I was trying to determine the standard enthaply change of neutralization for H_{2}SO_{4} and NaOH. In my reaction 58 cm^{3 }of H_{2}SO_{4 ,} c=(1,80 mol/dm^{3}) reacted with 1dm^{3 }NaOH c=0,162mol/dm^{3}. That means that 0,104 mol of H_{2}SO_{4 }reacted with 0,162 mol of NaOH. In my experiment I calculated standard enthaply change of neutralization and my result was -67241,79 J/mol. If i understand correctly my result should have been around -55.8 kJ/mol.

I would like to know what could have affected my result?

We used tehnicqe of calorimetry.

## Recheck calculations :

Recheck calculations :

Limiting reactant is NaOH and if you check balanced reaction...

2NaOH + H2SO4---->2H2O + Na2SO4

so the number of moles of H2O formed 0.162 mol

generally experimentallly calculated values are less than 55.8 KJ because some heat is always given off even in insulated system.Heat lost to the stirrer / thermometer and coffee cup calorimeter is also not 100 % insulated.So experimental value of heat is generally less than theoretical value.Please recheck the calulations.

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