Calculate the amount of heat required for the melting of 10.0 kg at −10∘C. Given that latent heat of fusion of ice is 3.3×105J/kg and specific heat capacity of ice is 2.2×103J/kg∘C.
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Calculate the amount of heat required for the melting of 10.0 kg at −10∘C. Given that latent heat of fusion of ice is 3.3×105J/kg and specific heat capacity of ice is 2.2×103J/kg∘C.
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- Suppose you want to raise the temperature of a 0.185-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. Part (a) How much heat, in kilocalories, must be transferred for this to happen, including the energy needed for phase changes? Part (b) How much time, in seconds, is required to do this, assuming a constant 20.0 kJ/s rate of heat transfer?A piece of metal with a mass of 5.05 g originally at 25.5°C is dropped into 25 g of water originally at 82.7°C. The final temperature of the metal and the water is 81.5°C. Determine the specific heat of the metal and consult Table 5.2 to determine its possible identity.The quantity of heat Q that changes the temperature deltaT of a mass m of a substance is given by Q=cmdeltaT, where c is the specific heat capacity of the substance. For example, for H2O, c=1cal/g degree C. And for a change of phase, the quantity of heat Q that changes the phase of a mass m is Q-mL, where L is the heat of fusion or heat of vaporization of the substance. For example, for H2O, the heat of fusion is 80 cal/ g and the heat vaporization is 540 cal/g. Part A: Use these relationships to determine the number of calories to change 0.60 kg of 0 degree C ice to 0 degree C ice water. Part B: Use these relationships to determine the number of calories to change 0.60 kg of 0 degree C ice water to 0.60 kg of 100 degree C boiling water. Expresss your answer to two significant figures and include appropriate units.
- 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 heavy pot made of copper has a mass of 2.24 kg (including the lid) and is heated in an oven to a temperature of 154 °C. You pour 0.12 kg of water at 26.0 °C into the pot and quickly close the lid so that no steam can escape. We assume that no heat is lost to the surrounding. For copper, Ccopper 390 J/(kg.K) For water, Cwater 4190 J/(kg.K), L, = 2256 kJ/kg, L; = 333 kJ/kg. %3D What is the final mass of steam in the pot? onIce at 0 °C is placed in a Styrofoam cup containing 0.62 kg of lemonade at 32 °C. The specific heat capacity of lemonade is virtually the same as that of water; that is, c = 4180 J/(kg C°). After the ice and lemonade reach an equilibrium temperature, some ice still remains. The latent heat of fusion for water is Lf = 3.35 x 105 J/ kg. Assume that the mass of the cup is so small that it absorbs a negligible amount of heat, and ignore any heat lost to the surroundings. Determine the mass of ice that has melted, in grams.
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