Answer in Organic Chemistry for emily #119311
April 21st, 2023
Dissolution of ammoinum nitrate is endothermic (positive enthalpy value), so temperature decreases. In real life he added more salt than should be added, so the registered temperature change will be larger. When he calculates the experimental enthalpy change normalized per 1.0 g, he will get higher enthapy than the accepted one. Because to get the correct enthaply he should had normalized it per 1.5 g ammonium nitrate.