Two 20.0 g ice cubes at −16.0 ∘C are placed into 225 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts.   heat capacity of H2O (s) 37.7 J/(mol⋅K) heat capacity of H2O (l) 75.3 J/(mol⋅K) enthalpy of fusion of H2O 6.01 kJ/mol   Tf= ________∘C

Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C.What was the initial temperature change of the ice? The specific heat capacity of H 2 O(s) = 2.1J/(g·ºC)

Suppose you have a perfectly insulated container holding 2.00 kg of liquid water at a temperature of 20.0°C. You also have a large supply of ice cubes which are stored at a temperature of-20.0°C. (a) What is the maximum mass of ice you can add to the water so that all of the ice melts? Assume no heat is lost to the environment. (b) Suppose you add twice the mass of ice that you found in part a. How much solid ice will remain once thermal equilibrium is reached?

Two 20.0 g ice cubes at -17.0 °C are placed into 235 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/ (mol·K) heat capacity of H,O(1) 75.3 J/ (mol·K) T = enthalpy of fusion of H,O 6.01 kJ/mol