How much heat is required to convert 5 kg of ice at -20C to steam at +100C? (relevant constants given below for convenience) Cice= 2.108x103 J/kg°C Cwater= 4.186x10³ J/kg°C L= 3.335x105 J/kg Lv= 2.260x106 J/kg O 2.303 × 106 J O 1.360 x 107 J O 1.485 × 10’ J O 1.527 x 107 J 1.570 × 107 J
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- 2.2 kg of ice (solid phase of water) at -10°C is heated under atmospheric pressure. Answer the following questions. Use the following values for your calculation. specific heat of ice: 2.1 kJ/(kg °C) specific heat of water: 4.2 kJ/(kg °C) specific heat of vapor: 2.0 kJ/(kg °C) latent heat of fusion: 334 kJ/kg latent heat of vaporization: 2260 kJ/kg How much heat is required to raise the temperature of the ice to melting point T = 0°C? How much heat is required to change the phase of the ice to liquid water? How much heat is required to raise the temperature of the liquid water to boiling point T = 100°C?An iron rod with an initial length of 13.65 m has its temperature raise from 10°C to 31.74°C. If an iron has a coefficient of thermal expansion of 12 times Fr..10 to 6th power 1/Celsius what is the changing in the length of the rod?Question 11 After some time, you pour 0.5 kg of milk, whose initial temperature was 5°C. What will be the final equilibrium temperature of this system? Let: 1.5 kg of coffee, originally at 90°C, is placed into a .3 kg aluminum cup. J Ccoffee = 4186 kg K J CAI = 500 kg K J CMilk = 3000 kg K Question 12 A solid steel sphere of radius 50 acts as a perfect radiator, calculate the amount of heat it will radiate after 1 min. cm is heated to 3000 K. If the sphere
- @ 2 O: F2 W S 8. An electric immersion heater has a power rating of 1900 W. If the heater is placed in a 1.8 kg of water at 30 °C, how many minutes will it take to bring the water to a boiling temperature? (Assume that there is no heat loss except to the water itself. Cwater=4186 J/kg.°C) min # 3 X 80 F3 E D $ 4 C F4 R TI F or do % 5 V F5 T G > 6 MacBook Air B F6 < H 887 & ◄◄ F7 U N * 8 J DII F8 M ( 9 K F9 O ) C L F10 (4) P F11 31 + 11 F12 18 BEL ?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° CWhen 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}
- The initial temperature of 60 g of ice is -200C. The specific heat capacity of ice is 0.5 cal/g.C0 and water’s is 1 cal/g.C0. The latent heat of fusion of water is 80 cal/g. How much heat is required to raise the ice to 00C and completely melt the ice? (b) How much additional heat is required to heat the water (obtained by melting the ice) to 620C?A person tries to cool down her bath water by adding 5.0 Kg of ice at 0°C to 75.0 Kg of water at 70°C. What is the final temperature of the water? (Lf = 333 KJ/Kg & cH2O =4186 J/Kg°C)What is the ratio of the energy required to warm 125 g of Ice (0.0 \deg C) to body temperature (37 \deg C) to warming the same amount of water through the same temperature change? Answer format is the number Eice/Ewater = (2 significant figures) Latent Heat of Fusion of Water: 335, 000 J/kg Specific Heat Capacity of Water: 4186 J/kg/\deg C
- Calculate the total heat transfer from the 5.0 m² surface shown in the figure. Tur = 0°C h = 40 W/m²-K T = 180°C ɛ = 0.90 fluid T = 10°C insulatedMeasurement of specific heat of metals Aluminum Cupper Mass of inner cup of calorimeter mcal, g 50 50 Specific heat of calorimeter Ccal, cal/(g °C) Specific heat of water Cw, cal/(g °C) 0.217 0.217 1.00 1.00 Mass of metal Mm, g 80 140 Mass of inner cup + water mcal + Mw, g 220 240 Mass of water Mw, g 170 190 Initial temperature of calorimeter and water to, °C Initial temperature of metal tm, °C 22 22 100 100 Final equilibrium temperature tr, °C 30 26 Thermal energy gain by calorimeter and water Qgain, cal Specific heat of metal Cm, cal/(g °C) Standard specific heat of metal Cst , cal/(g °C) 0.217 0.093 |% error Thermal energy lost = Thermal energy gained Thermal energy Q = cmAt %3D %3D Specific heat C |Thermal energy lost by metal = Thermal energy gained by (water + calorimeter) %3D EmMm(tm-tf)=(ccatMeat +CwMw)(tp- to) %3D (Ccaimcal+ Cymw)(tf- to). Gm = %3D Mm(tm - t;) |2.2 kg of ice (solid phase of water) at -10°C is heated under atmospheric pressure. Answer the following questions. Use the following values for your calculation. specific heat of ice: 2.1 kJ/(kg °C) specific heat of water: 4.2 kJ/(kg °C) specific heat of vapor: 2.0 kJ/(kg °C) latent heat of fusion: 334 kJ/kg latent heat of vaporization: 2260 kJ/kg How much heat is required to change the phase of the liquid water to vapor? How much heat is required to raise the temperature of vapor to 200°C?