CaCl₂(s) → Ca²⁺(aq) + 2Cl⁻(aq) ∆H = -81.5 kJ/mol A 15.0-g sample of CaCl₂ is dissolved in 265.0 g water with both substances at 25.0°C. Calculate the final temperature (in °C) of the solution assuming no heat loss to the surroundings and assuming the solution has a specific heat capacity of 4.184 J/°C･g.

Consider an unknown metal X with a mass of 67.5 g at an initial temperature of 76.1 °C. The metal is placed in 88.7 g of water initially at 20.5 °C in an insulated container. The final equilibrium temperature of the system is 32.1 °C. Calculate the specific heat (J/(g·°C)) of the metal X.   Use Cs = 4.18 J/(g·°C) for the specific heat of water. Assume that the only energy exchange that occurs is between the metal and 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 4.18 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.

The Δ?vapΔ⁢Hvap of a certain compound is 47.57 kJ·mol−147.57 kJ·mol−1 and its Δ?vapΔ⁢Svap is 67.46 J·mol−1·K−1.67.46 J·mol−1·K−1. What is the boiling point of this compound?

Answer the following question about an aqueous solution of tetrahydrofuran (C4H8O)with a concentration of 4.20 molal. The enthalpy of vaporization of tetrahydrofuran is 445.9 J/g. How much energy is required to convert the amount of tetrahydrofuran in the solution to vapor?

Question 16 ons What mass of nitrogen gas (N,) occupies a volume of 14.5L at 33 °C and 1.30 atm? Type your answer in the space provided and show your work on a separate sheet of paper. Edit View Insert Format Tools Table

8.96 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.

The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).

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).