A 17 g of -4.5 °C ice cube is put into a beaker with 350 mL of 78 °C hot water. Calculate the final temperature in the beaker. (enthalpy of fusion of water = 6.01 kJ/mol, specific heat capacity of liquid water = 4.184 J/g•°C, specific heat capacity of ice = 2.03 J/g•°C, density liquid water = 1.00 g/mL)

Solid carbon dioxide, more commonly known as dry ice, is directly converted to gas when heated instead of melting first. Adding warm water to dry ice is enough to promote this process.
Calculate the mass of dry ice added to 25.0 L of water at 70°C given that the dry ice completely sublimes when the water reaches 20°C. Assume no heat is lost to the surroundings. The ΔH°_f for CO₂(s) is -427.4 kJ/mol.

A 50.0-g block of an unknown substance initially at 177.39 °C was submerged in 40.0 mL of water initially at 10.0 °C. At thermal equilibrium, the temperature of both substances is 39.31 °C. Identify and calculate the heat capacity of the unknown substance.`

A 20.0-g block of aluminum at 110 °C and a 20.0-g block of gold at 10 °C are in contact with each other and isolated from the rest of the universe. Which statement applies for the final temperature of the blocks.

In an insulated container, a zinc block that was initially at 89.2°C was added to 75.0 g of water at 23.0 °C. When the mixture reached thermal equilibrium, its final temperature is 29.4 °C. What is the mass of the zinc block? (c_zinc = 0.388 J/(g∙°C))

If 50.0 mL of ethanol (density = 0.789 g/mL) initially at 7.0 °C is mixed with 50.0 mL of water (density = 1.0 g/mL) initially at 28.4 °C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?