Question

Table 4.2: Enthalpy of Neutralization for an Acid-Base Reaction Trial 1 Concentration of NaOH 1. i mol/L Initial temperature of NaOH 22.1°C Volume of NaOH Concentration of HCI 45, I mL 1.2 mol/L 22.3°C Initial temperature of HCI Trial 2 lol mol/L 21.9°C 63 mL 45. Iml 1,2 mol/L 22.5°C 45.2 mL 27.5° 22.2°C 5.3°C 90.3 mL 4.18 Jg! °C! Volume of HCI 45.3 ml Final temperature of mixture Average initial temperature (HCl and NaOH) Ti Temperature change, (47) 28.6°C 22.2°C 6.4°C 90.4mL 4.18 Jg' °C Mass of final mixture (assume density of mixture is 1.00 g/mL) Specific heat capacity for H20 (Cp) 2.418 103 qwater 2.00x10-3 qcal Gran Moles reacted of the limiting reagent AH(qrxn per mole reacted) Average AH, of both trials

Answer 1

The heat of the calorimeter is calculated:

q cal = Cal * ΔT = 31.4 J / ° C * 6.4 ° C = 200.96 J

Trial 2: 166.42 J

Reaction heat is calculated:

q rx = q water + q cal = 2418 + 200.96 = 2618.96 J

Trial 2: 2000 + 166.42 = 2166.42 J

The moles of reagent limit are 0.05 mol

The reaction enthalpy change is calculated:

ΔHrx = - qrx / n = - 2.62 kJ / 0.05 = - 52.4 kJ / mol

Trial 2: - 43.4 kJ / mol

Average = - 47.9 kJ / mol

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