College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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How much heat must be removed from 456 g of water at 25.0°C to change it into ice at -10.0°C? The specific heat of ice is 2090 J/kg ∙ K, the latent heat of fusion of water is 33.5 × 104 J/kg, and the specific heat of water is 4186 J/kg ∙ K
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- A cooking pot has a copper bottom of area 4.00x 10-2 m2 and thickness 1.00 cm. if the pot is set on a 521 °F stove top and filled with ice water, what is the melting rate of the ice? The thermal conductivity of copper is 3.90x 102 J/(s m K) and the latent heat of fusion of water is 3.35x 105 J/kg.(answer must be in kg/s) Estimate the lowest environment temperature that a person, who has skin temperature 34.0 °C, total skin area 1.53 m², emissivity 0.800, and metabolic energy production 157 J/s, can stand naked without a significant drop of body temperature. (answer in celicus)arrow_forwardYou hold a 338 grams of coffee in a 267 gram porcelain cup which is too hot to drink at 85°C. You want to cool it down to 50°C by adding crushed ice at 0°C. Assume that there are no heat losses to your hand or surrounding. Specific heat of porcelain: 1000 J/kg°C Specific heat of coffee: 4186 J/kg°C Latent heat of fusion for ice: 3.33 x 10^5 J/kg How many grams of ice should you add? Assume that there are no heat losses to your hand or surroundings.arrow_forward2.6 of water at 28 °C is added to 5.0 of water at 69 ° C. What is the temperature of the mixture in °C if no energy was lost? ( specific heat of water is 4186 J/Kg ^ C)arrow_forward
- A plastic cup of negligible mass contains 0.280 kg of an unknown liquid at a temperature of 30.0 °C. A 0.0270 kgkg mass of ice at a temperature of 0.0°C°C is added to the liquid, and when thermal equilibrium is reached the temperature of the combined substances is 14.0 °C°C. Assuming no heat is exchanged with the surroundings, what is the specific heat capacity of the unknown liquid? Express your answer in joules per kilogram-kelvin.arrow_forwardHow many joules are needed to change 50g of ice at 0°C to steam at 120°C?The latent heat of fusion of ice is 3.35 x 10°J/kg; latent heat of vaporization of water is 2.26 x 10°J/kg. The specific heat capacities of ice; water, and steam, respectively, are 2093 J/(kg. K), 4186 J/(kg. K) and 2010 J/(kg. K). out of Select one: A. 50.68 kJ B. 63.96 kJ O C. 227.6 kJ D. 53.96 kJ E. 20.5 kJ F. 800.2 kJ G. 153.7 kJ H. 22.76 kJarrow_forwardA copper vessel whose mass is 150 g contains 60 g of water at 15.50C. How many calories of heat are required to bring the water to a final temperature of 850C? The specific heat of water is 1.0 cal/g C0.arrow_forward
- You are given 204 g of coffee (same specific heat as water) at 80.0°C (too hot to drink). In order to cool this to 60.0°C, how much ice (at 0.0°C) must be added? Ignore the heat capacity of the cup and heat exchanges with the surroundings. Specific heat capacity (15.0°C) of water is 4.186 kJ/(kg-K). The latent heat of fusion of water is 333.7 × 103 J/kg.arrow_forwardCALCULATIONarrow_forwardSpecific Heat of Water = 4186 J/kg °C, Specific Heat of Iron = 452 J /kg °C, Specific Heat of Ice = 2093 J/kg °C, Specific Heat of Lead = 130 J/kg °C Latent Heat of Fusion = 3.34 x 105 J/kg, Specific Heat of Copper = 385.1 J /kg.°C Density of iron = 7.874 g /cm3 Density of copper = 8.95 g /cm3 2. Convert 403 K to °F temperature.arrow_forward
- If 31.0 g of milk at a temperature of 3.95°C is added to a 250-g cup of coffee at a temperature 88.5°C, what is the final temperature of the mixture? Assume coffee has a specific heat of 4.19 x 10° 1/(kg · K) and milk has a specific heat of 3.93 x 103 1/(kg · K). °Carrow_forwardAn ice tray is removed from a freezer, where the ice was at a temperature of -11°C, and left on a countertop. If the mass of the ice is 0.29 kg, how much heat must be added in k to turn all the ice into room temperature water (that is, liquid water at 20°C)? The specific heat of water is 4.2 kgC kJ the heat of fusion of water is 335 kg kJ and the specific heat of ice is 2.1 kg°C* 133.69 This is a change of phase question. There are 3 cases we have to consider: 1. The heat required to increase the temperature of the ice, Q1 2. The heat required to turn the ice into a liquid (a phase change), Q2 3. The heat required to raise the temperature of the now liquid water, Q3 For Q1, you will use the equation Q = mcATusing the c=2.1 kJ/(kg*C). Keep in mind that the hparrow_forwardYou wish to cool a 1.95 kg block of brass initially at 80.0°C to a temperature of 41.0°C by placing it in a container of water initially at 20.0°C. Determine the volume (in L) of the liquid needed in order to accomplish this task without boiling. The density and specific heat of water are respectively 1,000 kg/m3 and 4,186 J/(kg · °C), and the specific heat of brass is 380 J/(kg · °C).arrow_forward
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