a) How much heat is required to raise the temperature of 250ml of water from 20°C to 35°C? b) How much heat is lost by the water as it cools back down to 20.0°C?
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A: Given: The answer is shown as:
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A: Mass of ice = mice = 21.4 g Mass of water = mw = 75.3 g Final/equilibrium temperature of the mixture…
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- You drop an ice cube into an insulated container full of water and wait for the ice cube to completely melt. The ice cube initially has a mass of 80.0 g and a temperature of 0°C. The water (before the ice cube is added) has a mass of 770 g and an initial temperature of 26.0°C. What is the final temperature (in °C) of the mixture? (Assume no energy is lost to the walls of the container, or to the environment.)A 0.310 kg aluminum bowl holding 0.795 kg of soup at 25.0°C is placed in a freezer. What is the final temperature (in °C) if 373 kJ of energy is transferred from the bowl and soup, assuming the soup's thermal properties are the same as that of water? °℃ tA 1.0-m-long steel beam, initially at a temperature of 250 C, increases in temperature to 1000 C by inserting it into an insulating jacket for several minutes while the inside of the jacket is subsequently flooded with steam. By how much does the length of the steel beam expand? (The thermal coefficient of linear expansion for steel is 12 x 10-6 (C0)-1) a. 0.90 mm b. 1.0 mm c. 0.70 mm d. 0.80 mm e. 0.60 mm
- A 0.200-kg mass of metal with a specific heat of 1255.8 J/kg-°C, initially at 90°C, is placed in a 0.500-kg calorimeter, with a specific heat of 418.6 J/kg-°C, initially at 20°C. The calorimeter is filled with 0.100 kg of water, initially at 20°C. The specific heat of water is 4186 J/kg-°C. What is the final temperature once the combination of metal, calorimeter, and water reach equilibrium? O 70°C 40°C 60°C O 50°CA coffee cup calorimeter contains 48.00 grams of water at 25.0°C. Two additional samples of water are added to the calorimeter as follows: 38.00 grams of water at 53.5°C 52.50 grams of water at 65.5°C Assuming there is no heat absorbed by the calorimeter or lost to the surroundings, calculate the final temperature of the water in °C. The specific heat of water is 4.184 J g‑1°C-1.Problem 6: You have 4.9 kg of water in an insulated container. You add 0.95 kg of ice at -21 °C to the water and the mix reaches a final, equilibrium temperature of 11 °C. The specific heats of ice and water are 2.10 ×103 J/kg⋅C° and 4.19 ×103 J/kg⋅C°, respectively, and the latent heat of fusion for water is 3.34 ×105 J/kg. Calculate the initial temperature of the water, in degrees Celsius.
- 12 Assume Lake Huron contains 3.60 x 10-2 m³ of water, and assume the water's density is that of water at 20°C and 1 atm. (a) How much energy (in J) is required to raise the temperature of that volume of water from 12.8°C to 23.6°C? 1.627e24 From the density of water and the volume, what is the mass of the water? What is specific heat? How is it related to the energy input, mass, and temperature change? Use it to solve for the energy. Be careful with units. J (b) How many years would it take to supply this amount of energy by using a power of 1,400 MW generated by an electric power plant? yrAn 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 hp1)A common practice for a person with a high fever is to take a bath in cool water. Assuming an 80 kg person is really ill and needs to cool down from 40°C to 37°C. What is the minimum amount of water needed for bathing assuming the water begins at room temperature, 25°C? The specific heat of the body on average is 3470 J/kg°C and water is 4186 J/kg°C. 16.6 kg 212.2 kg 19.8 kg 200 kg 2( photo question) 3) Describe the distinguishing features between mechanical waves and light waves, and longitudinal versus transverse waves. Be sure to include the terms medium, particles, vacuum, perpendicular and direction of wave motion. professor can you answer these questions please?
- You drop an ice cube into an insulated bottle full of water and wait for the ice cube to completely melt. The ice cube initially has a mass of 70.0 g and a temperature of 0°C. The water (before the ice cube is added) has a mass of 880 g and an initial temperature of 20.0°C. What is the final temperature (in °C) of the mixture? (Assume no energy is lost to the walls of the bottle, or to the environment.) ?°CYou drop an ice cube into an insulated container full of water and wait for the ice cube to completely melt. The ice cube initially has a mass of 60.0 g and a temperature of 0°C. The water (before the ice cube is added) has a mass of 850 g and an initial temperature of 30.0°C. What is the final temperature (in °C) of the mixture? (Assume no energy is lost to the walls of the container, or to the environment.)Anice chest at a beach party contains 12 cans of soda at 3.70°C. Each can of soda has a mass of 0.35 kg and a specific heat capacity of 3800 J/(kg C). Someone adds a 8.99-kg watermelon at 25.0°C to the chest. The specific heat capacity of watermelon is nearly the same as that of water. Ignore the specific heat capacity of the chest and determine the final temperature T of the soda and watermelon in degrees Celsius. Number Units Tube Initial Final