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<p>La reacción de hidrogenación del but-1,3-dieno para dar butano es:</p> <p><img width="205" height="30" title="C_4H_6(g) + 2\ H_2(g)\ \to\ C_4H_{10}(g)" style="font-size: 10pt; line-height: 1.5em; display: block; margin-left: auto; margin-right: auto;" alt="C_4H_6(g) + 2\ H_2(g)\ \to\ C_4H_{10}(g)" src="http://ejercicios-fyq.com/local/cache-vignettes/L287xH42/afa5ff009e9e4b5fc17727ec46191fc0-7bbb4.png" /></p> <p>C<span style="font-size: 10pt; line-height: 1.5em;">alcula la entalpía de la reacción a 25 ºC</span><span style="font-size: 10pt; line-height: 1.5em;">:</span></p> <p>a) A partir de la entalpía de formación del agua y de las entalpías de combustión del buta-1,3-dieno y del butano.</p> <p>b) A partir de las entalpías de enlace.</p> <p>Datos: ΔHº<sub>c</sub> (KJ/mol): (C<sub>4</sub>H<sub>6</sub> <sub>(g)</sub>)= -2540.2; C<sub>4</sub>H<sub>10 (g)</sub> = -2877.6 ; ΔHºf (H<sub>2</sub>O) =-285.6 KJ/mol ; </p> <p>Entalpías de enlace (kJ/mol): (C-C) = 348,2 ; (C=C) = 612,9 ; (C-H) = 415,3 ; (H-H) = 436,4.</p>
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16.66667%
14.28571%
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Monday, 6 August 2018, 3:27 PM
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