Experimento de fisicoquímica
Enviado por migamaster111 • 1 de Abril de 2020 • Informes • 837 Palabras (4 Páginas) • 93 Visitas
Experimento No.1: Calor de Disolución y Neutralización
Autor 1: Estefanía Rosero Rodríguez, Autor 2: Manuela Manrique Holguín
Universidad Tecnológica de Pereira
Correo-e: estefania.rosero@utp.edu.co , manuela.manrique@utp.edu.co
Abstract:
The heat of dissolution or enthalpy of dissolution (at constant pressure) ΔHsoln is the heat generated or absorbed when a certain amount of solute dissolves in a certain amount of solvent.
It is not possible to carry out this measurement, but in a constant pressure calorimeter the difference can be determined and therefore ΔHsoln. Like the other enthalpy changes, for exothermic processes the sign of ΔHsoln is negative (-), and for endothermic processes the sign is positive (+).
On the other hand, the heat of neutralization is understood as the heat generated when an acid reacts with a base to produce water; The process is neutralization comprises only the combination of hydrogen and hydroxyl ion to form non-ionized water.
Due to this, this experiment was carried out, we were able to acquire capabilities that allow us to determine the thermodynamic properties and their applications in different industries such as acid producing industries. This was achieved through the implementation of a dewar vessel for the identification of said properties.
Understanding and applying these thermodynamic properties allows us to obtain greater efficiency in industrial processes.
Keywords: dewar vessel, industry, thermodynamic properties.
CONTENIDO
- Datos experimentales
El laboratorio consistió en determinar el calor de disolución del ácido sulfúrico e hidróxido de sodio en agua, además que también se determinó el calor de neutralización entre ambos reactivos; para ello se determinó previamente la constante K del calorímetro con agua destilada.
[pic 1]
Figura 1. Montaje de laboratorio con vaso Dewar.
Los resultados obtenidos para cada proceso fueron los siguientes:
Tabla 1. Datos para la medida del equivalente en agua del calorímetro (K).
Temperatura inicial (°C) | 24 | ||
Temperaturas (°C) | Tiempo (s) | ||
Ensayo 1 | Ensayo 2 | Ensayo 3 | |
80,7 | 84,492 | 83,8 | 15 |
81,1 | 85,152 | 84,799 | 30 |
80,4 | 84,296 | 83,974 | 45 |
79,868 | 83,626 | 83,283 | 60 |
79,987 | 83,272 | 82,508 | 75 |
79,81 | 82,763 | 82,58 | 90 |
78,826 | 82,5 | 82,398 | 105 |
80,09 | 82,265 | 82,12 | 120 |
80,01 | 82,05 | 82,022 | 135 |
- | 81,887 | 81,93 | 150 |
- | 81,855 | 81,7 | 165 |
- | - | 81,512 | 180 |
- | - | 81,359 | 195 |
Por medio de los datos presentados en la tabla No.1 se calcula K, los resultados obtenidos se presentan en la tabla No.2:
[pic 2]
[pic 3]
[pic 4]
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Tabla 2. Valores de K.
K1 | 35,6722014 |
K2 | 28,1565984 |
K3 | 30,129535 |
K | 31,319449 |
Continuo a esto se realizan los cálculos del calor de disolución tanto del hidróxido de sodio como de ácido sulfúrico:
- Calor de disolución NaOH:
Tabla 3. Toma de datos NaOH.
T. Inicial | T. Inicial | Tiempo (s) |
25,64 | 24,643 | |
Ensayo 1 | Ensayo 2 | |
26,125 | 25,505 | 15 |
26,328 | 26,098 | 30 |
26,659 | 26,64 | 45 |
26,941 | 27,006 | 60 |
27,296 | 27,655 | 75 |
27,426 | 28,039 | 90 |
27,631 | 28,337 | 105 |
27,768 | 28,468 | 120 |
27,895 | 28,826 | 135 |
28,044 | 28,737 | 150 |
28,073 | 28,707 | 165 |
28,084 | 28,689 | 180 |
28,09 | 28,699 | 195 |
28,084 | 28,712 | 210 |
28,082 | 28,72 | 225 |
28,08 | 28,706 | 240 |
28,706 | 255 | |
28,7 | 270 |
...