What is the Molar Enthalpy of Neutralization (ΔHn) in kJ/mol if 5.00 moles of HCl(aq) (acid) neutralized 5.00 moles of NaOH(aq) (base) and released 16396 J of heat?
16396/5 = ? and convert to kJ.
To find the molar enthalpy of neutralization (ΔHn) in kJ/mol, you need to calculate the heat released (ΔH) in joules and then convert it to kilojoules by dividing by the number of moles involved in the reaction.
Given:
- Moles of HCl(aq) = 5.00 mol
- Moles of NaOH(aq) = 5.00 mol
- Heat released (ΔH) = 16396 J
Step 1: Calculate the moles of heat released per mole of HCl
Divide the heat released by the moles of HCl:
ΔH per mole of HCl = ΔH / Moles of HCl
ΔH per mole of HCl = 16396 J / 5.00 mol
Step 2: Convert the units from joules to kilojoules
Since 1 kJ = 1000 J, divide the result from step 1 by 1000:
ΔH per mole of HCl (in kJ/mol) = (16396 J / 5.00 mol) / 1000
Now you can do the calculation to find ΔHn in kJ/mol.