
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- What quantity of joules of energy are needed to transform 11 kg of ice at 0.00°C to vapor at 155°C? Specific heat of water is cwater = 4186 J/kg C° Specific heat of steam is csteam = 2010 J/kg C° Latent heat of fusion of water is Lfusion = 3.33 X 105 J/kg Latent heat of vaporization of water is Lvaporization = 2.26 X 106 J/kg Boiling point of water = 100° Carrow_forwardWhat mass of water at 28.0°C must be allowed to come to thermal equilibrium with a 1.75-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 66.0°C? Assume any water turned to steam subsequently recondensesarrow_forwardA 23 g ice cube at -15.0oC is placed in 129 g of water at 48.0oC. The Specific heat of ice is 2.090 J/g K, the specific heat of water is 4.186 J/g K, and the latent heat of fusion for water is 333 J/g. What is final temperature in celsius of the system when the equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter.arrow_forward
- Suppose that 0.95 g of steam (aka gaseous water), initially at 100 °C, condenses on a 75.0 g block of iron that is initially at 22 °C. What is the final temperature of the combined system when thermal equilibrium is reached?arrow_forwardWhat mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.95-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 60.0°C? Assume any water turned to steam subsequently recondenses. kgarrow_forwardAn ice block of mass 1.2000000000000002 kg at an initial temperature of –11 ∘C is put into a copper pot of mass 2.5 kg containing 4.3 L of water at 21 ∘C. If you heat up the pot, what is the amount of energy (in J) you need to convert all the ice and the water into steam? (Assume that no energy is lost from the system.) You may need some or all of the following constants: The specific heat of ice is 2200 J/kg ∘C, the specific heat of copper is 386 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg and the heat of vaporization for water is 2256000 J/kg .arrow_forward
- What mass of water at 20.0°C must be allowed to come to thermal equilibrium with a 1.90-kg cube of aluminum initially at 150°C to lower the temperature of the aluminum to 70.0°C? Assume any water turned to steam subsequently recondenses. kgarrow_forwardשפיי יוון 6:58 PM | 18.9KB/s ●●● expert.chegg.com/exă Shur 3w/ Question 3 How much heat is required to convert 25.4 g of liquid water (H2O) at 85°C to steam at 135° C? The specific heat capacity for liquid water is 4.18 1/g "C. for steam is 2.01 J/g-C. and the enthalpy of vaporization is 40.7 kJ/mol. Report your answer in kl.arrow_forwardI am stuck on this question i got for homework :( I got a final temperature as 150 degrees Celsius which not possiblearrow_forward
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