As the calorimeter is completely insulated, heat released during the neutralisation reaction of the acetic acid and sodium hydroxide is absorbed by the solution of the two and the aluminium cup.
Mass of solution=Mass of acetic acid+Mass of sodium hydroxide
=59.21 g+50.03 g=109.24 g
Rise in temperature of the solution=Rise in temperature of the Aluminium cup=Final temperature of solution-initial temperature of the solution
=26.8°C-19.9°C=6.9°C
Heat absorbed by the solution and the calorimeter
=Mass of solution x specific heat of solution x rise in temperature of solution + Mass of aluminium cup x specific heat of aluminium cup x rise in temperature
=109.24 gx4.184 J/g°C x6.9°C+41.55 g x 0.903 J/g°Cx6.9°C
=3153.71 J+258.89 J
=3412.60 J
Heat released in the neutralisation reaction of acetic acid and sodium hydroxide=-heat absorbed by the solution
=-(3412.60 J)
=-3412.60 J/1000 J/kJ=3.412 kJ (1 kJ=1000 J)
Molar mass of acetic acid (CH3COOH)=2xMolar mass of C+4xMolar mass of H+2xMolar mass of O=2x12 g/mol+4x1 g/mol+2x16 g/mol=24 g/mol+4 g/mol+32 g/mol=60 g/mol
Number of moles of acetic acid=Given mass/Molar mass
=59.21 g/60 g/mol=0.99 mol
Molar mass of sodium hydroxide (NaOH)=Molar mass of Na+Molar mass of O+Molar mass of H=23 g/mol+16 g/mol+1 g/mol=40 g/mol
Number of moles of sodium hydroxide=Given mass/molar mass=50.03 g/40 g/mol=1.25 mol
The balanced chemical equation for reaction between acetic acid and sodium hydroxide is
As per the balanced chemical reaction
1 mol acetic acid reacts with 1 mol NaOH
So 0.99 mol acetic acid reacts with 0.99 mol NaOH
But we have 1.25 mol NaOH which is more than the required amount
So acetic acid is the limiting reagent
So molar enthalpy of neutralisation=heat released in neutralisation/number of moles of acetic acid
=-3.412 kJ/0.99 mol=-3.45 kJ/mol
The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M...
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