A 400 g piece of copper initially at a temperature of 500°C is placed in 300 g water at 60.0°C. Calculate the mass of water that boils away.

In an insulated container of negligible mass, a 4.00-kg piece of iron at an unknown initial temperature is placed with 3.00 kg of ice at -30.0°C. After reaching thermal equilibrium, the container holds 2.20 kg of ice and 0.80 kg of liquid water. Determine the initial temperature of the iron. Use the Specific heat capacity of ice, 𝑐_𝑖=2.1J/g°C, the Specific heat capacity of iron, 𝑐_Fe=0.45 J/g°C, Latent heat of fusion of ice, 𝐿_𝑓=334 J/g.

A science experiment involves a student with a mass of approximately 75.0 kg and a body temperature of about 38.0 °C drinking half a liter of water at 8.00 °C at the beginning. What will his new body temperature be after reaching thermal equilibrium? Assume that there's no metabolic heating during this period. The specific heat capacity for human bodies is typically around 3480 J/kg⋅K. The specific heat capacity of water is 4186 J/kg⋅K.

In a laboratory experiment, a researcher takes a cube of ammonia from a freezer set to -100.0°C and places it into a 100 g silver calorimeter containing 500 g of water. The water is initially at room temperature, 25.0°C. After some time, the system reaches thermal equilibrium, with all the water at 10.0°C. Given this information, determine the mass of the ammonia cube used in the experiment. Use specific heat capacity of ammonia (solid) = 2.09 J/g^.°C, specific heat capacity of ammonia (liquid) = 4.70 J/g^.°C, specific heat capacity of silver = 0.235 J/g^.°C, specific heat capacity of water = 4.18 J/g^.°C, and heat of fusion of ammonia = 332 J/g.