Heat of Solution

Heat of Solution

Objectives:

This experiment aimed to determine the heat of the solution of different ionic compounds using water as a solvent and to establish whether the dissolving procedure results in exothermic or endothermic reactions.

 Introduction/Overview/Background

The heat of the salt solution in water may be measured by dissolving a specific amount of the salt in a specific amount of water and noting the temperature change with a thermometer. The temperature change can measure the heat of the solution. When the mark q is given, the chemical and physical changes include heat release or absorption. The absorption of heat implies that the variation is endothermic and is marked using a positive mark. Heat release implies that the change is exothermic and is marked using a negative mark. Therefore, for endothermic reactions, it’s (q>0) and (q<0) for exothermic. When the pressure in the system is constant, the heat flow is equal to the total heat.

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 Materials used:

Goggles and apron

Distilled water

Thermometer

Stirring rod

CaCl₂, NAOH, KOH

MgSO₄

Graduated cylinder

Foam cup as a calorimeter

Balance

NH₄CL,NH₄NO

CH₃CO₂Na,NaHCO₃,NH₄NO₃

Procedure:

1. Measure 100.0 ml of distilled water at room temperature and pour it into the plastic foam cup. Record the temperature of the water in the data table to the nearest 0.1
2. Measure a mass of 8-10 grams of calcium chloride using the laboratory balance on paper. Record the mass to the nearest 0.01g.
3. Shake the NH₄CL from the paper into the water and stir slowly with the stirring rod until the solid dissolves.
4. Ensure that the bulb of the thermometer is completely immersed in the liquid. If the temperature increases, record the highest temperature reached. If the temperature reduces, record the lowest temperature reached.
5. Please remove the solution by pouring it down the drain, rinse the cup, and return it and the thermometer to the lab bench.
6. Repeated steps 2-5 using calcium chloride

 Results and Discussion:

Solute	Solute mass (g)	Mass of water (g)	Mass of solution (g)	Initial T(C)	Final T	rxn/mol	Exothermic/ Endothermic
NH4NO3 Trial 1	7.549	100g	107.549	21.7	16.3	25.768	endothermic
Trial 2	8.066	100g	107.066	21.2	15.4	26.019	endothermic
Trial 3	7.949	100g	107.949	21.4	15.5	26.8	endothermic
Average ∆Hrxn/mol=+26.20                         literature value=+25.7 % ERROR=2%
CaCl2 Trial 1	7.279	100g	107.279	21.5	30.6	-62.265	exothermic
Trial 2	8.051	100g	108.051	21.6	32.2	-66.06	exothermic
Trial 3	8.018	100g	108.018	21.4	31.5	-63.2	exothermic
Average ∆Hrxn/mol=-63.84                          literature value=-81.3 % ERROR=22%
NaOH Trial 1	7.9499	100g	107.9499	21.5	39.8	-41.597	exothermic
Trail 2	8.074	100g	108.074	21.5	41.0	-41.9	exothermic
Trial 3	7.577	100g	107.377	21.5	38.7	-42.2	exothermic
Average ∆Hrxn/mol=-41.90                          literature value=-44.3 % ERROR=5.4%
NaHCO3 Trail 1	8.8932	100g	107.9499	21.7	17.4	18.499	endothermic
Trail 2	8.057	100g	108.074	21.3	17.5	22.59	endothermic
Trail 3	8.323	100g	107.323	21.4	17.6	17.4	endothermic
Average ∆Hrxn/mol=+19.50                literature value=+16.7 ERROR=16.8%

1. Calculate the change in temperature T=T_final – _Tinitial
2. NH4NO₃

Trial 1

• 3-21.7=-5.4

Trial 2

• 4-21.2=-5.8

Trial 3

• 5-21.4=-5.9

1. CaCl₂

Trial 1

• 6-21.5=9.1

Trial 2

• 2-21.6=10.6

Trial 3

• 5-21.4=10.1

1. NaOH

Trial 1

• 8-21.5=18.3

Trial 2

• 2-21.6=10.6

Trial 3

• 5-21.4=10.1

1. NaHCO₃

Trial 1

• 4-21.7=-4.3

Trial 2

• 5-21.3=-3.8

Trial 3

• 6-21.4=-3.8

2. Percentage error

% error=100%

NH4NO₃

1.9%

CaCl₂

22%

NaOH

=5.4%

NaHCO₃

=16.8%

The table above shows the data obtained from the experiment. The first part shows the heat of the solution of water and NH4NO_3. This run had a temperature gain, which meant the reaction was endothermic. There was temperature loss in the heat of the solution of water and CaCl₂, implying an exothermic reaction. There was a temperature loss in the heat of the solution of water and NaOH, implying an exothermic. Lastly, there was a temperature gain in the heat of the solution of water and NaHCO₃, which meant an endothermic reaction. The percent error for the exothermic reaction was a large value because the temperature was reduced, and heat was lost. The percent error for the endothermic reaction was a small value because the temperature was raised, and the heat was gained.

Conclusions:

This experiment aimed to determine if the solution heat for several compounds was exothermic or endothermic. Each experimental setup was run for three different trials. From the experimental results, the reaction between water and NH4NO₃ was endothermic_, water and CaCl₂ were exothermic, water and NaOH were exothermic, and water and NaHCO₃ were endothermic. The experiment also aimed to determine the percentage error for each reaction. There was a considerable percent error for the three trials of the exothermic reactions, whereas there was a small percent error for the three trials of the endothermic reactions.

References:

Chen, D., Yang, H., Yi, Z., Xiong, H., Zhang, L., Zhu, S., & Cheng, G. (2018). C8N26H4: an environmentally friendly primary explosive with high heat of formation. Angewandte Chemie, 130(8), 210

Lozano, E. M., Pedersen, T. H., & Rosendahl, L. A. (2019). Modeling of thermochemically liquefied biomass products and heat of formation for process energy assessment. Applied Energy, 254, 113654.3-2106

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Lab Report

Heat of solution

This lab report must be done in Word; please include all data I have attached and follow the sample lab layout also attached. Please show all calculations and formulas and include graphs.