Part B: Mass of calorimeter = 3.297 g Mass of calorimeter and water = 51.540 g Mass of unkown sample = 5.059 g Initial temperature of water = 19.3 °C Final temperature of water = 26.0 °C

Specific Heats of Substances Substance Specific Heat g-°C Brick 0.20 Ethanol 0.58 0.10 pooM Calculate the amount of heat, in calories, that must be added to warm 70.9 g of brick from 19.3 °C to 41.0 °C. Assume no changes in state occur during this change in temperature. heat added: cal Calculate the amount of heat, in calories, that must be added to warm 70.9 g of ethanol from 19.3 °C to 41.0 °C. Assume no changes in state occur during this change in temperature. heat added: cal

3.56 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.

A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 156 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 degrees Celsius. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures.

3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 11.81°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･°C and the density of the solution is 1.20 g/mL).

calculate the amount of heat released by 23.0g of water when its temperature is cooled from 68.0'C to 31.0'C. the specific heat of water is 4.18 j/g'c