. A piece of an iron metal of unknown mass is heated to 325.9 o C and then placed in a styrofoam coffee cup containing 225.2 mL of water at 22.15 o C. After the system comes to thermal equilibrium, the temperature of the water is 29.65 o C. Assuming that no heat is lost to the cup or the surroundings, determine the mass of the iron metal. The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C. The density of water is 1.000 g/mL.

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. A piece of an iron metal of unknown mass is heated to 325.9 o C and then placed in a styrofoam coffee cup containing 225.2 mL of water at 22.15 o C. After the system comes to thermal equilibrium, the temperature of the water is 29.65 o C. Assuming that no heat is lost to the cup or the surroundings, determine the mass of the iron metal. The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C. The density of water is 1.000 g/mL. 

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