450 g of water at 10°C is in a pot on the stove. A block of ice with mass 225 g that is originally at -10°C is placed in a second identical pot on the stove. Heat is then added to the two samples of water at two different but constant rates. Assume that the heat is transferred immediately to the ice or water (in other words, neglect the increase in temperature for the pots). We will also neglect evaporation. The ice melts and becomes water, and you observe that both samples of water reach 60.0 °C after 11 minutes. The specific heat of liquid water is 4186 J/(kg °C), and of solid water is 2060 J/(kg °C). The latent heat of fusion of water is 3.33 x 10^5 J/kg.
Heat continues to be supplied to the two pots at constant rates beyond the time when they have equal temperature. When the water in the second pot reaches 80°C, what is the temperature of the water in the first pot?