Enthalpy Change for the Decomposition of Ammonium Chloride, Lab Reports of Chemistry

Download Enthalpy Change for the Decomposition of Ammonium Chloride and more Lab Reports Chemistry in PDF only on Docsity! Enthalpy Change for the Decomposition of Ammonium Chloride Purpose To determine the calorimeter constant (J/°C). To determine the enthalpy of neutralization and dissolution (J/mol) for reactions. Results Experiment 1 data Volume of cold water in the calorimeter 45.00 ml Initial temperature of the cold water (°C) 21.50 °C Volume of hot water added to the calorimeter (ml) 45.00 ml Initial temperature of the hot water (°C) 60.00 °C Final temperature in the calorimeter (°C) 34.90 °C Experiment 1 data analysis Mass of water calculation = density * volume: 45.00 ml * 1 g/ml = 45.00 g of water Q=mC*AT Q hot = 45.00 g * 4.184 J/g*°C * (34.90 °C- 60.00 °C) = - 4725 I Q cota = 45.00 g * 4.184 J/g*°C * (34.90 °C- 21.50 °C) = 2522 J Q ea = -(Q cots + Q not) Qea =-( 2522 J-4725 J) = 2203 J AT ca = 34.9 °C —21.50 °C =13.4 °C C ca = Q ea /AT; 2203 J/ 13.4 C = 164.4 J/ °C Experiment 2 data Volume of HC! solution in the calorimeter 25.00 ml (ml) Volume of NH; solution added (ml) 25.00 ml Final temperature in the calorimeter (°C) 29.00 °C HCI concentration 2.00 M. NH; concentration 2.00 M Experiment 2 data analysis HCI + NH3 --> NH4C1 2M * 0.025 L of NH3 = 0.050 moles of NH3