Three ice cubes are used to chill a soda at 20°C with mass msoda = 0.25 kg. The ice is at 0°C and each ice cube has a mass of 6.0 g. Assume that the soda is kept in a foam container so that heat loss can be ignored. The soda has the same heat capacity as water (4186J/kg°C) and the latent heat of ice is 334,000 J/kg. Find the final temperature when all ice has melted?
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- A 7 kg of glass bowl (c = 840 J/kg·K) contains 16 kg of water (c =4186 J/kg·K) at 25°C. 2.5 kg of ice (c = 2.1x103 J/kg·K) are added to the water. The ice has an initial temperature of -20.0°C, having kept in a very cold freezer. It may be assumed that there is no heat flow between the bowl and the external environment. When thermal equilibrium is reached, all the ice melted, the final temperature of the mixture is above 0°C. Determine this temperature. Lf for water = 33.5x104 J/kgA 0.250-kg aluminum bowl holding 0.800 kg of soup at 25.0°C is placed in a freezer. What is the final temperature if 430 kJ of energy is transferred from the bowl and soup? Assume the soup has the same thermal properties as that of water, the specific heat of the liquid soup is 1.00 kcal/(kg · °C), frozen soup is 0.500 kcal/(kg · °C), and the latent heat of fusion is 79.8 kcal/kg. The specific heat of aluminum is 0.215 kcal/(kg · °C).You 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.
- The amount of heat per second conducted from the blood capillaries beneath the skin to the surface is 260 J/s. The energy is transferred a distance of 1.5 x 103 m through a body whose surface area is 1.4 m². Assuming that the thermal conductivity is that of body fat, determine the temperature difference between the capillaries and the surface of the skin.Suppose you want to raise the temperature of a 0.195-kg piece of ice from -20.0°C to 130°C. The heat of fusion is Lf = 334 kJ/kg, and the heat of vaporization is Lv = 2256 kJ/kg. In this problem, take 1520 J/kg⋅°C as the specific heat of steam, and 2090 J/kg⋅°C as the specific heat of ice. How much heat, in kilocalories, must be transferred for this to happen, including the energy needed for phase changes? How much time, in seconds, is required to do this, assuming a constant 20.0 kJ/s rate of heat transfer?A closed box is filled with dry ice at a temperature of -86.0 °C, while the outside temperature is 21.0 °C. The box is cubical, measuring 0.394 m on a side, and the thickness of the walls is 4.49 × 102 m. In one day, 3.76 × 106 J of heat is conducted through the six walls. Find the thermal conductivity of the material from which the box is made. Number Units
- A thermally isolated container has 479 grams of water in it and a 376 gram plastic block. The water had an initial temperature of 352 K. The plastic had an initial temperature of 300 K. The plastic and water reach an equilibrium temperature of 342 K. Water has a specific heat of 4.182 J/(gram K). What is the specific heat of the plastic block in J/(gram K)?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.We have 39.5 g of a particular substance. Its specific heat in solid form is 0.8 J/(g K) and its specific heat in liquid form is 1.4 J/(g K); it's latent heat of melting is 170 J/g. Its initial temperature is 196 and its melting point is 223. We wish to raise its temperature to 297 (where it is a liquid). How much heat is required?
- 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°CAn unknown substance has a mass of 0.125 kg and an initial temperature of 90.0°C. The substance is then dropped into a calorimeter made of aluminum containing 0.285 kg of water initially at 21.5°C. The mass of the aluminum container is 0.150 kg, and the temperature of the calorimeter increases to a final equilibrium temperature of 32.0°C. Assuming no thermal energy is transferred to the environment, calculate the specific heat of the unknown substance.A styrofoam container used as a picnic cooler contains a block of ice at 0°C. If 564 g of ice melts in 1 hour, how much heat energy per second is passing through the walls of the container? The heat of fusion of ice is 3.33 x 10° J/kg. Answer in units of W.