A blacksmith uses the heat energy from an oven to heat steel and other metals. Increasing the temperature makes it easier to form a metal into a desired shape, such as a horseshoe. The blacksmith also uses cold water to cool a hot horseshoe to room temperature. A steel horseshoe of mass mshoe =0.50 kg at a temperature of 800 K ("red hot") is dropped into a bucket of water (mwater =1.0 kg) at 300 K (about room temperature). What is the final temperature of the horseshoe and the water? For simplicity, assume none of the water evaporates, so none of the water is converted to steam.
who uses a bucket of water ( mwater =1.0 kg, Twater i=300 K) to cool a hot, steel horseshoe. This time, he has a much larger horseshoe (mshoe =2.0 kg, Tshoe i=800 K, and notices that when he drops the horseshoe in the water, some of the water evaporates as steam. Assuming the final temperature of the horseshoe plus water plus steam is 100°C (_ 373 K), how much of the water is converted into steam?