When water is heated in an insulated container and reaches thermal equilibrium with its surroundings, which of the following statements is true?

If you combine 350.0 mL of water at 25.00°C and 100.0 mL of water at 95.00°C, what is the final temperature of the mixture, assuming no heat is lost to the surroundings?

An aluminum block initially at 25°C loses 2.89 x 10^3 J of heat. If the specific heat capacity of aluminum is 0.897 J/g°C and the mass of the block is 150 g, what is the final temperature of the aluminum?

A 101 g piece of aluminum (c_aluminum = 0.900 J/g°C) is heated to 128.1 °C and added to 62.6 g of water at an initial temperature of 24.2 °C. Assuming no heat is lost to the surroundings, what will the final temperature of the mixture be?

Ice cubes at exactly 0°C with a total mass of 54.0 g are combined with 140 g of water at 75°C in an insulated container. Given that the heat of fusion (ΔH_fus) is 6.02 kJ/mol and the specific heat capacity of water (c_water) is 4.18 J/g°C, what is the final temperature of the system if no heat is lost to the surroundings?

While water is in the process of freezing, what happens to its temperature?

Which energy changes are associated with a liquid freezing?

Which energy changes are associated with a liquid boiling?

Which equation is commonly used to calculate the change in thermal energy (q) of a substance during a temperature change?