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How many joules are given off when 120 g of water are cooled from 25ºC to - 25ºC.
SHC of ice is 2090J/kg SLHF is 335kJ/kg
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- At 25.0 m below the surface of the sea, where the temperature is 5.00C, a diver exhales an air bubble having a volume of 1.00 cm3. If the surface temperature of the sea is 20.0C, what is the volume of the bubble just before it breaks the surface?How much heat would flow into an 80 cm x 40 cm x 3.0 mm glass window each hour on a day when the outside temperature is 103 F and inside temperature is 70 F? Kglass = 0.84 W/m-K. O 1.64x10³ J/s O 2.96x10² J/s O 1.64x10² J/s O 2.96x10³ J/s2 kg of ice at 0°C are placed in a closed glass beaker (k=0.80 W/m-C). The closed beaker is then placed in a 30°C room. The surface area of the beaker is 5x10-3 m²; and its walls are 0.005m 5. thick. How much heat is required to melt the ice? How long does it take the ice to melt?
- KIkg, Cwater=4.18 kJ*K/, What will be the final temperature of 40 g of ice at 0 °C mixed with 375 g of water at 88 °C. kJ (Cice= 2.05 kg, Kork/ kg; Lfwater=333.5 K/ kg @ 0 °C, Lywater= 2257 kJIkg Cwater=4.18 kJ*K/, Csteam-2.01 @100 °C) T= °CAluminum is often melted down for recycling purposes. Assuming 1 kg of aluminum is at 20 deg C (room temperature), what is the minimum amount of heat needed to melt it to a liquid? The specific heat capacity of aluminum is 899 J/kg°C, the melting point is 660°C, and the latent heat of fusion is 3.97 x 105 J/kg. 972,000 J571,000 J397,000 J500,000 JA 355mL cup of hot chocolate has an initial temperature of 49°C. How many Calories of thermal energywill the liquid exchange if the drinker’s body temperature is 37°C? Assume hot chocolate is basicallywater. ??2? = 1???/??°C
- What is the outside temperature if 2.5x106 J of heat is lost through 4.0 m² of 3-cm thick glass (k = 0.8 J/smk) in one hour from a house kept at 20°C? 9.5⁰ 13.5⁰ O 5.5⁰ 11.5⁰ 7.5⁰An iron bucket has a mass of 2 kg and contains 8 kg of water. If the initial temperatureis 6 ° C, to what temp. will the bucket and water be raised by the addition of 3 kg ofwater at 95° C.s.h.c. iron = 500 J/kg° C,s.h.c. water = 4190 J/kg° C2kg of ice at 0 degree celsius are placed in a closed glass beaker( k = 0.80W/m-c). The closed beaker is then placed in a 30 degree celsius room The surface area of the beaker is 5x10-3 m² and its walls are 0.005m thick. How much heat is required to melt the ice? How long does it take the ice to melt?
- A 0.035-kg ice cube at -30.0°C is placed in 0.405 kg of 35.0°C water in a very well-insulated container. The latent heat of fusion for water is Lf = 79.8 kcal/kg. What is the final temperature of the water, in degrees Celsius? Tf =Suppose you want to raise the temperature of a 0.21-kg piece of ice from -20.0degrees Celsius to 130degrees Celsius. 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 times degree Celsius 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? Also, how much time, in seconds is required to do this, assuming a constant 20.0 kJ/s rate of heat transfer?A 6.0 kg zinc cannonball has been sitting in the desert sun all day. Its temperature is 49°C. Night falls on the desert, the wolf howls at the moon, and the temperature falls to a chilling -20°C. How much heat will the cannonball release as it cools to air temperature? (The specific heat of zinc is 390 J-kg^-1°C^-1). * O 1.6 x 10^5 J O 3.2 x 1015 J O 1700 J O 47000 J