A sample of 27.8 g of ammonium nitrate, NHẠNO3, was dissolved in 130.2 g of water in a coffee cup calorimeter. The temperature changed from 28.94 °C to 16.51 °C. Calculate the heat of solution of ammonium nitrate in kJ/mol. Assume that the energy exchange involves only the solution and that the specific heat of the solution is 4.18 J/g°C. Heat of solution = i kJ/mol

In a coffee cup calorimeter, 40.0 mL of 0.33 M nitric acid (HNO3) and 40.0 mL of 0.33 M potassium hydroxide (KOH) are mixed to observe the heat released during the neutralization reaction. Based on the data in the table, what is the enthalpy of the neutralization reaction between HNO3 and KOH? Initial temperature in the calorimeter (°C) Final temperature in the calorimeter (°C) Final mass of the neutralized solution (g) Calorimeter constant (J/C)) 21.3 23.5 79.74 4.57

A 5.71 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. Was the dissolution process endothermic or exothermic?

A 5.71 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. What quantity in moles of the unknown salt were used in the reaction?