How to calculate the molar enthelpy

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SUMMARY

This discussion focuses on calculating the molar enthalpy change for a reaction involving sodium hydroxide (NaOH) and sulfuric acid (H2SO4). The user conducted an experiment using 60 ml of 1.0 mol/L NaOH and 40 ml of 1.0 mol/L H2SO4, recording an initial temperature of 22.5°C and a maximum temperature of 26°C. The calculated change in molar enthalpy was determined to be 24.4 kJ/mol, which is significantly lower than the accepted value of 56 kJ/mol. The user suspects that the discrepancy may stem from experimental errors rather than calculation mistakes.

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Homework Statement



1) add 60 ml of 1.0 mol/L Sodium Hydroxide solution to a polystyrene calorimeter.
2) mix it with 40-ml sample of 1.0 mol/L sulfuric acid solution in a graduated cylinder.

3) Add the acid to the base, stirring slowly with the thermometer. record the highest temperature recorded

initial temp: 22.5
highest: 26

------------------------------------------------------
Cacluate the number of moles of the base (the limiting reagent)

2) Calculate the change in molar enthalpy with respect to sodium hydroxide.

Homework Equations





The Attempt at a Solution


I think, I solved it. n = c.v
n = 0.06 * 1 = 0.06 mol NaOH


2nd) H = m.c.t/n

100g * 4.184 * 3.5 / 0.06
= 24.4 KJ
is this correct?

the reason why I am confused is because the accepted value is 56kj/mol. My answers is way off. Wither I messed up during the experiment or in my writtten solution or in both
Plz help
 
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IMHO solution looks OK, so most likely there was something wrong with the experimental part.
 

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