When 2.045 g of NH4NO3 (molar mass is 80.05 g/mL) is added to 100.0 mL of water at 25.09C, the final temperature of the water is 23.03C. What is the molar heat of solution (H) of NH4NO3 in kJ/mol?

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

When 40.00 grams of fictional compound X is added to water to make 236.0 grams of solution, the temperature increases from 19.05 °C to 63.46 °C. What is the heat of solution for compound X (in kJ/mol) given that the molar mass of compound X is 73.87 g/mol. Assume the specific heat capacity of the solution is 4.18 J/g°C.

A constant pressure calorimeter contains 286 g of water at 20.0 °C. A 13.41 g of substance X (molar mass 154 g/mol) at 20.0°C was dissolved in this water.  The temperature of the solution increased to 23.5 °C. Assuming the specific heat of the mixture is 4.184 J g‑1°C‑1, and the density of the solution is 1.00 g/cm3, calculate the enthalpy change (in kJ) for the dissolution of 1 mole of X.

Which of the molecules below would produce the following H-NMR spectrum?   Select one: 1. A 2. D 3. B 4. E 5. C

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.

When a 6.00 g6.00 g sample of KClKCl is dissolved in water in a calorimeter that has a total heat capacity of 4.47 kJ⋅K−1,4.47 kJ⋅K−1, the temperature decreases by 0.310 K.0.310 K. Calculate the molar heat of solution of KCl.

Cold packs (like the kind used by athletes to treat sprains and other minor injuries) rely on the fact that the enthalpy of dissolution of ammonium nitrate is positive. Is this an exothermic or endothermic reaction? Exothermic Endothermic Neither because this is a closed system and therefore no heat is lost.