A calorimeter contains 1.500kg of water at 80.0°C. Then 0.500kg of ice at -5.00°Cis added to the water. What is the final temperature, in °C, after the system has come to thermal equilibrium? (Look at the equation sheet for data on water.)
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Specific heat of water = 4190(J/kg*K)
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- CALCULATIONSpecific 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.A kettle brings 2.15 kg of water at 34.9˚C to steam at 110˚C. How much heat does this take? 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
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- When the indoor temperature of a house is 25°C and the outdoor temperature is -8°C, the inside and outside surfaces of the glass are measured to be 21.3°C and 17.3°C. If the glass has an area of 3.16 m2 and a thickness of 6.14 mm, what is the rate of heat (in W) lost though the window? {kglass = 0.78 W/m∙K}1.2-kg of ice at -6.0°C is dropped into 5.0 L (5.566-kg) of car coolant. The initial temperature of the coolant is 25.0°C. The ice and coolant are insulated, so energy transfers to the outside is negligible. After hours, all ice melts and the final temperature of the mixture of water-coolant is 1.8°C. The specific heat of ice is 2090 J/kg °C; the specific heat of water is 4186 J/kg °C; the latent heat of fusion for water is 334000 J/kg. A. What is the energy needed for heating the ice to 0 °C? B. Determine the energy needed to melt the ice into water. C. Determine the total energy needed to heat the -6.0°C ice to 1.8°C water. (Please note: the total energy also includes the part heating water from 0.0 °C to 1.8 °C.) D. Determine the specific heat capacity of the coolant.A copper kettle contains water at 22.5 °C. When the water is heated to 96.3 °C, the volume of the kettle expands by 5.95 x 10-5 m3. Determine the volume of the kettle at 22.5 °C.
- Arelyz and Hyeonggyun drop a 378.0-g piece of metal at 100.0°C into 447.0 g of water at 20.0°C. The final temperature of the system is measured to be 50.0°C. What is the specific heat of the metal in J/kgK, assuming no heat is exchanged with the surroundings or the cup containing the water? The specific heat of water is 4190 J/(kg K).When a material changes phase - liquid, solid, gas- heat exchange is required. This heat is called the Latent heat. is the equation where L is the Latent heat and is material specific. How much heat is required to take water (mass of .55 kg) from -20 to 20 C? L for ice to water is 33.5 * 104 J/kg. the specific heat of ice is 2090 J/(kg*C).and for water is 4186 J/(kg*C).An incandescent light bulb with a surface area of 0.0120 m2 and an emissivity of 0.9 has a surface temperature of 178°C. What is the rate of thermal radiation emitted from the bulb [round your final answer to one decimal place]? {o = 5.6704 x 10-8 W/(m²-K“)} 60 W T.