How much heat is required to melt a 1.5-kg piece of ice and then warm up the water released by the melting ice to the room temperature 20 oC? Assume that initially the piece of ice was at temperature of -22.3 oC. The specific heat of ice is 2093 J/kg oC; the specific heat of water is 4186 J/kg oC, and the latent heat of fusion of water is 3.34x105 J/kg. Give answer in Joules.

How much heat energy needs to be given up to freeze 2.12 kg of milk if initially the milk was at the room temperature 20 oC? Assume that the latent heat of fusion of milk is 275700 J/kg, and the specific heat of milk is 3890 J/kgoC.

Consider the following selected properties of water: Consider the following selected properties of water: Density (liquid water): d = 1.00 g/mL Heat of fusion: AHfus = 6.01 kJ/mol Heat of vaporization: AHvap = 40.67 kJ/mol Specific heat (liquid water): Cp = 4.184 J/(g-K) = 4.184 J/(g-°C) How much heat is needed to completely evaporate 36 mL of water at its normal boiling temperature? 47 J 81 J 47 kJ 110 kJ 81 kJ

An aluminum block has a mass  of 200g and a temperature of 400°C, it is then dropped into an aluminum calorimeter of mass 1.0 Kg filled with 100 g of water at a temperature of 5.0°C. What is the the temperature when equilibrium is reached. Given: specific heat of aluminum is 0.22 kcal/(kg-°C) specific heat of water is 1.00 kcal/(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

In an insulated vessel, 239 g of ice at 0°C is added to 635 g of water at 15.0°C. (Assume the latent heat of fusion of the water is 3.33 x 10° J/kg and the specific heat is 4,186 J/kg · °C.) (a) What is the final temperature of the system? °C (b) How much ice remains when the system reaches equilibrium?

An ice block of mass 1.2000000000000002 kg at an initial temperature of –11 ∘C is put into a copper pot of mass 2.5 kg containing 4.3 L of water at 21 ∘C. If you heat up the pot, what is the amount of energy (in J) you need to convert all the ice and the water into steam? (Assume that no energy is lost from the system.)   You may need some or all of the following constants: The specific heat of ice is 2200 J/kg ∘C, the specific heat of copper is 386 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg and the heat of vaporization for water is 2256000 J/kg .