Two 20.0 g ice cubes at −21.0 ∘C are placed into 215 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, ?f, of the water after all the ice melts.

A 0.537 g sample of steam at 103.2 ∘C is condensed into a container with 5.60 g of water at 16.7 ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18  J g⋅ ∘C,, the specific heat of steam is 2.01  J g⋅ ∘C,, and Δ?vap=40.7 kJ/mol.

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

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05  kg of water decreased from 117  °C to 56.5  °C.  Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C