SUMMARY
This discussion focuses on calculating the heat of formation for ammonium chloride (NH4Cl) using calorimetry. The experiment involved mixing 50ml of 1.51M ammonia (NH3) with 50ml of 1.59M hydrochloric acid (HCl), resulting in a temperature change (deltaT) of 8.6°C. A second part of the experiment involved dissolving 4.082g of NH4Cl in 100ml of water, yielding a deltaT of -2.8°C. Participants are guided to write out the chemical reactions and determine the heat capacity of the ammonium chloride solution to calculate deltaH per mole for each reaction.
PREREQUISITES
- Understanding of calorimetry principles
- Knowledge of chemical reaction equations
- Familiarity with heat capacity concepts
- Basic skills in stoichiometry
NEXT STEPS
- Calculate the heat capacity of the ammonium chloride solution
- Learn how to derive deltaH from calorimetry data
- Study the enthalpy changes for dissolution reactions
- Explore the concept of standard heat of formation
USEFUL FOR
Chemistry students, laboratory technicians, and educators involved in thermochemistry and calorimetry experiments.