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GCSE Assessment - Investigation into Enthalpy of Neutralisation Introduction - The aim of this investigation is to show that heat of neutralisation is an exothermic reaction which produces water. The amount of energy given out for one mole of water is about -57.3 kJ/mol. This needs to proven by this experiment as well. Results Stage One These are the results I gained from the titration. Titrant (HCl) Rough 1 2 Initial (cm³) 12 10 22 Final (cm³) 22.5 20.7 32 Titre (cm³) 10.5 10.7 10 Stage Two The results gained are as follows: Time (s) Temp for expt.1 (ºC) Temp for expt.2 (ºC) Average temp (ºC) 0 16 16 16 5 18.2 18 18.10 10 25.1 24.9 25 15 28.5 27.8 28.15 20 29.4 28.9 29.15 30 29.5 29.1 29.3 40 29.5 29.1 29.3 50 29.5 29.1 29.3 60 29.5 29.1 29.3 70 29.5 29.1 29.3 80 29.5 29.1 29.3 90 29.5 29.1 29.3 100 29.5 29.1 29.3 120 29.2 29.1 29.15 140 29.0 28.9 28.95 160 28.6 28.2 28.4 180 27.9 27.7 27.8 200 26.8 26.9 26.85 220 26.1 26.3 26.2 240 25.5 25.7 25.6 Calculations for Stage One Concentration of NaOH Moles = Mass Molar mass Moles = 8g (23+16+1) = 40 = 0.2 Therefore concentration of NaOH is 0.2 mol/dm³. Concentration of diluted bench HCl Moles of NaOH in 10cm³ = V × C = 10 ×0.2 = 0.002 moles 1000 1000 Equation NaOH + HCl › NaCl + H2O Moles 1 1 Vol/cm³ 10 10.4 ‹ This figure is the average titre gained from Stage One. Conc. g/dm³...

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