Don't provide handwritten sollution ...   A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium the temperature of the water and metal was 33.5 °C. Using the specific heat of water (4.184 J/g °C), calculate how much heat flowed into the water

5.21 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.

An enthalpy of solution discusses the enthalpy change of dissolving an ionic compound in water.  8.31 grams of NaOH is added to 152.5 mL of H2O at 298 K. What is the final temperature of this solution after the salt dissolves if the enthalpy of solution for NaOH is -44.5 kJ/mol? The heat capacity of water is 4.184 J/ (g K) and the density of water is 1.00 g/mL.

When 30.87 grams of fictional compound X is added to water to make 438.9 grams of solution, the temperature increases from 26.23 °C to 62.34 °C. What is the heat of solution for compound X given that the molar mass of compound X is 130.58 g/mol? Assume the specific heat capacity of the solution is 4.18 J/g°C.     -280.2 kJ/mol     280.2 kJ/mol     -66.24 kJ/mol     4.649 kJ/mol     66.24 kJ/mol