Challenge Problem!!! Two 20.0 g ice cubes at -11.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) 37.7 J/(mol·K) 75.3 J/(mol-K) T₁ = enthalpy of fusion of H₂O 6.01 kJ/mol C

Why are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.

The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.

A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0C. The reaction is 2Na(s)+2H2O(l)2NaOH(aq)+H2(g)H=368kJ Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/gc, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.