Heat of Solution

Results:

Figure.1: Temperature (Co) vs. time (min) graph for part A, trial 1

Figure.2: Final report Data for part A, trial 1

Figure.3: Temperature (Co) vs. time (min) graph for part A, trial 2

Figure.4: Final report Data for part A, trial 2

Figure.5: Temperature (Co) vs. time (min) graph for part B

Figure.6: Final report Data for part B

Figure.7: Temperature (Co) vs. time (min) graph for part C

TRIS Standardization for Trials 1 & 2
	Trial 1	Trial 2
Mass of TRIS in (g)	0.5003	0.5091
Initial Temp in	25.3290	25.1794
in ()	0.2812	0.2717
in (cal)		-29.309
in (
	106.001

Table 1: Part A Calculated data

Exothermic Heat of Neutralization
Initial Temp in	25.270
()	1.668
(cal)	-

Table 2: Part B Calculated data

Endothermic Heat of Neutralization
Mass of KNO3(g)	0.7005
Initial Temp in	24.82
()	-0.47
(cal)

Table 3: Part C Calculated data

Sample Calculations:

Part A: Standardization with TRIS for Trial 1

HCl Volume calculation:

Temperature rise 1st trial:

Calorimeter’s Heat Capacity () calculation

Heat Capacity of the Calorimeter () for 2nd trial:

, and

Thus,

Average for part A:

Part B: Calculations: Exothermic Heat of Neutralization

Calculation:

Where is the average value of part A and is for part B

Limiting reactant and its number of moles:

NaOH mole calculation:

HCl: mole calculation:

Since the number of moles of NaOH is greater than the number of moles for HCl, HCl is the limiting reactant.

in :

For Neutralization reaction calculation:

Where, Cs is the value of part A and is the value of part B.

Part C: Endothermic Heat of Solution

for KNO3 solution calculation

Where is part A value and is for part C value.

in :

Where is the molecular weight of KNO3 and is the mass of KNO3 in gram.

for solution calculation:

Literature value calculation:

Exothermic Heat of Neutralization

Number of moles for NaOH:

Number of moles for H2O:

ΔHLiterature (22.24) [3] = -470.198 kJ/mol = -112.38 kcal /

Number of moles for HCl:

Number of moles for H2O:

ΔHLiterature () [2] = -166.272 kJ/mol = -39.74

Number of moles for NaCl:

Number of moles for H2O:

ΔHLiterature () [2] = - 406.923 kJ/mol = 97.26 kcal/mol of NaCl

ΔH of H2O = -285.830 kJ/mol = - 68.32 kcal/mol

ΔHrxn= ΔH(products) – ΔH(reactants)

ΔHrxn= [-406.923 - 285.830] - [-470.198 - 166.272]

= -56.283 kJ/mol = -13.452 kcal/mol

Endothermic Heat of Solution

c = -118.22 kcal/mol

Number of moles for KNO3:

Number of moles for H2O:

ΔHLiterature () [3] = -459.784 kJ/mol = -109.89 kcal/mol of KNO3

ΔHrxn= ΔH(products) – ΔH(reactants) = [- 109.89] - [-118.22] = 8.33 kcal/mol

Infinite Dilution

ΔH∞ = ΔHrxn[2] = [-97.34-68.315] - [-112.36-39.952] = -13.343 kcal/mol

ΔHneutr.rxn = -13.452 kJ/mol

Differences in ΔH= (-13.452) – (-13.343) = 0.109 kJ/mol

Error Analysis

Percentage error in ΔH

% error in =

% error in =

Dissection

Reaction	ΔH Experimental	ΔH Literature
		-13.452
		8.33

Table (4): ΔH Experimental and Literature values