A coffee cup calorimeter contains 100.0mL of 1.50 M Ba(NO3)2 at 25.0 degrees Celsius. A student pours 100.0mL of 1.50 M Na2SO4 at 25 degrees Celsius into the calorimeter. A precipitate forms and the temperature rises to 29.7 degrees Celsius. Assume that no heat was lost to the surroundings, the volumes were additive, the specific heat capacity of the solution was 4.184 j/gal and the density of the solution was 1.00 g/mL. A) this reaction could be represented as a complete ionic or a net ionic equation. Write the balanced chemical equation that should be used in association with the value for this reaction.
B) find the amount of the heat that was last or gained by the solution in the calorimeter.
C) find the heat of reaction
D) is the reaction endothermic or exothermic?