A 815-g metal ball absorbs 5.750 kJ of thermal energy. If the specific heat capacity of the metal is 0.292 J/(g °C) and the final temperature of the metal ball is 76.5 °C, what is the initial temperature in °C?

A 10.5-g ice cube at 0°C is placed onto a 245-g block of aluminum. Calculate the temperature change of the aluminum upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the aluminum. The specific heat capacity of aluminum is 0.897 J/g°C and the heat of fusion of ice is 334 J/g. What is the temperature change of the aluminum?

A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.231 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol∙°C. (Atomic mass of gold = 197 g/mol)

A 40.0 gram block of an unknown metal is cooled to -20.0 °C in a laboratory freezer and then immediately dropped into 140.0 grams of 24.0 °C water in an insulated container. If the final temperature of both the block and water is 22.7 °C, what is the specific heat capacity of the metal?

A 45.0 g aluminum spoon (specific heat 0.88 J/g °C) at 24 °C is placed in 180 mL (180 g) of coffee at 85 °C, and the temperature of the two becomes equal. What is the final temperature when the two become equal? Assume that coffee has the same specific heat as water (4.18 J/g °C).

A 90.0 g piece of metal, initially at 98.60 °C, is placed into 120.0 g of water initially at 24.30 °C. If the final temperature of the water is 34.00 °C, what is the specific heat capacity of the metal? (The specific heat of water is 4.184 J/g·°C).

A sample of aluminum metal absorbs 11.2 J of heat, causing its temperature to increase from 23.2 °C to 30.5 °C. Given that the specific heat capacity of aluminum is 0.90 J/g-K, what is the mass of the sample in grams?

A volume of 75.0 mL of H2O is initially at room temperature (22.00 °C). A chilled steel rod at 2.00 °C is placed in the water. If the final temperature of the system is 21.10 °C, what is the mass of the steel bar? Use the following specific heat capacities: c_water = 4.18 J/g°C, c_steel = 0.452 J/g°C.

Given that the heat of fusion of water is 6.02 kJ/mol, the heat capacity of H2O(l) is 75.2 J/mol·K, and the heat capacity of H2O(s) is 37.7 J/mol·K, calculate the total heat required to convert 1 mole of ice at -10°C to liquid water at 0°C.