What mass of steam at 100oC must be mixed with 300 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 40oC? The specific heat of ice is 2220 J/(kg K), the specific heat of water is 4190 J/(kg K), the heat of fusion of water is 333 kJ/kg, the heat of vaporization of water is 2256 kJ/kg.

A 17.2 L aluminum pot filled to the brim with 8.58˚C water.  How many litres of water will overflow when the temperature of the water is raised to 73.8˚C [round your final answer to three decimal places]?  Note that the pot and the water will be in equilibrium at both temperatures. {volume coefficient of thermal expansion for water = 207 × 10-6 ˚C-1; volume coefficient of thermal expansion for aluminum = 70 × 10-6 ˚C-1}

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).

A 1040kg iron bar with a length of 2.00m and temperature of −45.25˚C is immersed in 50kg of liquid water at 90˚C. The specific heat of liquid water 4.186 kJ/(kg˚C), and the latent heat of fusion of water is 333kJ/kg. The specific heat of iron is 0.45kJ/(kg˚C) and its melting point is 1538˚C. The goal is to determine the final temperature of the system (iron+water) once it reaches thermal equilibrium, and also the state of each substance (solid, liquid, gas)   d) If you did (c) correctly, the iron will still be colder than 0˚C, so the system is not yet in thermal equilibrium. As the iron heat up more, the water, already at 0˚C, will cool down. How much mass of water becomes ice?  e) What is the final temperature of the system? f) Given the final temperature you have calculated for the system, what is the change in the length of the iron bar? (The coefficient of linear expansion of iron is 12x10–6 / ˚C ).

A cube of ice is taken from the freezer at -9.5 °C and placed in a 95-g aluminum calorimeter filled with 300 g of water at room temperature of 20.0 °C. The final situation is observed to be all water at 16.0 °C. The specific heat of ice is 2100 J/kg · C°, the specific heat of aluminum is 900 J/kg · C°, the specific heat of water is is 4186 J/kg·C°, the heat of fusion of water is 333 kJ/Kg. Part A What was the mass of the ice cube? Express your answer to two significant figures and include the appropriate units. ? Value Units m = Submit Request Answer

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?