Use the following calorimetric values to answer the question: The specific heat capacity of water is 4,186 J/kg°C. The specific heat capacity for copper is 387 J/kg°C.

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

A 87.9 g chunk of limestone (specific heat: 0.22 J/g°C) is heated to 231.9 °C and dropped into a beaker containing 300.0 g of water (specific heat: 4.184 J/g°C) at 20.2 °C.What will be the final temperature of the system after it reaches thermal equilibrium?

A nickel at 30 °C is dropped into a glass of 15.0 g soda at 3.0 °C, if the heat capacity of the nickel is 4.40 J/°C, the heat capacity for the glass is 11.1 J/°C, and the soda has the same specific heat capacity as water (4.184 J/g°C), what is the final temperature of the mixture?

A student conducted several calorimetry investigations. In the first of the investigations, the student heats a 21.0 g price of metal that is know to have a specific heat capacity of 0.449 J/g°C to a temperature of 80°C. Then a piece of metal is added to the beaker of water (70.0 grams at 20.00°C). The specific heat capacity of water is 4.187 J/g°C. If the student repeated the investigation with 50.0 g of water instead what would be different.

A 120.0 g sample of a metal at 75.0 °C is added to 150.0 g H20 at 15.0 °C. The temperature of the water rises to 18.3°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. Specific heat capacity for water is 4.18 J / °C g.