Hello! This question is regarding the results I got for a Heat of Neutralization experiment. Sources online tell me that the accepted value of NaOH and HCl heat of enthalpy is about 53 to 57KJ but it seems that in all those cases, the reactants only had 1.0M... but mine had 2.0M... would this affect it at all? My experimental heat of neutralization was 34KJ... which would then give me a percent error of 38%!! This is terrible T__T
So the Heat of Neutralization experiment was performed by mixing 50.0mL of 2.0M HCl and 51.0mL of 2.0M NaOH. The following are the results and raw data collected:
Average initial temperature of reactants: 16.0 degC
Final product temperature: 24.2 degC
change in temp: 8.2degC
given heat capacity: 3.89 J/(g degC)
given density: 1.04 g/mL
combined product volume: 101.0mL
so in calculating heat transferred, Q: [101.omL] x [3.89 J/(g degC)] x [1.04 g/mL] x [8.2 degC] = 3400J
thus, corresponding heat of neutralization: (3400J) / (0.1 mol HCl reacting) = 34000 J or 34KJ
So the Heat of Neutralization experiment was performed by mixing 50.0mL of 2.0M HCl and 51.0mL of 2.0M NaOH. The following are the results and raw data collected:
Average initial temperature of reactants: 16.0 degC
Final product temperature: 24.2 degC
change in temp: 8.2degC
given heat capacity: 3.89 J/(g degC)
given density: 1.04 g/mL
combined product volume: 101.0mL
so in calculating heat transferred, Q: [101.omL] x [3.89 J/(g degC)] x [1.04 g/mL] x [8.2 degC] = 3400J
thus, corresponding heat of neutralization: (3400J) / (0.1 mol HCl reacting) = 34000 J or 34KJ