**Data** 1. **Neutralization Reaction between NH₃ and HCl** | | Trial 1 | Trial 2 | |-----------------------|---------|---------| | Volume of NH₃, mL | 100.0 | 74.0 | | Volume of HCl, mL | 100.0 | 68.0 | | Molarity of NH₃, M | 1.60 | 0.80 | | Molarity of HCl, M | 1.60 | 0.70 | | Initial Temperature, °C | 20.0 | 20.0 | | Final Temperature, °C | 29.98 | 24.18 | | Enthalpy of Neutralization, KJ/mol | | | | Average Enthalpy of Neutralization, KJ/mol | | | **Explanation:** This table shows the data from a neutralization reaction experiment involving ammonia (NH₃) and hydrochloric acid (HCl). The experiment was conducted over two trials. Measurements include the volume and molarity of the reactants, as well as initial and final temperatures. Enthalpy of neutralization is a key outcome of interest, though specific values were not provided in the table. **Calculation Steps:** 1. For each neutralization reaction, write a complete balanced equation. 2. Calculate the number of moles of acid and the number of moles of base reacting using the molarity and the volume. 3. Based on the balanced equation for the neutralization and the answers for step 2, determine the limiting reactant (the acid or the base). 4. Assume that the density of the solution after mixing is 1.0 g/mL. Calculate the mass of the solution after mixing the acid and the base. 5. Assume that the specific heat capacity of the solution is 4.184 J/g°C. Calculate the heat absorbed by the solution (\(q_{\text{sol}}\)) using the formula: \[ q_{\text{sol}} = mC \Delta T \] where \(\Delta T\) is the difference between the final and initial temperatures. 6. Find the average of the heats derived from the two determinations for each neutralization. 7. We are assuming that heat is only transferred between the reaction and the solution. Therefore, the following equation applies: \[ q_{\text{rxn}} + q_{\text{sol}} = 0 \] - (a) Since you have found the average \(q_{\text{sol}}\) (step 6), determine the value of \(q_{\text{rxn}}\). - (b) Since pressure is constant, \(q_{\text{rxn}} = \Delta H\) per mole. 8. Find the molar heat of neutralization by dividing the answer in step 7b by the number of moles of the limiting reactant that was found in step 3. **Note:** You will write a full lab report for this lab exercise.