How much heat is absorbed when the temperature of a 4.1 g copper coin increases from 15.3 °C 74.6 °C? The specific heat of copper is 0.385 J/g°C.

How much heat must be added to a 38-g sample of aluminum to increase its temperature by 250.0°C? The specific heat capacity for aluminum is 0.902 J/g°C.

What is the specific heat of a 45.51 g piece of an unknown metal that exhibits a 45.2 °C temperature change upon absorbing 1870 J of heat?

A material has a specific heat of 0.625 J/g°C.  A 75.6 g sample of this material is heated  and them placed in 35.2 g of water at 21.4 °C.  The temperature of the water rises to 32.7 °C.  What was the initial temperature of the material?

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

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 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C.   If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt?   How many moles of the unknown salt were used in the reaction ?     _______ J?

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?