A calorimeter contains 100. g of water at 22.5°C. A 20. g sample of NH4NO3 is added to the water in the calorimeter. After the solid has dissolved, what is the temperature of the water? The enthalpy of solution for dissolving ammonium nitrate is 25.41 kJ/mol. And the MM is 80.04g. Assume that no heat is lost to the calorimeter or the surroundings and that the heat capacity is 4.18 J/g°C for solution (the same as that of pure water).

Using this reversible reaction, answer the questions below: n2o4 2no2 (colorless) (reddish-brown) -as the temperature increased, what happened to the n2o4 concentration? -was the formation of reactants or products favored by the addition of heat? -which reaction is exothermic? right to left or left to right? -if the change of enthalpy of this reaction when proceeding left to right is 14 kcal, which chemical equation is correct? n2o4 2no2 + 14 kcal n2o4 2no2, hr = +14 kcal n2o4 + 14 kcal 2no2 n2o4 2no2, hr = -14 kcal