The specific heat of water is 4.184 J/g0C. The density of both HCL and NaOH is 1.00 g/mL
Assume that specific heats HCL and NaOH are also 4.1984 J/g C.
For Trial 1
To calculate the heat actually evolved, use the formula
q = m c Δt
To convert ml to grams, multiply volume with density (m = V X D)
(100 mL + 100 mL) = 200 mL of solution
100 mL X 1 g/ml = 2 00 grams of solution.
Find the temperature change.
Δt = t final – t initial = 40 0C – 24 0C =160C
q = m c Δt
q = 200 grams X 4.184 J /g0C x 16 0C
q= 13388.8 J
q = 13.39KJ
This is the heat gained by the water, but in fact it is the heat lost by the reacting HCl and NaOH, therefore q = - 13.39KJ
Moles of HCl = 0.278
Moles of NaOH = 0.25
NaOH is limiting reagent
Enthalpy of neutralization /mol of limiting reagent = -13.39KJ /0.25
=- 52.56 KJ/mol
For Trial 2
Δt = t final – t initial = 38 0C – 23.5 0C =14.50C
q = m c Δt
q = 200 grams X 4.184 J /g0C x 14.5 0C
q= -12133.6 J
q = - 12.13KJ
Moles of HCl = 0.278
Moles of NaOH = 0.25
Enthalpy of neutralization /mol of limiting reagent = -12.13KJ /0.25
=- 48.52 KJ/mol
For Trial 3
Δt = t final – t initial = 38 0C – 22.5 0C =15.5 0C
q = m c Δt
q = 200 grams X 4.184 J /g0C x 15.5 0C
q= 12970.4 J
q = -12.97KJ
Enthalpy of neutralization /mol of limiting reagent =- 12.97KJ /0.25
= -51.88 KJ/mol
Mean enthalpy of neutralization /mol of limiting reagent
= (-52.56 KJ/mol + -48.52 KJ/mol +-51.88 KJ/mol ) /3
Mean enthalpy of neutralization /mol of limiting reagent - 50.99 KJ/mol
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